A solution is prepared at that is initially in chlorous acid , a weak acid with , and in potassium chlorite . Calculate the pH of the solution. Round your answer to decimal places.

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25-01-2020
Chemistry

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A solution is prepared at that is initially in chlorous acid , a weak acid with , and in potassium chlorite . Calculate the pH of the solution. Round your answer to decimal places.

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Аноним Аноним · Answer 1 · 2020-01-27T05:14:57+01:00

The question is incomplete, here is the complete question:

A solution is prepared at 25°C that is initially 0.075 M in chlorous acid [tex](HClO_2)[/tex] , a weak acid with [tex]K_a=1.1\times 10^{-2}[/tex], and 0.34 M in potassium chloride [tex](KClO_2)[/tex] . Calculate the pH of the solution. Round your answer to 2 decimal places.

Answer: The pH of the solution is 2.62

Explanation:

The chemical equation for the reaction of chlorous acid and potassium hydroxide follows:

[tex]HClO_2+KOH\rightarrow KClO_2+H_2O[/tex]

To calculate the pH of acidic buffer, we use the equation given by Henderson Hasselbalch:

[tex]pH=pK_a+\log(\frac{[salt]}{[acid]})[/tex]

[tex]pH=pK_a+\log(\frac{[NaHCO_3]}{[H_2CO_3]})[/tex]

We are given:

[tex]pK_a[/tex] = negative logarithm of acid dissociation constant of chlorous acid = 1.96

[tex][KClO_2]=0.34M[/tex]

[tex][HClO_2]=0.075M[/tex]

pH = ?

Putting values in above equation, we get:

[tex]pH=1.96+\log(\frac{0.34}{0.075})\\\\pH=2.62[/tex]

Hence, the pH of the solution is 2.62