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Electromeric Effect

calculate the...

Question

calculate the carbonate conc. in [CO3 ] in a 0.10 M solution of the weak acid, carbonic acid (H2CO3 ). The dissociation constants of carbonic acid are Ka1 =4.510^-7 & Ka210^-11 and . (1) 4.7 × 10^-4 M (2) 1.0 × 10^-4 M (3) 4.5 × 10^-4 M (4) 2.1 × 10^-4 M

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Solution

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

K_{a_{1}} = 4.0 \times 10^{- 7}

K_{a_{2}} = 7.0 \times 10^{- 11}

[H C O_{3}^{-}]

C O_{3}^{2 -}

K_{a 1} f o r H_{2} C O_{3} = 4.45 \times 10^{- 7}

K_{a 2} f o r H_{2} C O_{3} = 4.69 \times 10^{- 11}

10^{- 4.18} = 6.6 \times 10^{- 5}

p H

0.010 M

N a H {C O}_{3}

K_{1} = 4.5 \times 10^{- 7}

K_{2} = 4.7 \times 10^{- 11}

C O_{3}^{2 -}

K_{a 1} f o r H_{2} C O_{3} = 4.45 \times 10^{- 7}

K_{a 2} f o r H_{2} C O_{3} = 4.69 \times 10^{- 11}

10^{- 4.18} = 6.6 \times 10^{- 5}

p H

0.01 M N a H C O_{3}

K_{a_{1}} a n d K_{a_{2}}

H_{2} C O_{3}

4.5 \times 10^{- 7} a n d 4.7 \times 10^{- 11}

25^{o} C

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calculate the carbonate conc. in [CO3 ] in a 0.10 M solution of the weak acid, carbonic acid (H2CO3 ). The dissociation constants of carbonic acid are Ka1 =4.5*10^-7 & Ka2*10^-11 and . (1) 4.7 × 10^-4 M (2) 1.0 × 10^-4 M (3) 4.5 × 10^-4 M (4) 2.1 × 10^-4 M