MEDIUM

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$H_{3} P O_{4} + H_{2} O ⇌ H_{3} O^{+} + H_{2} P O_{4}^{-}; p K_{1} = 2.15$
$H_{2} P O_{4}^{-} + H_{2} O ⇌ H_{3} O^{+} + H P O_{4}^{2 -}; p K_{2} = 7.20$
Hence pH of 0.01 M $N a H_{2} P O_{4}$ is

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Important Questions on Ionic Equilibrium

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

What is the pH of the resulting solution when equal volumes of

0.1

M NaOH and

0.01

M HCl are mixed?

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

Two solutions,

A

and

B,

each of

100 L

was made by dissolving

4 g

N a O H

and

9.8 g

H_{2} S O_{4}

in water, respectively. The

p H

of the resultant solution obtained from mixing

40 L

of solution

A

and

10 L

of solution

B

is ____________.

(\log 2 = 0.3)

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

Following solutions were prepared by mixing different volumes of

NaOH

and

HCl

of different concentrations.

(i)

60 mL \frac{M}{10} HCl + 40 mL \frac{M}{10} NaOH

(ii)

55 mL \frac{M}{10} HCl + 45 mL \frac{M}{10} NaOH

(iii)

75 mL \frac{M}{5} HCl + 25 mL \frac{M}{5} NaOH

(iv)

100 mL \frac{M}{10} HCl + 100 mL \frac{M}{10} NaOH

The

pH

of which one of them will be equal to

1

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

Given

pH

of a solution

' A'

' 3'

and it is mixed with another solution

' B'

having

pH

' 2'

. If both solutions are mixed, the resultant

pH

of the solution will be (Assume concentration and volume remain unchanged after mixing of individual solution)

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

10 m l

10 M

H_{2} S O_{4}

is mixed to

100 m l

1 M

N a O H

solution. The resultant solution will be

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

50 mL

solution of strong acid of

pH = 1

is mixed with a

50 ml

solution of strong acid of

pH = 2

. The

pH

of the mixture will be nearly

(\log 5.5 = 0.74)

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

What will be the resultant

pH

when

200 mL

of an aqueous solution of

HCl (pH = 2.0)

is mixed with

300 mL

of an aqueous solution of

NaOH (pH = 12)

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

Equal volumes of

pH

of a solution

A

3

and another solution

B

having

pH = 2

are mixed, then resultant

pH

of the solution will be :

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

The pH of a solution obtained by mixing 50 mL of 1 N

H C l

and 30 mL of 1 N

N a O H

is [

\log 2.5 = 0.3979

]

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

Represent the union of two sets by Venn diagram for each of the following.

$X = {x | x$ is a prime number between $80$ and $100}$

$Y = {y | y$ is an odd number between $90$ and $100}$

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

A solution is prepared by mixing 100 mL 0.50 M hydrazoic acid (HN₃), whose K_a = 3.6 x 10^{- 4} , with 400 mL of 0.10 M cyanic acid (HOCN), whose K_a = 8 x 10^{- 4} . Which of the following is (are) true regarding.

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

Which of the following solution will have

pH

close to

1.0

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

10 mL of 0.1 M

tribasic acid

H_{3} A

is titrated with

0.1 M NaOH

solution. What is the ratio of

\frac{[H_{3} A]}{[A^{3 -}]}

2^{nd}

equivalence point?

[Given : K_{a_{1}} = 10^{- 3}, K_{a_{2}} = 10^{- 8} and K_{a_{3}} = 10^{- 12}]

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

Determine the

pH

value of a solution obtained by mixing

25 mL

0.2 M HCl

and

50 mL

0.25 N NaOH

solutions.

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

A solution contains

10 mL 0.1 N

N a O H

and

10 mL 0.05 N

H_{2} S O_{4}

. What is the

p^{H}

of the corresponding solution?

MEDIUM

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

90 m l H C l

solution of

0.1 M

is added to

10 m L

0.89 M N a O H

solution. To this mixture,

40 m L

H_{2} {S O}_{4}

solution is added to get a

p H

of 2. The molarity of

H_{2} {S O}_{4}

added is -

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

Which of the following solutions will have pH close to 1.0 ?

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

What will be the

pH

of the solution on mixing two equal volume of solutions having

pH = 3

and

pH = 4

[\log 5.5 = 0.7404]

EASY

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

A solution was prepared by mixing

50 mL

0.2 M HCl

and

50 mL

0.1 M NaOH

. The

pH

of the solution is

HARD

Chemistry>Physical Chemistry>Ionic Equilibrium>pH Calculations for Different Solutions

Bromine in excess is dropped to a

0.01 M

{SO}_{2}

. All of

{SO}_{2}

is oxidized to

H_{2} {SO}_{4}

and the excess

{Br}_{2}

is removed by flushing with gaseous

N_{2}

. Determine the

pH

of the resulting solution assuming

K_{a 1}

H_{2} {SO}_{4}

very large &

K_{a2} = 10^{- 2} .

Take the value of

\log (3.24) = 0.51

. Give the answer to the nearest integer value after multiplying with 100.

H3PO4+H2O⇌H3O++H2PO4-; pK1=2.15 H2PO4-+H2O⇌H3O++HPO42-; pK2=7.20 Hence pH of 0.01 M NaH2PO4 is

Important Questions on Ionic Equilibrium

Learn and Prepare for any exam you want !

$H_{3} P O_{4} + H_{2} O ⇌ H_{3} O^{+} + H_{2} P O_{4}^{-}; p K_{1} = 2.15$
$H_{2} P O_{4}^{-} + H_{2} O ⇌ H_{3} O^{+} + H P O_{4}^{2 -}; p K_{2} = 7.20$
Hence pH of 0.01 M $N a H_{2} P O_{4}$ is