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Byju's Answer

Standard XII

Chemistry

Basic Buffer Action

The pH of a b...

Question

The pH of a buffer containing equal molar concentrations of a weak base and its chloride ( $K_{b}$ for weak base $= 2 \times 10^{- 5}, log 2 = 0.3$ ) is:

5

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9

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4.7

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9.3

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Solution

The correct option is D $9.3$
Applying the equation
$p O H = log \frac{[S a l t]}{[B a s e]} - log K_{b}$
$= log 1 - log 2 \times 10^{- 5} = 4.7$
$p H = (14 - 4.7) = 9.3$

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Similar questions

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(A^{+})

25^{\circ} C

.
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The pH of a buffer containing equal molar concentrations of a weak base and its chloride (Kb for weak base =2×10−5,log2=0.3) is:

The correct option is D 9.3Applying the equationpOH=log[Salt][Base]−logKb=log1−log2×10−5=4.7pH=(14−4.7)=9.3

The pH of a buffer containing equal molar concentrations of a weak base and its chloride ( $K_{b}$ for weak base $= 2 \times 10^{- 5}, log 2 = 0.3$ ) is:

The correct option is D $9.3$
Applying the equation
$p O H = log \frac{[S a l t]}{[B a s e]} - log K_{b}$
$= log 1 - log 2 \times 10^{- 5} = 4.7$
$p H = (14 - 4.7) = 9.3$