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[" 99.An aqueous solution of "0.01MCH(3)...

[" 99.An aqueous solution of "0.01MCH_(3)COOH" has "],[" van't Hoff factor of "1.01." If "pH=-log[H^(+)],pH],[" of "0.01MCH_(3)COOH" solution would be : "],[qquad (1/22]

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An aqueous solution of 0.01 M CH_(3) COOH has van't Hoff factor 1.01 . If pH = - "log"[H^(+)] , pH of 0.01 M CH_(3)COOH solution would be :

An aqueous solution of 0.01 M CH_3COOH has Van't Hoff factor 1.01. If pH=-log [H^+] , pH of 0.01 M CH_3COOH solution would be

Calculate the pH of 0.1 MNH_(3) solution.

The pH of 0.1 M solution of CH_(3)COOH if it ionizes to an extent of 1% is .

Calculate pH solution: 0.1 M CH_(3)COOH (K_a=1.8 xx 10^(-5))

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