What is the pH of solutions having the following H3O+ concentrations? Identify each as acidic, basic, or neutral.
(a) [H3O+] = 1.0 × 10−3M
(b) [H3O+] = 1.0 × 10−13M
(c) [H3O+] = 3.4 × 10−10M
Acidic solutions have pH less than 7
Neutral solutions have pH = 7
Basic solutions have pH greater than 7
let us calculate pH of each solution
pH = -log [H3O+]
a) [H3O+] = 1.0 × 10−3M
pH = -log(1x10^-3) = 3
Since pH <7 , solution is acidic
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(b) [H3O+] = 1.0 × 10−13M
pH = -log [H3O+]
pH = -log(1x10^-13) = 13
Since pH >7 , solution is basic
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(c) [H3O+] = 3.4 × 10−10M
pH = -log [H3O+]
pH = -log(3.4x10^-10) = 9.47
Since pH >7 , solution is basic
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