Conjugate Base Concentration
Conjugate Base Concentration - Related Videos
06:35
Acid and Base Concentrations - Concepts
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2020
Acids and Bases An Arrhenius acid produces hydrogen ions when it is dissolved in water: HA + H2O → H+(aq) + A-(aq) Here, HA is the non-dissociated acid, H+ is the hydrogen cation, and A- is the solvated anion — called the conjugate base. An Arrhenius base produces hydroxide ions when dissolved in water: BOH + H2O → B+(aq) + OH-(aq) Here, BOH is the non-dissociated base, OH- is the hydroxide ion, and B+ is the solvated cation — called the conjugate acid. A conjugate base is formed when an acid...
14:48
Acid and Base Concentrations - Student Protocol
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2020
Source: Smaa Koraym at Johns Hopkins University, MD, USA Preparation of ~0.1 M NaOHExpand In the first part of the lab, you will use a 50% w/w solution of NaOH to prepare 500 mL of ~0.1 M. The 50% w/w NaOH is indicative of its weight ratio. For example, if the instructor prepared 150 mL of the 50% w/w NaOH solution, then 150 g of NaOH was dissolved in 150 g of water, and the total weight of the solution is 300 g. To begin, put on the appropriate personal protective equipment,...
05:17
Acid and Base Concentrations - Instructor Prep
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2020
Source: Smaa Koraym at Johns Hopkins University, MD, USA Preparation of ReagentsExpand Here, we show the laboratory preparation for 10 students working in pairs, with some excess. Please adjust quantities as needed. Prepare 25 mL of 50% w/w NaOH solution. Weigh 25 g of NaOH pellets and add them to a 125-mL Erlenmeyer flask. Measure 25 mL of deionized water and add it to the flask. Add a magnetic stir bar and mix the solution on a stir plate until the solution appears...
02:29
Relative Strengths of Conjugate Acid-Base Pairs
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2020
Brønsted-Lowry acid-base chemistry is the transfer of protons; thus, logic suggests a relation between the relative strengths of conjugate acid-base pairs. The strength of an acid or base is quantified in its ionization constant, Ka or Kb, which represents the extent of the acid or base ionization reaction. For the conjugate acid-base pair HA / A−, the ionization equilibrium equations and ionization constant expressions are Adding these two chemical equations yields the equation for the...
13:17
Manufacture of Concentrated, Lipid-based Oxygen Microbubble Emulsions by High Shear Homogenization and Serial Concentration
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Cited by 12 •
2014
We describe methods for the manufacture of large volumes of lipid-based oxygen microbubbles (LOMs) designed for intravenous oxygen delivery using high-shear homogenization and serial concentration.
FAQs
Acid dissociation establishes a balance rather than complete conversion: HA transfers a proton to water, producing hydronium and A−, while the reverse process remains part of the equilibrium. The equilibrium position depends on Ka, so a greater tendency to dissociate produces more A− relative to HA under comparable conditions. This balance determines the concentration reached by the conjugate base.
The amount of A− formed depends on both Ka and the starting concentration of HA. For the same weak acid, changing the initial concentration changes the equilibrium concentrations, so Ka alone cannot specify [A−]. Calculations therefore combine the acid dissociation constant with the initial acid concentration to estimate how much HA converts into its conjugate base.
The Henderson–Hasselbalch relationship uses pH and pKa to connect the concentrations of A− and HA. When pH is below pKa, the acid form is relatively favored; when pH is above pKa, the conjugate base is relatively favored. At pH equal to pKa, the relationship indicates comparable concentrations of the two forms, supporting buffer assessment.
pH describes the solution’s acidity, but the absolute concentration of A− also depends on how much acid is present. The Henderson–Hasselbalch relationship provides the ratio of A− to HA through pH and pKa, while the initial acid concentration supplies the concentration scale. Consequently, pH data must be interpreted with acid concentration when estimating [A−].
A useful estimate requires the acid’s initial concentration and its Ka value, because these determine the equilibrium conversion of HA into A−. If pH or pKa is available, the Henderson–Hasselbalch relationship can instead connect the acid and conjugate-base concentrations. Selecting the appropriate approach depends on whether equilibrium or pH information is provided.
Tracking [A−] helps show how acid–base composition changes during titration and whether a solution contains the proportions needed for buffer behavior. Because pH, pKa, [HA], and [A−] are related, these values support pH control and buffer selection. The same analysis also aids chemical speciation by identifying which acid form predominates under specified conditions.