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Chapter 9: Q42P (page 209)

Calculate the pH of a solution prepared by mixing $0.0800 mol$ of chloroacetic acid plus $0.0400 mol$ of sodium chloroacetate in $1.00 L$ of water.
(a) First do the calculation by assuming that the concentrations of HA and $A^{-}$ equal their formal concentrations.
(b) Then do the calculation, using the real values of and in the solution.
(c) Using first your head, and then the Henderson-Hasselbalch equation, find the pH of a solution prepared by dissolving all the following compounds in one beaker containing a total volume of $1.00 L : 0.180 {molCICHCOO}_{2} H, 0.020 mol {CICHCHO}_{2} {Na}_{2} 0.080 {molHNO}_{3,}$ and $0.080 molCa {(OH)}_{2}$ . Assume that $Ca {(OH)}_{2}$ dissociates completely.

Short Answer

Expert verified

a) The pH is $2.56$ .

b) The pH is $2.61$ .

c) The pH is $2.86$ .

Step by step solution

01

Concept used.

The pH of the buffer determined by the concentration ratio of $[A^{-}]$ and $[HA]$ by the following Henderson-Hasselbalch equation: $pH = {pK}_{a} + \log ([A^{-}] / [HA])$

02

First do the calculation by assuming that the concentrations of HA and A- equal their formal concentrations.

a)

The pH,

$pH = {pK}_{a} + \log ([A^{-}] / [HA]) pH = {pK}_{a} + \log ([sodium chloroacetate] / [chloroacetic acod]) pH = 2.865 + \log (0.04 / 0.08) = 2.56$

03

The calculation using the real values of HA and A- in the solution.

b)

Calculate the pH by using the real values of $[HA]$ and $[A^{-}]$ :

$K_{a} = \frac{[H^{+}] [A^{-}]}{[HA]} = \frac{[H^{+}] (0.04 - [H^{+}]}{0.08 - [H^{+}]} [H^{+}] = 2.48 脳 10^{3} M pH = - \log [H^{+}] = - \log (2.48 脳 10^{3}) = 2.61$

04

The pH of a solution prepared by dissolving all the following compounds in one beaker.

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Most popular questions from this chapter

Does the pH change in the right direction when HCl is added?

What concentration of OH^- is produced by H₂O dissociation in this solution? Was it justified to neglect water dissociation as a source of OH^-?

Find the pH and fraction of association $(伪)$ of a 0.100Msolution of the weak base B with $K_{b} = 1.00 脳 10^{- 5}$ .

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

Why doesn鈥檛 water produce $10^{- 7} M H^{+}$ , andwhen

is added?

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