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PH of a 0.300M solution. Help me please.

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What is the pH of a 0.300M solution of HCN in which the CN- concentration has been adjusted to 0.00100 M?

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  1. HCN -->  H+  &  CN-

    K = [H+]  [CN-] / [HCN]

    4.9e-10 = [H+]  [0.001] / [0.300]

    H+ = 1.47e-7

    your answer is: pH = 6.83

    books differ on the Ka for various acids. if you have a Ka , you should use it instead of the one from my book

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