Find the concentration of HCO_3^-,in a 0.01Msolution of carbonuc acid if pH of this solution is 4.18.Ka_1 for H2CO3=4.45x10^-

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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}

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}

H^{+}, H C O_{3}^{-}

{C O}_{3}^{2 -}

0.01 M

4.18

K_{1} = 4.45 \times 10^{- 7}, K_{2} = 4.69 \times 10^{- 11}

(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}^{-}]

0.025 M

An aqueous solution of carbonic acid ( $H_{2} C O_{3}$ ) contains

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