20 mL solution contains 0.1 M NH_4Cl and 0 | vedclass

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(A) The given solution is a basic buffer consisting of a weak base $(NH_4OH)$ and its salt with a strong acid $(NH_4Cl)$.According to the Henderson-Ha

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Addition of $1 \ mL$ water

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(A) The given solution is a basic buffer consisting of a weak base $(NH_4OH)$ and its salt with a strong acid $(NH_4Cl)$.According to the Henderson-Hasselbalch equation for a basic buffer,$pOH = pK_b + \log \frac{[Salt]}{[Base]}$.Dilution of a buffer solution with water does not change the ratio of the concentration of the salt to the concentration of the base,as both concentrations decrease by the same factor.Therefore,the $pH$ of a buffer solution remains unchanged upon the addition of a small amount of water.

$20 \ mL$ solution contains $0.1 \ M \ NH_4Cl$ and $0.01 \ M \ NH_4OH$. By adding which one will its $pH$ not change?

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