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Question

# What volume of 0.2 M NH4Cl solution should be added to 100 ml of 0.1 M NH4OH solution to produce a buffer solution of pH=8.7? Given : pKb of NH4OH=4.7; antilog (0.6)=4

A
50 ml
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B
100 ml
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C
200 ml
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D
None of the above
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Solution

## The correct option is C 200 mlGiven: pH=8.7, pKb(NH4OH)=4.7 ⇒pOH=14−8.7=5.3 Now Henderson equation for basic buffer is ⇒pOH=pKb+log[Salt][Base] ⇒pOH−pKb=log[Salt][Base]⇒5.3−4.7=log[Salt][Base]⇒0.6=log[Salt][Base] ⇒mmoles of saltmmoles of base=4 If volume of salt = V ml ⇒V×0.2100×0.1=4 ⇒V=200 ml

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