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Chapter 9: Q9FE (page 207)

Find the pH of 0.050 M sodium butanoate (the sodium salt of
butanoic acid, also called butyric acid).

Short Answer

Expert verified

The of Sodium butanoate is 8.76.

Step by step solution

01

Th base dissociation constant

The K_b base dissociation constant is a measure of basicity or the strength of the base in general.

The value ofis:

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

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

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

$K_{w} = K_{a} 脳 K_{b}$

02

Step 2: Calculate the pH of 0.050M sodium butanoate

The chemical equation can be given as,

${CH}_{3} {CH}_{2} {CH}_{2} {CO}_{2}^{-} H_{2} O 鈬� {CH}_{3} {CH}_{2} {CH}_{2} {CO}_{2} H + {OH}^{-}$

The value of $K_{b}$ is calculated from the value of $K_{w}$ and $K_{a}$

$K_{b} = \frac{K_{w}}{K_{a}} = 6.58 脳 10^{- 10}$

$FromICEtable : \frac{x^{2}}{0.050 - x} = K_{b} x = \sqrt{(0.050) (6.58 脳 10^{- 10}) x} = 5.74 脳 10^{- 6} M$

The pH of weak base is calculated using the equation,

$pH = [H^{+}] = \frac{K_{w}}{[{OH}^{-}]} pH = - \log [H^{+}] pH = - \log [5.74 脳 10^{- 6} M] pH = 8.76$

The pH of 0.050M Sodium butanoate is 8.76.

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Most popular questions from this chapter

(a) Write the chemical reactions whose equilibrium constants are $^{K_{b}}$ and $^{K_{a}}$ for imidazole and imidazole hydrochloride respectively.

(b) Calculate the pH of a solution prepared by mixing $^{1.00 g}$ of imidazole with $^{1.00 g}$ of imidazole hydrochloride and diluting torole="math" localid="1655093511290" $^{100.0 mL}$ .

(c) Calculate the pH of the solution if $^{2.30 mL}$ of $^{1.07 {MHCIO}_{4}}$ are added.

(d) How many milliliters of $^{1.07 {MHCIO}_{4}}$ should be added to of imidazole to give a pH ofrole="math" localid="1655093364034" $^{6.993}$ ?

Select a compound from Table 9-2 that you could use to make 250mLof 0.2Mbuffer with a pH of 6.0. Explain how you would make the buffer.

Write the chemical reaction whose equilibrium constant is

(a) $K_{a}$ for benzoic acid, $C_{6} H_{5} {CO}_{2} H$

(b) $K_{b}$ for benzoate ion, $C_{6} H_{5} {CO}_{2}^{2 -}$

(c) $K_{b}$ for aniline, $C_{6} H_{5} {NH}_{2}$

(d) $K_{a}$ for anilinium ion, $C_{6} H_{5} {NH}_{3}^{+}$

Describe how to prepare 250mLof 1.00M ammonia bufferpH9.00 starting with 28 wt % ${NH}_{3}$ (鈥渃oncentrated ammonium hydroxide鈥� listed on the back inside cover of the book) and 鈥渃oncentrated鈥滺CI(37.2 wt %)or 鈥渃oncentrated鈥� NaOH(50.5wt%)

A solution contains 63 different conjugate acid-base pairs.

Among them is acrylic acid and acrylate ion, with the equilibrium ratio [acrylate]/[acrylic acid]5 0.75. What is the pH of the solution?

$H_{2} C = {CHCO}_{2} H {pK}_{a} = 4.25$

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