(a)
Interpretation:
The principal reaction is
Concept Introduction:
Acid dissociation constant:
Consider a weak-acid equilibrium reaction,
The acid dissociation constant
A weak acid is one that doesn’t undergo completion.
The negative logarithm of an equilibrium constant is called as
The
The value of acid dissociation constant
The value of
Base dissociation constant:
Consider a reaction of weak base,
The value of
Where
(b)
Interpretation:
The
Concept Introduction:
Acid dissociation constant:
Consider a weak-acid equilibrium reaction,
The acid dissociation constant
A weak acid is one that doesn’t undergo completion.
The negative logarithm of an equilibrium constant is called as
The
The value of acid dissociation constant
The value of
Base dissociation constant:
Consider a reaction of weak base,
The value of
Where
(c)
Interpretation:
The number of
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General Chemistry: Atoms First
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- Tartaric acid is a weak diprotic fruit acid with Ka1 = 1.0 103 and Ka2 = 4.6 105. a Letting the symbol H2A represent tartaric acid, write the chemical equations that represent Ka1 and Ka2. Write the chemical equation that represents Ka1 Ka2. b Qualitatively describe the relative concentrations of H2A, HA, A2, and H3O+ in a solution that is about 0.5 M in tartaric acid. c Calculate the pH of a 0 0250 M tartaric acid solution and the equilibrium concentration of [H2A]. d What is the A2 concentration in solutions b and c?arrow_forward(a) Calculate the pH in the solution formed by adding 10.0 mL of 0.050 M NaOH to 40.0 mL of 0.0250 M benzoic acid (C6H5COOH, Ka = 6.3 * 10-5). (b) Calculate the pH in the solution formed by adding 10.0 mL of 0.100 M HCl to20.0 mL of 0.100 M NH3.arrow_forwardWrite the chemical equation and the Ka expression for the acid dissociation of each of the following acids in aqueous solution. First show the reaction with H+1aq2 as a product and then with the hydronium ion: (a) C6H5COOH, (b) HCO3 -.arrow_forward
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