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Chapter 0: Q6-I E (page 1)

Succinic acid dissociates in two steps:

Short Answer

Expert verified

Base dissociation constant for given reaction is,

$K_{b 1} = 4.3 x 10^{9} K_{b 2} = 1.6 x 10^{- 10}$

Step by step solution

01

formula for acid and base dissociation constant

Consider a weak-acid equilibrium reaction ${HA}^{K_{3}} H^{+} + A^{-}$

The acid dissociation constant $K_{a}$ can be given as,

$K_{a} = \frac{[H^{+}] [A^{- 1}]}{[HA]}$

Consider a reaction of weak base,

role="math" localid="1663382177574" $B + H_{2} O^{K_{O}} {BH}^{+} + {OH}^{-}$

The value of $K_{b}$ can be calculated as,

$K_{b} = \frac{[{BH}^{+}] [OH]}{[B]}$

Where $K_{b}$ is called as base dissociation constant.

The value of $K_{w}$ is calculated by the formula,

$K_{w} = K_{a} x K_{b}$

02

Step 2: calculate Base dissociation constant

Acid dissociation constant for given reaction is,

$K_{a 1} = 6.2 \times 10^{- 5} K_{a 2} = 2.3 \times 10^{- 6}$

To calculate: Base dissociation constant $(K_{b})$ for first step

$K_{w} = K_{a} \times K_{b}$

Where,

$(K_{b})$ is base dissociation constant.

$(K_{w})$ is ionic product of water $(1.00 \times 10^{14})$

$(K_{a})$ is acid dissociation constant

$K_{b 1} = \frac{K_{w}}{K_{a 2}}$

$\frac{1.0 \times 10^{- 14}}{2.3 \times 10^{6}} K_{b 1} = 4.3 \times 10^{9}$

To calculate: Base dissociation constant $(K_{b})$ for second step

$K_{b 2} = \frac{K_{w}}{K_{a 1}}$

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Most popular questions from this chapter

25. Write a mass balance for a solution of $F e_{2} ({SO}_{4})_{3}$ if the species

are ${Fe}^{3 +}, Fe {(OH)}^{2 +}, Fe {(OH)}_{2}^{+}, {FeSO}_{4}^{+}, {SO}_{4}^{2 -}$ androle="math" localid="1663402048017" ${SO}_{4}^{2 -}$ .

Consider the following equilibria in aqueous solution:

(1) ${Ag}^{+} + {Cl}^{-} ⇌ AgCl (aq) K = 2.0 \times 10^{3}$

(2) $AgCl (aq) + {Cl}^{-} ⇌ {AgCl}_{2}^{-} K = 9.3 \times 10^{1}$

(3) $AgCl (s) ⇌ {Ag}^{+} + {Cl}^{-} K = 1.8 \times 10^{- 10})$

(a) Calculate the numerical value of the equilibrium constant for the reaction $AgCl (s) ⇌ AgCl (aq)$ .

(b) Calculate the concentration of $AgCl (aq)$ in equilibrium with excess undissolved solid AgCl.

(c) Find the numerical value of $K$ for the reaction ${AgCl}_{2}^{-} = AgCl (s) + {Cl}^{-}$

Find the area from $800$ to $1000$ hours.

Effect of concentration in the titration of weak acid with strong base.Use your spreadsheet from Problem 11-66 to prepare a family of titration curves for pKa = 6, with the following combinations of concentrations: (a) C_a = 20 mM, C_b = 100 mM; (b) C_a = 2 mM, C_b = 10 mM; (c) C_a = 0.2 mM, C_b = 1 mM.

Write the $K_{a}$ reaction for trichloroacetic acid,, ${Cl}_{3} {CCO}_{2} H$ for anilinium ion, ${NH}_{3}$ , and for lanthanum ion, ${La}^{3 +}$ .

See all solutions

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