Name: Measuring the Densities of Aqueous Glasses at Cryogenic Temperatures (Video) | JoVE Journal
Uploaded: 2017-06-28T14:00:00.000+00:00
Duration: 9 min 50 s
Description: Learn to measure vitreous phase densities of aqueous solutions at cryogenic temperatures using micro- to picoliter samples. This method enables rapid cooling and analysis of cryoprotected biological mixtures.

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5 minutes

This work was supported by the NSF under award MCB-1330685. DWM acknowledges partial support from Cornell University&#39;s Molecular Biophysics Training Grant (NIH T32GM0082567).

CAUTION: Please consult all relevant material safety data sheets (MSDS) before use. Please use all appropriate safety practices when using compressed gases, including appropriate calibrated gas handling regulators and valves, and approved gas tubing. Contact with liquid cryogens can cause  severe frostbite and necrosis. Use appropriate personal protective equipment (face shield, gloves, lab coat, full length pants, closed-toe shoes), all of which must be impermeable to liquid nitrogen. Remain standing and ensure an unobstructed exit path from the apparatus when using liquid cryogens. Be aware of asphyxiation hazards when using compressed gases and liquid cryogens, and work in a well-ventilated area with adequate make-up air (a fume hood or a high air turnover rate room.)
1. Preparation of Aqueous Solutions for Density Measurements
NOTE: Because weights are more easily measured to a high accuracy than volumes, solution concentrations are measured in w/w units. All densities and melting or boiling temperatures assume an atmospheric pressure of ~100 kPa. The following steps describe the preparation of a 35% w/w glycerol solution. The same procedure can be used for other concentrations and solutes.
<ol>
	<li>For each solute type and concentration of interest, roughly estimate the required solute mass to obtain the desired final concentration (e.g., between 25% w/w and 100% w/w) for a total solution volume, Vtot = 10 mL solution volume. For example, for a 35% w/w glycerol solution (ρs = 1.26 g/mL), the solute mass, ms is: 
	<img alt="Static equilibrium formula; equation shows mass calculation; xV_tot, ρ_s, ρ_w notation." src="/files/ftp_upload/55761/55761eq1.jpg" data-altupdatedat="1788250015000" data-alt="Equation"> 
	where x is the solute mass fraction (0.35) and ρw= 1 g/mL is the density of water.</li>
	<li>Place a 15 mL centrifuge tube (or other volume-calibrated water-impermeable container) on the pan of an analytical microbalance. Dispense the desired mass of solute/cryoprotectant (e.g., 3.77 g glycerol for a 35% w/w solution) into the tube, and record the actual solute mass.</li>
	<li>Add high purity (&gt;18 MΩ) deionized water to bring the total mass up to 10.0 g</li>
	<li>Vortex the container for 30 s (for liquid solutes) or 5 min (for solid solutes), until the solution is optically homogeneous.</li>
	<li>Measure and record the final mass of the solution. Seal the container with an airtight cap and store at constant temperature (293-298 K).</li>
</ol>
2. Preparation of the Sample Cooling Chamber
<ol>
	<li>Place the experimental apparatus described below in an enclosure and flow dry air (&gt;5% relative humidity (r.h.)) into the enclosure. 
	NOTE: The enclosure may be a simple metal frame with its top and three sides sealed with clear plastic sheet and with experiment access via a fourth side covered with flexible plastic sheet. Wear face shields and full body covering to minimize moisture introduced by the experimenter. Moisture condensation and ice formation can interfere with cryogenic temperature density measurements in several ways, and so it must be minimized.</li>
	<li>Place a disk of neoprene rubber on the bottom of a 4.5 L glass Dewar flask, to protect the Dewar flask from damage.</li>
	<li>Carefully insert a high thermal conductivity copper chamber (a hollow cylinder with a sealed bottom) into the flask until it rests on the rubber disk. Adjust struts projecting outward from the chamber to the Dewar walls so that the chamber is centered and has no tendency to rock. 
	NOTE: The Dewar flask will hold liquid nitrogen, and the much smaller volume copper chamber will hold a liquid N2-Ar mixture. The liquid nitrogen provides a thermal bath that maintains the copper chamber and its contents at a constant temperature of 77 K and reduces boiling and evaporative losses in the chamber. The chamber's small diameter suppresses surface waves that can interfere with buoyancy measurements, and helps isolate the liquid within the chamber from frost and ice formed elsewhere in the apparatus.</li>
	<li>Insert the outlet of a gas tube with dry N2 gas flowing at ~2 L/min down to the bottom of the copper chamber, and purge the chamber of moist air.</li>
	<li>Slowly pour liquid nitrogen into the Dewar flask, outside the copper chamber, allowing time for nitrogen boil-off. 
	NOTE: The final fill level, after boiling has ceased, should be within approximately 4 cm of the top of the copper chamber.</li>
	<li>Cover the outer portion of the Dewar flask with an annular foam insulating lid. Remove the dry N2 gas purge tube from the copper chamber and insert into a matching opening in the lid. 
	NOTE: The combination of N2 gas from boil-off in the Dewar flask and from the purge flow expels any moist air and prevents it from condensing and crystalizing on cold surfaces.</li>
	<li>Slowly pour liquid nitrogen into the copper chamber. The final fill level, after boiling has ceased, should be within approximately 4 cm of the top of the copper chamber.</li>
	<li>Place a thin, optically transparent plastic sheet over the central opening or vent in the lid, and reduce the N2 gas flow rate to ~0.2 L/min, leaving a slight overpressure of N2 gas within the gas spaces above the cryogenic liquids. 
	NOTE: As long as cryogenic liquids are present in the Dewar and chamber, continue adjusting the N2 gas flow as needed to maintain this overpressure and prevent moisture from entering into the Dewar and forming ice.</li>
</ol>
3. Determination of the Volume and Density of the Test Mass at T = 298 K and T = 77 K
<ol>
	<li>Determine the apparent mass of a ~1 g, ~0.4 mL PTFE test mass (Table of Materials) in air at T= 298 K by placing it on the pan of a calibrated analytical microbalance.</li>
	<li>Determine the volume V(298 K) of the test mass at T = 298 K using a gas pycnometer, or by dimensional measurements using calipers. If using dimensional measurements, the test mass must have a simple, precise shape (no tapers or rounded corners) and the volume of the through-hole (for the suspending line) should be determined.</li>
	<li>Calculate the mass m of the test mass by correcting the measured apparent mass for the buoyant force exerted by air according to the following: 
	<img alt="Mass calculation formula, m = m_app in air + ρ_airV(298K), thermodynamics concept." src="/files/ftp_upload/55761/55761eq2.jpg" data-altupdatedat="1788250015000" data-alt="Equation"> 
	where ρair = 1.23 g/L (~0.1% correction).</li>
	<li>Place the microbalance on a stable platform roughly 10 cm above the Dewar flask and verify its calibration. Suspend the test mass using a 2 mil (50 μm) monofilament line strung from the hook on the underside of the microbalance (designed for hanging mass measurements) and through a hole in the test mass. Determine the apparent mass in air, and compare with the measurement in step 3.3, correcting as needed for the mass of the line.</li>
	<li>Determine the volume V(77 K) of the test mass at T = 77 K by measuring its apparent mass in pure liquid nitrogen, mapp in LN2. Lower the test mass into the liquid nitrogen within the copper chamber until it is fully submerged. When boiling has ceased, measure the apparent mass. 
	NOTE: If the liquid nitrogen in the copper chamber is quiescent and air currents between the microbalance and the liquid surface are minimal, this mass can be measured to greater than ± 0.0002 g accuracy.</li>
	<li>Estimate the buoyant force on the submerged portion of the line, and verify that it is small compared with measurement errors.</li>
	<li>Calculate the volume and density of the test mass at 77 K using its known mass m and the measured apparent mass in LN2 at 77 K, mapp in LN2, according to the following: 
	<img alt="Equation for volume calculation at 77K using apparent mass in liquid nitrogen; scientific formula." src="/files/ftp_upload/55761/55761eq3.jpg" data-altupdatedat="1788250015000" data-alt="Equation"> 
	where ρLN2((77 K)=0.807 g/mL.</li>
</ol>
4. Preparation of the Initial Liquid N2-Ar Mixture
<ol>
	<li>Flow Ar gas at a flow rate of ~2 L/min through a coiled tube to its outlet. Place the coiled tube on top of the upper struts that stabilize the position of the copper chamber, just above the liquid nitrogen level and below the top surface of the Dewar. Cold N2 and Ar gas will build up above the cryogenic liquids, and thermal conduction, convection, and radiation will cool the tubing and the Ar gas within.</li>
	<li>After allowing the coiled tube to cool for 5 min, place the outlet of the tube in the copper chamber, at least 10 cm below the surface of the liquid nitrogen. Then cover the Dewar with the annular lid and transparent sheet.</li>
	<li>Adjust the Ar flow rate until Ar bubbles rise from the tube outlet to the top surface of the liquid nitrogen. Then reduce the flow rate until the bubbles form at the outlet but dissolve or liquefy just before breaking the liquid nitrogen surface. 
	NOTE: As the Ar concentration in the copper chamber increases, periodically adjust the Ar flow rate as needed to maintain bubble formation. If the Ar flow rate is too low, the Ar may freeze inside the tube and block the flow.</li>
	<li>Add liquid nitrogen as needed to maintain its level in the surrounding Dewar. Remove ice as it accumulates on cold surfaces.</li>
	<li>Periodically mix the liquid by inserting a thin (e.g., 35 micron), circular sheet of copper foil attached to a thin insulating rod into the copper chamber, and slowly moving it up and down like a piston. This will reduce concentration gradients and the tendency for Ar to crystallize out of the solution.</li>
</ol>
5. Measuring and Adjusting the Density of the Initial N2-Ar Mixture
<ol>
	<li>Calculate the target density for the N2-Ar mixture by estimating the T =77 K density of the sample to be measured, e.g., measurements at higher concentrations of the sample's non-aqueous component.</li>
	<li>Attach the test mass using the monofilament line to the hook on the underside of the microbalance measuring pan, measure its apparent mass in air, and confirm agreement with the measurement in step 3.1.</li>
	<li>Mix the N2-Ar solution to eliminate concentration and density gradients as in step 4.5.</li>
	<li>Precool the test mass to T = 77 K by lowering it into the liquid nitrogen outside the copper chamber. Raise the test mass into the cold layer of nitrogen gas above the liquid nitrogen, wait for residual liquid nitrogen to evaporate off the test mass, and then lower the cold, dry test mass into the N2-Ar mixture until it is fully submerged and within 2 cm of the liquid surface.</li>
	<li>After any boiling and surface waves have disappeared, measure the apparent mass of the test mass. Calculate the solution density using its true mass m and T = 77 K volume V(77K) from step 3.7 according to the following: 
	<img alt="Cryogen density equation; formula; used for density calculation at 77K; scientific analysis." src="/files/ftp_upload/55761/55761eq4.jpg" data-altupdatedat="1788250015000" data-alt="Equation"></li>
	<li>Increase the solution density by flowing additional Ar until the desired initial density is obtained. Sample drops that sink can easily be lost, so the initial density should be at least a few percent higher than the expected sample density. The sample will then float, making it easier to keep track of it, and the N2-Ar mixture density will then only need to be adjusted downward by adding liquid N2.</li>
	<li>Remove the Ar precooling coiled tube and allow to warm and dry before next use.</li>
</ol>
6. Cooling Drops of Sample Solution
<ol>
	<li>Immediately prior to drop dispensing and cooling, repeat step 1.5 to mix the nitrogen/argon cryogenic liquid. Be careful not to introduce any bubbles.</li>
	<li>Remove the sample tube's airtight cap. Using a clean 1 mL syringe, extract up to 1 mL of solution, and replace the cap. Attach a 27 to 33 G needle onto the syringe, and then push a small amount of sample through the needle to expel air and any residues from previous dispensing.</li>
	<li>Two methods may be used to project sample drops into the N2-Ar mixture.
	<ol>
		<li>For samples with large non-aqueous component concentrations (&gt;45% w/w) that can be vitrified with modest cooling rates, lightly press the syringe to displace a small (250 μm to 1 mm) diameter, ~10 nL to 1 μL drop that hangs from the needle tip by surface tension. Gently tap the needle to detach and project the drop toward the liquid N2-Ar mixture.</li>
		<li>For samples that require faster cooling for vitrification, place the outlet of a gas tube connected to a vacuum generator (supplied by lab compressed air) in the gas space above the liquid N2-Ar mixture, and gently suction away the cold gas layer that forms. This increases cooling rates for small samples11.
		<ol>
			<li>Carefully touch the needle tip to a 25-75 μm thick clear polymer strip to dispense a small volume (&lt;10 nL, corresponding to a drop diameter &lt;200 μm) of sample. 
			NOTE: To obtain the smallest, most nearly spherical, and most easily removed drops, soak the strip in a hydrophobic coating solution for 10 min and let dry prior to sample dispensing.</li>
			<li>Grab the strip using an attached plastic or wood rod, and manually plunge the rod plus the strip into the liquid N2-Ar mixture.</li>
			<li>Once the drop has solidified and boiling has ceased, grab the strip edge opposite the rod using tweezers. Flex the strip, keeping it immersed in the liquid N2-Ar, until the sample drop pops off and floats to the surface.</li>
		</ol>
		</li>
	</ol>
	</li>
</ol>
7. Assessment of the State of the Sample
<ol>
	<li>Using a long working distance (5-10 cm) binocular microscope and bright, cool illumination from an LED or fiber optic illuminator, carefully examine the drop while keeping it immersed in the liquid N2-Ar. Vitrified drops should appear clear12,13. Reject drops that are hazy or cloudy (likely containing more than one phase) and/or that show optical imperfections including cracks (which may be associated with voids that change the average density). 
	NOTE: Painting the inside surface of the copper chamber to provide a black background can facilitate the identification of sample imperfections.</li>
</ol>
8. Determination of the Density of the Sample
<ol>
	<li>The dispensed drop will initially float, sink, or (rarely) be neutrally buoyant in the N2-Ar mixture. Floating drops may sometimes be held up by surface tension, tiny bubbles, or adhered ice particles. Inspect the entire drop surface with the microscope. Displace the drop downward from the liquid surface using a small (2-3 mm diameter, 10 cm long) precooled plastic or wood rod and observe its response.</li>
	<li>If the drop sinks, increase the density of the liquid N2-Ar using the procedure in step 4 until the drop becomes neutrally buoyant or floats.</li>
	<li>If the drop floats, decrease the density of the liquid N2-Ar by adding liquid nitrogen using a 1.8 mL cryovial. At large initial mixture densities (1.2-1.3 g/mL), adding N2 in 1 mL increments gives appreciable density changes, but this should be increased toward 5 mL at low densities (0.8-0.9 g/mL). Gently mix the N2-Ar (so as not to lose track of the sample drop) using the thin perforated copper foil sheet up-and-down in the copper chamber.</li>
	<li>After each N2 addition, use a small pre-cooled rod to gently displace the floating drop downward into the liquid, and observe its speed as it returns to the surface.</li>
	<li>When the solution density has been adjusted so that the drop appears to be neutrally buoyant or ascends very slowly (&lt;50 μm/s will ensure ~0.1% or better density accuracy for drops with volumes down to 50 pL), measure the N2-Ar mixture density as described in step 5. Then add additional liquid N2 until the drop first begins to slowly sink, and measure the N2-Ar mixture density again. These two measurements will provide bounds on the drop density.</li>
</ol>

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<li>Nagy, Z. P., Nel-Themaat, L., Chang, C. -C., Shapiro, D. B., Berna, D. P. <a target="_blank" href="https://www.ncbi.nlm.nih.gov/pubmed/24782022">Cryopreservation of eggs.</a> Human Fertility: Methods and Protocols. , 439-454 (2014).</li>
<li>Kriminski, S., Caylor, C. L., Nonato, M. C., Finkelstein, K. D., Thorne, R. E. <a target="_blank" href="http://www.ncbi.nlm.nih.gov/pubmed?term=((Flash+cooling+and+annealing+of+protein+crystals%5BTitle%5D)+AND+%22Acta+Cryst+Sect+D%22%5BJournal%5D)">Flash cooling and annealing of protein crystals.</a> Acta Cryst Sect D. 58 (3), 459-471 (2002).</li>
<li>Juers, D. H., Matthews, B. W. <a target="_blank" href="http://www.ncbi.nlm.nih.gov/pubmed?term=((Reversible+lattice+repacking+illustrates+the+temperature+dependence+of+macromolecular+interactions%5BTitle%5D)+AND+%22J+Mol+Biol%22%5BJournal%5D)">Reversible lattice repacking illustrates the temperature dependence of macromolecular interactions.</a> J Mol Biol. 311 (4), 851-862 (2001).</li>
<li>Juers, D. H., Matthews, B. W. <a target="_blank" href="http://www.ncbi.nlm.nih.gov/pubmed?term=((Cryo-cooling+in+macromolecular+crystallography%3A+advantages%2C+disadvantages+and+optimization%5BTitle%5D)+AND+%22Q+Rev+Biophys%22%5BJournal%5D)">Cryo-cooling in macromolecular crystallography: advantages, disadvantages and optimization.</a> Q Rev Biophys. 37 (2), 105-119 (2004).</li>
<li>Alcorn, T., Juers, D. H. <a target="_blank" href="http://www.ncbi.nlm.nih.gov/pubmed?term=((Progress+in+rational+methods+of+cryoprotection+in+macromolecular+crystallography%5BTitle%5D)+AND+%22Acta+Cryst+Sect+D%22%5BJournal%5D)">Progress in rational methods of cryoprotection in macromolecular crystallography.</a> Acta Cryst Sect D. 66 (4), 366-373 (2010).</li>
<li>Warkentin, M., Sethna, J., Thorne, R. <a target="_blank" href="http://www.ncbi.nlm.nih.gov/pubmed?term=((Critical+Droplet+Theory+Explains+the+Glass+Formability+of+Aqueous+Solutions%5BTitle%5D)+AND+%22Phys+Rev+Lett%22%5BJournal%5D)">Critical Droplet Theory Explains the Glass Formability of Aqueous Solutions.</a> Phys Rev Lett. 110 (1), 15703(2013).</li>
<li>Kriminski, S., Kazmierczak, M., Thorne, R. E. <a target="_blank" href="http://www.ncbi.nlm.nih.gov/pubmed?term=((Heat+transfer+from+protein+crystals%3A+implications+for+flash-cooling+and+X-ray+beam+heating%5BTitle%5D)+AND+%22Acta+Cryst+Sect+D%22%5BJournal%5D)">Heat transfer from protein crystals: implications for flash-cooling and X-ray beam heating.</a> Acta Cryst Sect D. 59 (4), 697-708 (2003).</li>
<li>Loerting, T., Bauer, M., Kohl, I., Watschinger, K., Winkel, K., Mayer, E. <a target="_blank" href="http://www.ncbi.nlm.nih.gov/pubmed?term=((Cryoflotation%3A+Densities+of+amorphous+and+crystalline+ices%5BTitle%5D)+AND+%22J+Phys+Chem+B%22%5BJournal%5D)">Cryoflotation: Densities of amorphous and crystalline ices.</a> J Phys Chem B. 115 (48), 14167-14175 (2011).</li>
<li>Shen, C., Julius, E. F., Tyree, T. J., Moreau, D. W., Thorne, R. E. <a target="_blank" href="http://www.ncbi.nlm.nih.gov/pubmed?term=((Thermal+contraction+of+aqueous+glycerol+and+ethylene+glycol+solutions+for+optimized+protein-crystal+cryoprotection+Thermal+contraction+of+aqueous+glycerol+and+ethylene+glycol+solutions+for+optimized+protein-crystal+cryoprotection%5BTitle%5D)+AND+%22Acta+Cryst+Sect+D%22%5BJournal%5D)">Thermal contraction of aqueous glycerol and ethylene glycol solutions for optimized protein-crystal cryoprotection Thermal contraction of aqueous glycerol and ethylene glycol solutions for optimized protein-crystal cryoprotection.</a> Acta Cryst Sect D. 72 (6), 742-752 (2016).</li>
<li>Warkentin, M., Berejnov, V., Husseini, N. S., Thorne, R. E. <a target="_blank" href="http://www.ncbi.nlm.nih.gov/pubmed?term=((Hyperquenching+for+protein+cryocrystallography%5BTitle%5D)+AND+%22J+Appl+Cryst%22%5BJournal%5D)">Hyperquenching for protein cryocrystallography.</a> J Appl Cryst. 39 (6), 805-811 (2006).</li>
<li>McFerrin, M. B., Snell, E. H. <a target="_blank" href="http://scripts.iucr.org/cgi-bin/paper?S0021889802009238">The development and application of a method to quantify the quality of cryoprotectant solutions using standard area-detector X-ray images.</a> J Appl Cryst. 35 (5), 538-545 (2002).</li>
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<li>Bosart, L. W., Snoddy, A. O. <a target="_blank" href="http://pubs.acs.org/doi/abs/10.1021/ie50228a032">Specific gravity of glycerol.</a> Ind Eng Chem. 20 (12), 1377-1379 (1928).</li>
<li>Rodrigues, M., Francesconi, A. Z. <a target="_blank" href="https://link.springer.com/article/10.1007/s10953-011-9756-5">Experimental study of the excess molar volumes of binary and ternary mixtures containing water + (1,2-ethanediol, or 1,2-propanediol, or 1,3-propanediol, or 1,2-butanediol) + (1-n-butyl-3-methylimidazolium bromide) at 298.15 K and atmospheric pressure.</a> J Solution Chem. 40 (11), 1863-1873 (2011).</li>
<li>Berejnov, V., Husseini, N. S., Alsaied, O. A., Thorne, R. E. <a target="_blank" href="http://scripts.iucr.org/cgi-bin/paper?do5023">Effects of cryoprotectant concentration and cooling rate on vitrification of aqueous solutions.</a> J Appl Cryst. 39 (2), 244-251 (2006).</li>
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</ol>

The authors have nothing to disclose.

The present apparatus and methods, developed primarily by undergraduates with limited access to instrument-building tools and machinery, nevertheless delivers highly accurate density measurements for individual liquid drops as small as 50 pL. In the concentration range near and above 50% w/w, where small cooling rates are sufficient to obtain vitrified samples, the densities agree with those obtained in previous measurements on bulk samples. Extrapolations of the present densities to 0% concentration – pure water – also ...

The physical properties of water and aqueous mixtures in their various phases are of fundamental interest, and are important to in vivo and in vitro understanding of biological systems. In contemporary cryobiology and biological cryopreservation, the vitreous or amorphous phases of aqueous cryoprotectant mixtures are of particular interest1,2. Nucleation and growth of ice crystals can disrupt cells and tissues, and promote protein denaturation and aggregation, so cryopreservation protocols that vitrify the solvent have become increasingly popular. In biomolecular crystallography, the crystallization of solvent in the channels between biomolecules disrupts crystal lattices and degrades diffraction properties. Vitrification is achieved through a combination of rapid cooling, dehydration, and addition of cryoprotective solutes such as glycerol, ethylene glycol, polyethylene glycols (PEGs), alcohols, and salts.
Vitrification limits ice crystallization and growth, but does not eliminate all cooling-related sample damage. For example, crystal mosaicity (a measure of the distribution of crystal plane orientations) routinely increases by a factor of 10 to 100 when protein crystals are cooled into a vitrified state3, and post-thaw survival rates of vitrified sperm cells and oocytes vary widely.
One damage mechanism is differential contraction of solvent and surrounding material during cooling3,4,5. The equilibrium solvent and solute concentrations within a crystal, cell or tissue are temperature dependent, and the solvent plus the solute and surrounding material may contract by different amounts. Rapid cooling may prevent solvent and solute redistribution prior to vitrification, and differential contraction may lead to large, inhomogeneous, nonequilibrium stresses that cause sample damage.
Rational approaches to reducing cooling-induced damage could thus benefit from the knowledge of temperature-dependent densities of liquid and vitrified aqueous mixtures. At solute concentrations above 50% weight of solute to weight of solution (w/w), most aqueous cryoprotectant mixtures can be vitrified with modest cooling rates of 10 K/s or less, allowing production of and density measurements using large vitreous samples6. Density can then be determined using Archimedes&#39; principle, by measuring the apparent weight of the sample when suspended in a liquid cryogen like nitrogen. However, as solute concentration decreases, cooling rates required for vitrification increase rapidly: Cooling rates for aqueous glycerol mixtures increase from &#60;10 K/s at 50% weight of solute in g to volume of solution in mL (w/v) to &#62;1,000 K/s at 25% w/v7. Heat transfer becomes boundary-layer limited, so that achieving larger cooling rates requires smaller and smaller samples8.
Measurements of the density of pure vitreous water and ice have been achieved by depositing micrometer-diameter (femtoliter volume) drops in a vacuum onto a cryogenically-cooled surface so as to build up a macroscopic (gram mass) sample. The density of this sample was determined by cryoflotation in a liquid nitrogen-argon mixture, in which the density of the cryogenic liquid was adjusted until the sample became neutrally buoyant9. However, generating large samples from a large number of small drops in a way that minimizes void volumes &#8211; an important source of error in previous vitreous phase density measurements &#8211; is non-trivial. For aqueous mixtures, differential evaporation of solution components during aerosolization and deposition in a vacuum can lead to substantial uncertainties in deposited concentrations.
We have developed a method, based on cryoflotation, that allows accurate density determination of aqueous mixtures using individual drops as small as 50 pL10. These drops can be rapidly cooled while retaining their original concentrations, and their cryogenic temperature state (vitrified or crystalline) can be assessed using a simple visual assay that correlates with X-ray diffraction measurements. This method is broadly applicable to aqueous and non-aqueous mixtures, and can be extended to a variety of biological samples including cells (e.g., stem and egg), tissue samples, and protein crystals having low-temperature densities between 0.8 and 1.4 g/mL.

<table><tbody><tr><td>centrifuge tube</td><td>Falcon</td><td>6029236</td><td>15 mL conical centrifuge tube</td></tr><tr><td>glycerol, &gt;99.5%</td><td>Sigma&amp;nbsp;</td><td>G9012-100 mL</td><td></td></tr><tr><td>ethylene glycol, &gt;99.8%</td><td>Sigma</td><td>324558-100 mL</td><td></td></tr><tr><td>analytical microbalance</td><td>Mettler</td><td>AE240</td><td>Analytical balance, 0.01 mg resolution, has hook on bottom for weighing below the balance&amp;nbsp;</td></tr><tr><td>vortexer</td><td>Scientific Industries</td><td>SI-0236</td><td>Vortex-Genie 2</td></tr><tr><td>Apparatus enclosure framing</td><td>Unistrut&amp;nbsp;</td><td>1-5/8&quot; metal framing</td><td>48&quot; wide x 24&quot; deep x 40&quot; tall&amp;nbsp;</td></tr><tr><td>Apparatus enclosure air barrier</td><td></td><td></td><td>any clear plastic sheeting</td></tr><tr><td>neoprene rubber disk</td><td></td><td></td><td>4&quot; diameter, 1/8&quot; thick</td></tr><tr><td>dewar flask</td><td>Scilogix Dilvac</td><td>SS333</td><td>4.5 liter dewar flask with steel case and clamp lid</td></tr><tr><td>copper chamber</td><td></td><td></td><td>This fabricated part is comprised of a 1.43&quot; diameter, 0.017&quot; wall thickness copper tube with a solid cylindrical copper base soldered to seal one end.&amp;nbsp; The copper base is 0.87&quot; tall and the overall chamber height is 7&quot;.</td></tr><tr><td>nitrogen gas</td><td>Airgas</td><td>NI HP300</td><td>99.998% pure N2 gas</td></tr><tr><td>argon gas</td><td>Airgas</td><td>AR HP300</td><td>99.998% pure Ar gas</td></tr><tr><td>rotameter</td><td>Omega</td><td>FL3692ST</td><td>2.52 L/min max flow rate</td></tr><tr><td>foam insulating lid</td><td></td><td></td><td>This part is fabricated from 4 lb/ft&lt;sup&gt;3&lt;/sup&gt; crosslinked polyethylene foam (supplied by Technifab, 1355 Chester Industrial Parkway, Avon, OH), and has an OD of 2.42&quot;, and ID of 1.52&quot;, and a thickness of 0.79&quot;.&amp;nbsp;&amp;nbsp;&amp;nbsp;&amp;nbsp;</td></tr><tr><td>PTFE test mass</td><td></td><td></td><td>This fabricated part is a 0.246&quot; diameter, 0.580&quot; tall cylinder with a 0.060&quot; diameter hole running perpendicular to and intersecting the cylinder axis ~0.10&quot; from one end.&amp;nbsp;</td></tr><tr><td>microbalance platform</td><td>Unistrut</td><td>1-5/8&quot; metal framing</td><td>11&quot; wide x 24&quot; long x 24&quot; high rectangular frame with an top aluminum sheet containing a hole for the monofilament and hanging test mass</td></tr><tr><td>2 mil (50 um) monofilament line</td><td>Berkley</td><td>NF1502-CM</td><td>Nanofil fishing line</td></tr><tr><td>Argon precooling coil tubing</td><td>VWR</td><td>60985-512</td><td>1/8&quot; ID x 1/4&quot; OD PVC tubing</td></tr><tr><td>perforated copper foil mixer</td><td></td><td></td><td>1.4&quot; diameter,&amp;nbsp; 35 micron thick copper disk, cut from 1 ounce/ft&lt;sup&gt;2&lt;/sup&gt; copper sheet and perforated with holes using an awl or other sharp pointed tool.&amp;nbsp; Insert 1-2 mm diameter rigid thermally insulating (plastic or wood) rod into the center and fix using epoxy as needed.</td></tr><tr><td>syringe</td><td>BD</td><td>309628</td><td>1 mL Luer-Lok tip syringe</td></tr><tr><td>vacuum generator</td><td>Gast</td><td>VG-015-00-00</td><td>compressed air venturi single stage vacuum generator</td></tr><tr><td>hydrophobic coating spray</td><td>RainX</td><td>620036</td><td>plastic water repellent</td></tr><tr><td>long focal length stereo microscope</td><td>Bausch and Lomb Stereozoom 6</td><td></td><td>0.67-4 x zoom pod with 20X eyepieces, 10 cm working distance&amp;nbsp;</td></tr><tr><td>LED ring illuminator</td><td>Amscope</td><td>LED144S</td><td></td></tr><tr><td>LED spot illuminator</td><td>Newhouse Lighting</td><td>NHCLP-LED</td><td>3W LED gooseneck clamp lamp</td></tr><tr><td>1.8 ml cryo vial</td><td>Nunc</td><td>V7634-500EA</td><td>Any 1.8 or 2 mL cryovial is adequate</td></tr></tbody></table>

measuring the densities of aqueous glasses at cryogenic temperatures

Measuring the Densities of Aqueous Glasses at Cryogenic Temperatures

We demonstrate a method for determining the vitreous phase cryogenic temperature densities of aqueous mixtures, and other samples that require rapid cooling, to prepare the desired cryogenic temperature phase. Microliter to picoliter size drops are cooled by projection into a liquid nitrogen-argon (N2-Ar) mixture. The cryogenic temperature phase of the drop is evaluated using a visual assay that correlates with X-ray diffraction measurements. The density of the liquid N2-Ar mixture is adjusted by adding N2 or Ar until the drop becomes neutrally buoyant. The density of this mixture and thus of the drop is determined using a test mass and Archimedes principle. With appropriate care in drop preparation, management of gas above the liquid cryogen mixture to minimize icing, and regular mixing of the cryogenic mixture to prevent density stratification and phase separation, densities accurate to &#60;0.5% of drops as small as 50 pL can readily be determined. Measurements on aqueous cryoprotectant mixtures provide insight into cryoprotectant action, and provide quantitative data to facilitate thermal contraction matching in biological cryopreservation.

Density measurements at T = 77 K for vitrified drops of aqueous glycerol and ethylene glycol versus cryoprotectant concentration are shown in Figure 1A and Figure 1B respectively, and the corresponding change in specific volume between T = 298 K and 77 K, calculated using previously determined T = 298 K densities, is shown in Figure 2. At h...

A protocol for determining the vitreous phase densities of micro- to pico-liter size drops of aqueous mixtures at cryogenic temperatures is described.

We demonstrate a method for determining the vitreous phase cryogenic temperature densities of aqueous mixtures, and other samples that require rapid ...

The overall goal of this experiment is to determine the glass or vitreous state densities of aqueous solutions at cryogenic temperatures. This method can help answer key questions in the fields of Cryobiology and Cryocrystallography, such as, how much do aqueous cryo protected mixtures contract or expand when cooled into a vitreous state at cryogenic temperatures. The main advantage of this technique is that both cryogenic temperature sample density and phase, can be determined using small samples that can be cooled rapidly.Though this method was developed for cryoprotecting solutions, it can also be used to determine cryogenic temperature densities of tissues, cell aggregates and other biological samples. I first had the idea for this method when I learned from Thomas Lutin, how to make a cryogenic liquid with a tunable density and the range between 0.9 and 1.3 grams per milliliter. To begin this procedure, place a disk of neoprene rubber on the bottom of a 4.5 liter glass dewar flask, to protect the dewar flask from damage.Carefully insert a high thermal conductivity copper chamber into the flask, until it rests on the rubber disk. Adjust struts projecting outward from the chamber to the dewar flask walls, so that the chamber centered and has no tendency to rock. Insert the outlet of a gas tube with dry nitrogen gas flowing at approximately two liters per minute, down to the bottom of the copper chamber and purge the chamber of moist air.Now, slowly pour liquid nitrogen into the dewar flask, outside the copper chamber, allowing time for nitrogen boil off. Remove the dry nitrogen gas tube from the copper chamber and insert it into a matching opening in a foam insulating lid. Then cover the outer portion of the dewar flask with the lid.Secure the lid in place with elastic straps. Slowly pour liquid nitrogen into the copper chamber, so that the final fill level after boiling has ceased, is within approximately five centimeters of the top of the copper chamber. Following this, place a thin optically transparent plastic sheet over the central opening in the lid.Reduce the nitrogen gas flow rate to approximately 0.2 liters per minute, leaving a slight overpressure of nitrogen gas within the gas spaces above the cryogenic liquids. Determine the apparent mass of a one gram 0.4 milliliter PTFE test mass, in the air, at 298 Kelvin, by placing it on the pan of a calibrated analytical micro balance. Next, suspend the test mass using a 50 micron monofilament line strung from the hook on the underside of the micro balance and through a hole in the test mass.Then, determine the apparent mass in air and compare to the mass measurement, correcting as needed for the mass of the line. To determine the volume of the test mass at 77 Kelvin, lower the test mass into the copper chamber containing liquid nitrogen until it is fully submerged. When boiling has ceased, measure the apparent mass.Flow Argon gas at a flow rate of approximately two liters per minute through a coiled tube to its outlet. Place the coiled tube on top of the upper struts that stabilize the position of the copper chamber, just above the liquid nitrogen level and below top surface in the dewar flask. After allowing the coiled tube to cool for five minutes, place the outlet and the tube in the copper chamber at least 10 centimeters below the surface and the liquid nitrogen.Then, cover the dewar flask with the annular lid and transparent sheet. Following this, adjust the Argon flow rate until bubbles rise from the tube outlet to the top surface of the liquid nitrogen. Then, reduce the flow rate until the bubbles form at the outlet but dissolve or liquefy just before breaking the liquid nitrogen surface.Periodically, mix the liquid by inserting a thin circular sheet of copper foil attached to a thin insulating rod into the copper chamber and slowly moving it up and down like a piston. After measuring the apparent mass of the test mass in air, remove the insulating dewar cover and cool the mass to 77 Kelvin by lowering it into the liquid nitrogen outside the copper chamber. Raise the cool test mass into the cold layer of nitrogen gas above the liquid nitrogen and wait for residual liquid nitrogen to evaporate off the test mass.Then, lower the cool, dried test mass into the liquid nitrogen Argon mixture until it is fully submerged and within two centimeters of the liquid surface. After any boiling and surface waves have disappeared, measure the apparent mass of the test mass. Immediately prior to drop dispensing in cooling, mix the nitrogen argon cryogenic liquid, as previously described.After removing the sample tubes cap, extract up to one milliliter solution using a clean one milliliter syringe. Attach a 27 to 33 gauge needle onto the syringe and then push a small amount of sample through the needle to expel air and any residues from previous dispensing. For samples that require faster cooling for vitrification, place the outlet of a gas tube connected to a vacuum generator, in the gas space above the liquid nitrogen argon mixture and gently suction away the cold gas layer that forms.For samples with large non-aqueous component concentrations that can be vitrified with modest cooling rates, lightly press the syringe to displace a small diameter, 10 nanoliter to one microliter drop that hangs from the needle tip by surface tension. Gently tap the needle to detach and project the drop towards the liquid nitrogen argon mixture. Using a long working distance binocular microscope, and bright, cool illumination from an LED illuminator, carefully examine the drop while keeping it immersed in the liquid nitrogen argon mixture.Vitrified drops should appear clear. Reject drops are cloudy or show an optical imperfections including cracks. The drop floats, decrease the density of the liquid nitrogen argon mixture by adding liquid nitrogen using a 1.8 milliliter cryo vial.Gently mix the liquid nitrogen argon mixture, using a thin perforated copper foil sheet and moving it up and down in the copper chamber. After each liquid nitrogen addition, move a small prequel rod beneath the floating drop to gently displace it downward into the liquid and observe its speed as it returns to the surface. Density measurements at 77 Kelvin for vitrified drops of aqueous glycerol and ethylene glycol, versus cryo protecting concentration, are shown here.The corresponding change in specific body in between 298 and 77 Kelvin, calculated using previously determined 298 Kelvin densities is displayed here. Near 20%to 25%solutions of both cryo protectants are predicted to show no net expansion or contraction. The slope of the volume change versus concentration has the largest magnitude below 40%where the effects of additional cryo protectant on waters, tetrahedral low temperature structure are most pronounced.Once mastered, the initial high density liquid nitrogen argon cryogenic solution can be prepared in two to two and a half hours and the densities of individual drops can be determined in 10 to 15 minutes. While attempting this procedure, it's important to remember to watch for icing and remove as much of the cold gas layer that forms on the liquid nitrogen argon mixture surface as possible, using a vacuum generator. Following this procedure, drops can be collected, stored in liquid nitrogen and later measured using cryocrystallography to verify the phase of a drop.Don't forget, that working with liquid cryogens can be extremely hazardous and precautions such as, wearing appropriate gloves, face shields, clothing and footwear, should always be taken while performing this procedure.

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Learn to measure vitreous phase densities of aqueous solutions at cryogenic temperatures using micro- to picoliter samples. This method enables rapid cooling and analysis of cryoprotected biological mixtures.

Measuring the Densities of Aqueous Glasses at Cryogenic Temperatures

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