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Law of Mass Action

The pH of a...

Question

The $p H$ of a solution containing $0.4 M {H C O_{3}}^{-}$ and $0.2 M {C O_{2}}^{2 -}$ is:
$K_{a_{1}} (H_{2} C O_{3}) = 4 \times 10^{- 7}; K_{a_{2}} (H C O_{3}^{-}) = 4 \times 10^{- 11}$

10.4

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10.1

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601

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10.7

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Solution

The correct option is B $10.1$

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Similar questions

p H

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)

0.1 M H C O_{3}^{-}

0.2 M C O_{3}^{2 -} [K_{1} (H_{2} C O_{3}) = 4.2 \times 10^{- 7}

K_{2} (H C O_{3}^{-}) = 4.8 \times 10^{- 11}]

p H

N i (O H)_{2}

10^{- 3} M

N i^{2 +}

[K_{s p}

(N i (O H)_{2} = 10^{- 11}]

H C N

p H = 10.4

0.01

N a C N

K_{a} (H C N) = 4 \times 10^{- 10}

Δ p H

N a H C O_{3}

(i n i t i a l p H = 9, K a_{1} = 10^{- 7}, K a_{2} = 10^{- 11}

H_{2} C O_{3})

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