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The pH of a solution containing 0.4 M {H}{C}{{O}_{{{3}}}^{{-}}

Question

The pH of a solution containing 0.4 M $H C O_{3}^{-}$ and 0.2 M $C O_{3}^{2 -}$ 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

10.1

6.1

10.7

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James Discussed

The pH of a solution containing 0.4 M

H C O_{3}^{-}

and 0.2 M

C O_{3}^{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}]

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Question Text	The pH of a solution containing 0.4 M $H C O_{3}^{-}$ and 0.2 M $C O_{3}^{2 -}$ is : $[K_{a 1} (H_{2} C O_{3}) = 4 \times 10^{- 7}$ , $K_{a 2} (H C O_{3}^{-}) = 4 \times 10^{- 11}]$
Answer Type	Text solution:1
Upvotes	150