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Q1: What are the main components of a solution?
A solution consists of a solute, the substance being dissolved, and a solvent, the bulk liquid in which it dissolves. Together, these form a homogenous mixture. Solutions are characterized by their solute concentration, which measures how much solute is present per unit of solution. Understanding these components is essential for accurate solution preparation in laboratory work.
Q2: Why is purified water essential when making aqueous solutions?
Purified water must be used instead of tap water because tap water contains impurities that can compromise solution quality and affect experimental results. Using tap water in aqueous solutions can potentially damage multiple experiments downstream. A graduated cylinder should measure roughly three-quarters of the final solution volume in purified water before adding solutes to ensure proper preparation.
Q3: How do you calculate the amount of solute needed for a solution?
First, determine the moles of solute required to achieve your desired concentration in a given volume. Convert this value to grams using the molecular weight, which represents grams per mole of the chemical. Weigh the solute using a digital balance and weigh boat. Understanding concentration and measuring volumes accurately ensures reproducible results across experiments.
Q4: What does QS'ing a solution mean and why is it important?
QS'ing refers to adding quantity sufficient to reach the final desired volume of solution. The solution is poured into a volumetric flask using a funnel, and the meniscus must align with the mark on the flask. In aqueous solutions, the meniscus is concave and should be read at its lowest point to ensure accurate final volume and concentration.
Q5: What are two methods for sterilizing solutions in the laboratory?
Solutions can be sterilized by autoclaving, which subjects the solution to high-temperature steam under high pressure, or by filtration through a 0.22 micron filter to exclude bacterial cells. Sterilization is particularly important when preparing solutions for biological research involving living cells. Both methods effectively eliminate microbial contamination before experimental use.
Q6: How does phosphate buffered saline differ from other laboratory solutions?
Phosphate buffered saline (PBS) is a buffered solution that resists pH changes in the range of 7.2 to 7.6, mimicking physiological pH and osmolarity. PBS contains multiple salts with phosphate groups and has ion concentrations matching those of cells, making it isotonic. Common laboratory uses include washing cells and diluting biomolecules such as proteins in biological research.
Q7: What is the role of pH adjustment in solution preparation?
After solutes dissolve in solvent, pH can be adjusted using a calibrated pH meter for accuracy or pH paper for quick measurement. To raise pH, add dilute sodium hydroxide; to lower pH, add dilute hydrochloric acid slowly, as pH can change rapidly. Proper pH adjustment is critical for solutions used in biological research, where maintaining physiological conditions ensures experimental validity.
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