Question:

What is the pH of a 0.01 M solution of sodium hydroxide?

Answer:

[H3O+][OH-] = 1 x 10^-14 [H3O+](0.01) = 1 x 10^-14 [H3O+] = 1 x 10^-12 pH = -log [H3O+] = -log (1 x 10^-12) = 12 Or you could say, pOH = -log [OH-] = -log (0.01) = 2 pH + pOH = 14 pH + 2 = 14 pH = 12


Tags:
pH
Chemistry
Bases
Acid-base chemistry
Equilibrium chemistry
Hydroxide
Sodium hydroxide
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