If the pK_ a of acetic acid and pK_ b of NH_ 4 OH are 4.76 and 4.75 respectively, what will be the pH of ammonium acetate solution?

Correct answer: B. 7.005 When a weak acid (acetic acid) and weak base ( NH_ 4 OH) are mixed to form a solution. pH of the solution is then determined by following formula: pH=7+(1)/(2) [ pK_ a - pK_ b ] Given, pK _ a =4.76, pK_ b =4.75 pH=7+(1)/(2) [4.76 - 4.75] pH=7+0.005 pH=7.005

NTA Abhyas 2020

Exam: NTA Abhyas
Year: 2020
Subject: Chemistry
Chapter: Ionic Equilibrium

NTA Abhyas 2020 · Chemistry · Ionic Equilibrium

If the pK_ a of acetic acid and pK_ b of NH_ 4 OH are 4.76 and 4.75...

If the

{\text{pK}_{a}

of acetic acid and

{\text{pK}_{b}

{\text{NH}_{4} \text{OH}

are

4.76

and

4.75

respectively, what will be the

\text{pH}

of ammonium acetate solution?

Options

A $9.51$
B $7.005$
C $7.00$
D $6.9$

Correct answer

B. $7.005$

Step-by-step solution

When a weak acid (acetic acid) and weak base

\left({\text{NH}_{4} \text{OH}\right)

are mixed to form a solution.

\text{pH} of the solution is then determined by following formula:<br /><br />\text{pH}\text{=}\text{7}\text{+}\dfrac{1}{2} \left[{\text{pK}_{a} - {\text{pK}_{b}\right]<br /><br />Given,

{

\text{pK}

}_{a}

\text{=}\text{4}\text{.76,}

{

\text{pK}_{b} \text{=}\text{4}\text{.75}

\text{pH}\text{=}\text{7}\text{+}\dfrac{1}{2} \left[\text{4}\text{.76} - \text{4}\text{.75}\right]

\text{pH}\text{=}\text{7}\text{+}\text{0}\text{.005} <br /><br />\text{pH}\text{=}\text{7}\text{.005}

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