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Chapter 9: Q24P (page 209)

A 0.10 M solution of a base is 2.0% hydrolzed $(α = 0.020)$ Find $K_{b}$

Short Answer

Expert verified

The value of $K_{b} = 4.1 \times 10^{- 5}$ .

Step by step solution

01

Step : Consider a reaction

Let the given base be B.

The reaction of base B with water is as shown below:

$B + H_{2} O ⇌ {BH}^{+} + {OH}^{-} [B] = 0.1 - x [{BH}^{+}] = [{OH}^{-}] = x)$

02

Calculation of the value of x

$α = \frac{x}{F} x = α \times F = 0.02 \times 0.1 = 0.002$

03

Calculate

$\begin{array}{l} K = \frac{x^{3}}{0.1 - x} \\ = \frac{{(0.002)}^{2}}{0.1 - 0.002} \\ = 4.1 \times 10^{- 5} \end{array}$

Hence, the value of K_b is $4.1 \times 10^{5}$ .

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Most popular questions from this chapter

Effect of ionic strength on ${pK}_{a} . K_{a}$ for the localid="1654774253353" $H_{2} {PO}_{4} / {HPO}_{4}^{2 ‐}$ buffer islocalid="1654774257371" $K_{a} = \frac{[{HPO}_{4}^{2 ‐}] [H^{+}] Y_{HP {O_{4}}^{2 ‐}} Y_{H^{+ +}}}{[H_{2} P {O_{4}}^{‐}] Y_{H_{2} P {O_{4}}^{‐}}} = 10^{‐ 7.20}$ If you mix a localid="1654774261368" $1 : 1$ mole ratio of localid="1654774264927" $H_{2} {PO}_{4}$ andlocalid="1654774269015" $H_{2} P {O_{4}}^{‐ 2}$ at 0 ionic strength, the is 7.20. Using activity coefficients from Tablelocalid="1654774273534" $8 ‐ 1$ calculate the pH of a localid="1654774278805" $1 : 1$ mixture of and localid="1654774317458" $HP {O_{4}}^{‐ 2}$ at an ionic strength of 0.10. Remember thatlocalid="1654774320706" $pH = - {logA}_{H^{+}} = - \log [H^{+}] Y_{H^{+}}$

What concentrations of H⁺ and OH^- are produced by H₂O dissociation in 0.01 M NaOH?

A $0.0450 M$ solution of HAis 0.60%dissociated. Calculate ${pK}_{a}$ for this acid.

When is a weak acid weak and when is a weak acid strong? Show that the weak acid $99 %$ dissociatedrole="math" localid="1654854665468" $F = (0.0102) K_{a}$ will be 92%dissociated when dissolved in water if the formal concentration is one-tenth $(F = Ka / 10)$ of Show that the fraction of dissociation is 27%when $F = 10 Ka$ . At what formal concentration will the acid be 99%dissociatedCompare your answer with the left -hand curve in Figure 9-2

Find theand concentrations of ${({CH}_{3})}_{3} N$ and ${({CH}_{3})}_{3} {NH}^{+}$ in $0.060 M$ trimethylammonium chloride.

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