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?

Question

MARKS Content Team · Accepted Answer

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

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?

Solution

More Ionic Equilibrium Questions

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?

Solution

More Ionic Equilibrium Questions

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?