You visited us 3 times! Enjoying our articles? Unlock Full Access!

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

No worries! We‘ve got your back. Try BYJU‘S free classes today!

40 mL

No worries! We‘ve got your back. Try BYJU‘S free classes today!

30 mL

No worries! We‘ve got your back. Try BYJU‘S free classes today!

50 mL

Right on! Give the BNAT exam to get a 100% scholarship for BYJUS courses

Open in App

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.
$[H C O O N a] = \frac{0.1 \times V}{(V + 50)}$
$[H C O O H] = \frac{50 \times 0.05}{(V + 50)}$
$∴ p H = - log K_{a} + log \frac{[Salt]}{[Acid]}$
$4.0 = 3.7 + log \frac{\frac{(0.1 \times V)}{(V + 50)}}{\frac{2.5}{(V + 50)}}$
$V = 50 mL$

Suggest Corrections

Similar questions

Q. What volume of

0.10 M

sodium formate solution should be added to

50 m L

0.05 M

formic acid to produce a buffer solution of pH

4.0

p 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).

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. To a 50 mL of 0.05M formic acid how much volume of 0.10M sodium formate must be added to get a buffer solution of

p H = 4.4

[p K_{a}

of the acid is 3.8 ]

Join BYJU'S Learning Program

Explore more

Henderson Hassleback Equation

Standard XII Chemistry

Join BYJU'S Learning Program

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 $= 3.7$ ?