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Standard XII

Chemistry

Molarity

Calculate cha...

Question

Calculate change in pH of 1 litre buffer solution. Containing 0.10 mole each of $N H_{3}$ and $N H_{4} C l$ Cl upon adding of (a) 0.02 mole of dissolved gaseous HCl, Assuming volume to be constant,
$K_{b} [N H_{3}] = 1.8 \times 10^{- 5}$

0.167 unit

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0.176 unit

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0.175 unit

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0.177 unit

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Solution

The correct option is B 0.176 unit
$p O H o f N H_{3} a n d N H_{4} C l b u f f e r = - l o g K_{b} + l o g \frac{[S a l t]}{[b a s e]}$
$= - l o g 1.8 \times 10^{- 5} + l o g \frac{0.1}{0.1} = 4.75$
$p H = (14 - 4.75) = 9.25$
$N H_{3} + H C l \to N H_{4} C l$
$[S a l t] = (0.1 - 0.02) = 0.12 M$
$[B a s e] = (0.1 - 0.02) = 0.08 M$
$p O H = - l o g K_{b} + l o g \frac{0.12}{0.08} = 4.75 + 0.176 = 4.926$
$p H = (14 - 9.926) = 9.074$
$Δ p H = (9.25 - 9.074) = 0.176 u n i t .$

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Calculate change in pH of 1 litre buffer solution. Containing 0.10 mole each of NH3 and NH4Cl Cl upon adding of (a) 0.02 mole of dissolved gaseous HCl, Assuming volume to be constant, Kb[NH3]=1.8×10−5

Calculate change in pH of 1 litre buffer solution. Containing 0.10 mole each of $N H_{3}$ and $N H_{4} C l$ Cl upon adding of (a) 0.02 mole of dissolved gaseous HCl, Assuming volume to be constant,
$K_{b} [N H_{3}] = 1.8 \times 10^{- 5}$