Calculate the pH of a 0.10 M solution of hypochlorous acid, HOC1- Ka of HOC1 is

Question

Calculate the pH of a 0.10 M solution of hypochlorous acid, HOC1- Ka of HOC1 is 3.5 times 10-8. Express your answer numerically using two decimal places. Calculate the pH of a 0.10 M solution of HCl Express your answer numerically using two decimal places. plusminus pH of a Strong Acid, a Weak Acid, a Strong Base, and a Weak Base The pH of a solution is the negative logarithm of the molar concentration of hydronium ion, that is, pH = -log[H3O+] In neutral solutions at 25 degree C, [H30+] = 10-7 M and pH = 7. As [H30+] increases, pH decreases, so acidic solutions have a pH of less than 7. Basic solutions have a pH greater than 7. The hydroxide and hydronium ion concentrations are related by the the ion-product constant of water, Kw, as follows: Kw = 1.0 times 1.0-14 = [H30+][0H-] In the same way as the pH, we can define the pOH as pOH = -log[OH-]. It follows from the Kw, expression that pH + pOH = 14. Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2 Express your answer numerically using two decimal places. Calculate the pH of a 0.10 M solution of NaOH Express your answer numerically using two decimal places. Calculate the pH of a 0.10 M solution of hydrazine, N2H4. K4 for hydrazine is 1.3 times 10-6. Express your answer numerically using two decimal places

Explanation / Answer

pH is given by the formula = -log [H+]

Part B - its hydroxide so aqueous solution gives OH- ions

hence [OH-] = 0.1

pOH = -log[OH-] = -log0.1 = 1

Hence pH = 14 - pOH = 13

Part C - Again hydroxide

hence [OH-] = 0.1

pOH = -log (0.1) = 1

Hence pH = 14 - pOH = 13

Part D - For weak bases

[OH-] = sqrt(Kb * c) = sqrt(1.3 * 10^-6 * 0.1) = 3.6 * 10^-4

pOH = 3.443

pH = 14 - 3.443 = 10.557

Part E - For weak acids

[H+] = sqrt(Ka * c) = sqrt(3.5 * 10^-8 * 0.1) = 5.91 * 10^-5

pH = -log[H+] = 4.227

Part F - Its a strong acid

hence pH = -log[H+] = -log(0.1) = 1

Hence pH = 1

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