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pH of a Solution

Calculate the...

Question

Calculate the pH of a $0.033 M$ ammonia solution, if $0.033 M$ ${N H}_{4} C l$ is introduced in this solution at the same temperature. ( $k_{b}$ for ${N H}_{3} = 1.77 \times 10^{- 5}$ )

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Solution

To calculate the pH of the solution containing ammonia and NH4Cl, the Handerson Hasselbach equation is used
According to this equation,
pOH = pKb + log
where, pKb is to be calculated from Kb.
$k_{b}$ for ${N H}_{3}$ = 1.7710-5
$p k b$ = $- l o g k_{b}$ = -log (1.7710-5) = 4.75
[Salt] = $[N H_{4} C l]$ = 0.033 M
[Base] = $[N H_{3}]$ = 0.033 M
When we put all these values in the equation,
$p O H$ = 4.75 + log
= 4.75 + log (1) = 4.75+0 = 4.75
$p O H$ = 4.75
$p H$ = 14 - 4.75 = 9.25
$p H$ = 9.25
$p H$ of the solution = 9.25

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