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Henderson Hassleback Equation

What volume o...

Question

What volume of $0.1 M H C O O N a$ solution should be added to $50 mL$ of $0.05 M$ formic acid to produce a buffer solution of $p H = 4.0$ , $p K_{a}$ of formic acid $= 3.7$ ?

60 mL

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40 mL

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30 mL

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50 mL

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Solution

The correct option is D $50 mL$
Let $V mL$ of $0.1 M H C O O N a$ was mixed to $50 mL$ of $0.05 M H C O O H$ to form a buffer solution.
$[H C O O N a] = \frac{0.1 \times V}{(V + 50)}$
$[H C O O H] = \frac{50 \times 0.05}{(V + 50)}$
$∴ p H = - log K_{a} + log \frac{[Salt]}{[Acid]}$
$4.0 = 3.7 + log \frac{\frac{(0.1 \times V)}{(V + 50)}}{\frac{2.5}{(V + 50)}}$
$V = 50 mL$

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Similar questions

Q. What volume of

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What volume of 1.10 M sodium formate solution should be to 50 mL of 0.05 M formic acid to produce a buffer solution of pH 4.0? (pK_a for formic acid is 3.80).

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Henderson Hassleback Equation

Standard XII Chemistry

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What volume of 0.1 M HCOONa solution should be added to 50 mL of 0.05 M formic acid to produce a buffer solution of pH=4.0, pKa of formic acid =3.7 ?

The correct option is D 50 mLLet V mL of 0.1 M HCOONa was mixed to 50 mL of 0.05 M HCOOH to form a buffer solution. [HCOONa]=0.1×V(V+50) [HCOOH]=50×0.05(V+50) ∴ pH=−logKa+log[Salt][Acid] 4.0=3.7+log(0.1×V)(V+50)2.5(V+50) V=50 mL

What volume of $0.1 M H C O O N a$ solution should be added to $50 mL$ of $0.05 M$ formic acid to produce a buffer solution of $p H = 4.0$ , $p K_{a}$ of formic acid $= 3.7$ ?