Question

A buffer solution is prepared by mixing 0.1 M ammonia and 1.0 M ammonium chloride. At 298 K, the p$K_b$ of NH₄OH is 5.0. The pH of the buffer is
(a) 10.0
(b) 9.0
(c) 6.0
(d) 8.0

Answer 1

10 is the correct answer.

Answer 2

The pH of the solution is 8.0

Explanation:

The chemical reaction for ammonium hydroxide (ammonia) and hydrochloric acid follows the equation:

                  $NH_4OH+HCl\rightarrow NH_4Cl+H_2O$

To calculate the pOH of basic buffer, we use the equation given by Henderson Hasselbalch:

$pOH=pK_b+\log(\frac{[salt]}{[base]})$

$pOH=pK_b+\log(\frac{[NH_4Cl]}{[NH_4OH]})$

We are given:

$pK_b$ = negative logarithm of base dissociation constant of ammonium hydroxide = 5.0

$[NH_4Cl]=1.0M$

$[NH_4OH]=0.1M$

pOH = ?

Putting values in above equation, we get:

$pOH=5.0+\log(\frac{1.0}{0.1})\\\\pOH=6.0$

To calculate pH of the solution, we use the equation:

$pH+pOH=14\\\\pH=14-6.0=8.0$

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