Part E Calculate the pH of a 0.10 M solution of hypochlorous acid, HOCI. K of...

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Part E Calculate the pH of a 0.10 M solution of hypochlorous acid, HOCI. K of HOCI is 3.5 × 10-8. Express your answer numerically using two decimal places. pH = √, aß, AE, Submit Hints My Answers Give Up Review Part reset shortcuts? help Part F Calculate the pH of a 0.10 M solution of HCI. Express your answer numerically using two decimal places. VD, αβ, ΔΣ, pH Submit reset shortcuts ? help Hints My Answers Give Up Review Part + 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 °C, [H3O+] = 10-7 M and pH = 7. As [H3O+] 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, K, as follows: K=1.0 × 10-¹4 = [H3O+][OH-] In the same way as the pH, we can define the pOH as pOH = -log[OH-]. It follows from the K, expression that pH + pOH = 14. Part B Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2. Express your answer numerically using two decimal places. pH = Submit Hints My Answers Give Up Review Part Part D Part C Calculate the pH of a 0.10 M solution of NaOH. Express your answer numerically using two decimal places. 1945, αβ, ΔΣ, pH = Submit Γ' Ε, αβ, ΔΣ, reset shortcuts ? help pH = reset shortcuts ? help Hints My Answers Give Up Review Part Calculate the pH of a 0.10 M solution of hydrazine, N₂H₁. K₁, for hydrazine is 1.3 x 10-6. Express your answer numerically using two decimal places. [I'VD, αβ, ΔΣ, reset shortcuts ? help Part E Calculate the pH of a 0.10 M solution of hypochlorous acid, HOCI. K of HOCI is 3.5 × 10-8. Express your answer numerically using two decimal places. pH = √, aß, AE, Submit Hints My Answers Give Up Review Part reset shortcuts? help Part F Calculate the pH of a 0.10 M solution of HCI. Express your answer numerically using two decimal places. VD, αβ, ΔΣ, pH Submit reset shortcuts ? help Hints My Answers Give Up Review Part + 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 °C, [H3O+] = 10-7 M and pH = 7. As [H3O+] 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, K, as follows: K=1.0 × 10-¹4 = [H3O+][OH-] In the same way as the pH, we can define the pOH as pOH = -log[OH-]. It follows from the K, expression that pH + pOH = 14. Part B Calculate the pH of a 0.10 M solution of barium hydroxide, Ba(OH)2. Express your answer numerically using two decimal places. pH = Submit Hints My Answers Give Up Review Part Part D Part C Calculate the pH of a 0.10 M solution of NaOH. Express your answer numerically using two decimal places. 1945, αβ, ΔΣ, pH = Submit Γ' Ε, αβ, ΔΣ, reset shortcuts ? help pH = reset shortcuts ? help Hints My Answers Give Up Review Part Calculate the pH of a 0.10 M solution of hydrazine, N₂H₁. K₁, for hydrazine is 1.3 x 10-6. Express your answer numerically using two decimal places. [I'VD, αβ, ΔΣ, reset shortcuts ? help