MyQuestionIcon

1

You visited us 1 times! Enjoying our articles? Unlock Full Access!

pH of a Solution

Calculate the...

Question

Calculate the pH of a solution which is 0.1 M in HA and 0.5M in NaA. Ka for HA is $1.8 \times 10^{- 6}$ ?

A

3

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

B

4

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

C

6.4

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

D

10

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

Open in App

Solution

The correct option is C 6.4
$P N = P k a + log \frac{s a l t}{a c i d}$
$P n = - {log}_{10} (1.8 \times 10^{- 6}) + (\frac{0.5}{0.1})$
$= 5.74 + 0.6989$
$P N = 6.44$

Suggest Corrections

thumbs-up

0

Similar questions

Q. Calculate the composition of an acidic buffer solution

(H A + N a A)

of total molarity

0.29

p H = 4.4

K_{a} = 1.8 \times 10^{- 5}

H A

10 %

0.01 M

aqueous solution. Calculate the pH of a solution which is

0.1 M

H A

0.05 M

N a A

.

Q. A weak acid, HA is found to be 10% ionized 0.01 M aqueous. Calculate the pH of a solution which is 0.1 M in HA and 0.05 M in NaA:

Q. The composition of an acidic buffer solution of

N a A

H A

of total molarity

0.29

p H = 4.4

{K A}_{a} = 1.8 \times 10^{- 5}

[H^{+}]

in a solution containing

0.1

H C O O H

0.1

H O C N

K_{a}

H C O O H

H O C N

1.8 \times 10^{- 4}

3.3 \times 10^{- 4}

View More

Join BYJU'S Learning Program

similar_icon

Related Videos

lock

pH of a Solution

CHEMISTRY

Watch in App

explore_more_icon

Explore more

pH of a Solution

Standard IX Chemistry

Join BYJU'S Learning Program

CrossIcon