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What is the pH of a solution that has [H+] of 1.659e^-9 M

User Ajackster
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Answer is: pH = 8,75.
c(H⁺ or H₃O⁺) = 1,659·10⁻⁹ M = 1,659·10⁻⁹ mol/L = 0,000000001659 mol/L.

pH = -logc(H₃O⁺).

pH = -log(1,659·10⁻⁹ mol/L).

pH = 8,75.
When pH is less than seven (pH<7), solution is acidic.
When is equal seven (pH = 7), solution is neutral.
When pH is greater than seven (pH > 7), solution is basic
(like this example).

User Tillerstarr
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7.6k points
4 votes
pH of a solution is negative log of its hydrogen ion concentration. Mathematically it can be written as:

pH = - log[ H^(+)]
For the said problem pH will be:

pH = -log [ 1.659 * 10^(-9) ] \\ pH=-(log[1.659]+log[10^(-9)]) \\ pH=-log[1.659]+9log[10] \\ pH=-0.22+9=8.78

Thus the pH of solution will be 8.78.
User Rdiachenko
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