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Buffer Solutions

What volume o...

Question

What volume of $0.1 M$ sodium formate 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 $= 3.80)$
(antilog 1.59 =39.62)

3.96 mL

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39.6 mL

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45 mL

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35.6 mL

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Solution

The correct option is B 39.6 mL
Suppose $V m L$ of $0.1 M H C O O N a$ $is mixed to 50 mL of (0.05 M H C O O H$
$[Molarity] = \frac{Total millimole}{Total volume}$
In mixture $[H C O O N a] = \frac{0.1 \times V}{(V + 50)}$
$[H C O O H] = \frac{50 \times 0.05}{V + 50}$
By Henderson hasselbalch equation,
$p H = - log K_{a} + log \frac{[Salt]}{[Acid]}$
$4.0 = 3.80 + {log}_{10} \frac{\frac{0.1 \times V}{(V + 50)}}{\frac{2.5}{(V + 50)}}$
$V = 39.62 mL$

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Similar questions

Q. What volume of

0.1 M

sodium formate 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

= 3.80)

(antilog 1.59 =39.62)

Q. What volume of

0.1 M H C O O N a

solution should be added to

50 mL

0.05 M

formic acid to produce a buffer solution of

p H = 4.0

p K_{a}

of formic acid

= 3.7

Q. What volume of

0.10

M sodium formate solution should be added to

50

ml of

0.05

M formic acid to produce a buffer solution of

p H

4.0

K_{a}

for formic acid is

3.80

]

Q. What volume of

0.1 M H C O O N a

solution should be added to

50 mL

0.05 M

formic acid to produce a buffer solution of

p H = 4.0

p K_{a}

of formic acid

= 3.7

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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Buffer Solutions

Standard XIII Chemistry

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What volume of 0.1 M sodium formate 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 =3.80) (antilog 1.59 =39.62)

The correct option is B 39.6 mLSuppose V mL of 0.1 M HCOONa is mixed to 50 mL of (0.05 M HCOOH [Molarity]=Total millimoleTotal volume In mixture [HCOONa]=0.1×V(V+50) [HCOOH]=50×0.05V+50 By Henderson hasselbalch equation, pH=−logKa+log[Salt][Acid] 4.0=3.80+log100.1×V(V+50)2.5(V+50) V=39.62 mL

What volume of $0.1 M$ sodium formate 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 $= 3.80)$
(antilog 1.59 =39.62)