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pH the Power of H

Calculate the...

Question

Calculate the pH of a solution containing $0.1 M H C O_{3}^{-}$ and $0.2 M C O_{3}^{2 -} [K_{1} (H_{2} C O_{3}) = 4.2 \times 10^{- 7}$ and $K_{2} (H C O_{3}^{-}) = 4.8 \times 10^{- 11}]$ .

A

3.18

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B

10.62

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C

6.62

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D

9.31

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Solution

The correct option is B 10.62
$H C O_{3}^{-} + H_{2} O ⟶ H_{3} O^{+} + C O_{3}^{2 -} K_{2} = \frac{[H_{3} O^{+}] [C O_{3}^{2 -}]}{H C O_{3}^{-}} = 4.8 \times 10^{- 11} [H_{3} O^{+}] = 4.8 \times 10^{- 11} \times \frac{[H C O_{3}^{-}]}{[C O_{3}^{2 -}]} = 4.8 \times 10^{- 11} \times (\frac{0.1}{0.2}) \Rightarrow [H_{3} O^{+}] = 4.8 \times 10^{- 11} \times 0.5 p H = - log [H_{3} O^{+}] = - log [4.8 \times 10^{- 11} \times 0.5] = 10.62$

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Similar questions

p H

of a solution containing

0.4 M

H C O_{3}^{-}

0.2 M

C O_{3}^{2 -}

[K_{a_{1}} (H_{2} C O_{3}) = 4 \times 10^{- 7}; K_{a_{2}} (H C O_{3}^{-}) = 4 \times 10^{- 11}]

(G i v e n, l o g 4 = 0.60, l o g 0.5 = - 0.3)

p H

of the resulting solution and then mark the option in which

p H

exists between color transition range of an indicator.

50

0.1

H C O_{3}^{-} +

50

0.8

C O_{3}^{2 -}

.

H_{2} C O_{3}

K_{a_{1}} = 4 \times 10^{- 7}

K_{a_{2}} = 2 \times 10^{- 11}

Q. Calculate the pH of

0.1

M solution of (i)

N a H C O_{3}

N a_{2} H P O_{4}

N a H_{2} P O_{4}

C O_{2} + H_{2} O ⇌ H^{+} + C O_{3}^{2 -}

K_{1} = 4.2 \times 10^{- 7}

M

H C O_{3}^{-} ⇌ H^{+} + C O_{3}^{2 -}

K_{2} = 4.8 \times 10^{- 11}

M

H_{2} P O_{4} ⇌ H^{+} + H_{2} P O_{4}^{-}

K_{1} = 7.5 \times 10^{- 3}

M

H_{2} P O_{4}^{-} ⇌ H^{+} + H P O_{4}^{2 -}

K_{2} = 6.2 \times 10^{- 8}

M

H P O_{4}^{2 -} ⇌ H^{+} + P O_{4}^{3 -}

K_{3} = 1.0 \times 10^{- 12}

Q. Given an aqueous solution of

0.034 M

carbonic acid, the ionization constants for carbonic acid are

K_{1} = 4.2 \times 10^{- 7}

K_{2} = 4.8 \times 10^{- 11}

Select the correct statement from the following:

H_{2} {C O}_{3}

H_{2} {C O}_{3} ⇌ H^{+} + H {C O}_{3}^{-}; K_{1} = 4.3 \times 10^{- 7}

H {C O}_{3}^{-} ⇌ H^{+} + {C O}_{3}^{2 -}; K_{2} = 5.6 \times 10^{- 11}

Calculate the degree of hydrolysis and pH value of

0.12 M

{N a}_{2} {C O}_{3}

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pH the Power of H

Standard XII Chemistry

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