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Can some one break this down, and explain how what is happening ? Thank you The acid dissociation constant, Ka, for benzoic acid, C6H5COOH, is

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Can some one break this down, and explain how what is happening ?

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The acid dissociation constant, Ka, for benzoic acid, C6H5COOH, is 6.28105. What is the pH of a 0.15 molar solution of this acid? [H3O+]=[C6H5COO]=x Ka=(0.15)(x)(x)=6.28105pH=log10[H3O+] pH=2.5 with 2 decimal figures ( 1/2 for 3 sig figs)

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