Calculate the pH of a solution with (H3O)+ concentration equal to 6.67*10^-4 mol/L.

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The pH of a solution is defined as the negative logarithm of the Hydronium ion concentration of the solution. If the `(H_3O)^+` concentration is C, the pH of the solution is equal to `-log_10(C)` . Pure water at 25 C has a pH approximately equal to 7. As the `H^+`...

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The pH of a solution is defined as the negative logarithm of the Hydronium ion concentration of the solution. If the `(H_3O)^+` concentration is C, the pH of the solution is equal to `-log_10(C)` . Pure water at 25 C has a pH approximately equal to 7. As the `H^+` or hydronium ion concentration of acidic solution is greater than that of pure water, the pH of acidic solutions is less than 7 and conversely the pH of basic solutions is greater than 7.

For a solution with `(H_3O)^+` concentration equal to 6.67*10^-4 mol/L, the pH of the solution is equal to `-log_10(6.67*10^-4) ~~ -3.17`

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