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1) [A] In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a BrønstedLowry base. F - + HCO3 - HF (aq) + CO3 2- BrønstedLowry _____acidbase BrønstedLowry _____acidbase BrønstedLowry _____acidbase BrønstedLowry _____acidbase In this reaction: The formula for the conjugate _____acidbase of F - is------ The formula for the conjugate _____acidbase of HCO3 - is------- [B] In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a BrønstedLowry base. CH3COO- + HS- CH3COOH + S 2- BrønstedLowry _____acidbase BrønstedLowry _____acidbase BrønstedLowry _____acidbase BrønstedLowry _____acidbase In this reaction: The formula for the conjugate _____acidbase of CH3COOis ---- The formula for the conjugate _____acidbase of HSis-------- [C] In the following net ionic equation, identify each species as either a Brønsted-Lowry acid or a Brønsted-Lowry base. HCO3 - + HClO H2CO3 (aq) + ClOBrønstedLowry_____acidbase BrønstedLowry_____acidbase BrønstedLowry_____acidbase BrønstedLowry_____acidbase In this reaction: The formula for the conjugate _____acidbase of HCO3 - is The formula for the conjugate _____acidbase of HClO is (2) [A] The pH of an aqueous solution at 25°C was found to be 13.00. The pOH of this solution is----------- . The hydronium ion concentration is ----- M. The hydroxide ion concentration is-------M [B] The pOH of an aqueous solution at 25°C was found to be 13.00. The pH of this solution is------------ . The hydronium ion concentration is ----- M. The hydroxide ion concentration is ------ M. [C] The hydroxide ion concentration in an aqueous solution at 25°C is 9.4×10-2 M. The hydronium ion concentration is------- M. The pH of this solution is------------ . The pOH is------------ . (3) [A] What is the hydronium ion concentration in an aqueous hydroiodic acid solution with a pH of 2.920? [H3O+ ] =------------ M [B] What is the hydronium ion concentration in an aqueous hydrobromic acid solution that has a pOH of 9.700? [H3O+ ] =----------- M [C] What is the pOH of an aqueous solution of 0.468 M hydrochloric acid? pOH =------------ (4) [A] What is the pH of an aqueous solution of 8.43×10-2 M sodium hydroxide? pH =-------------. [B] What is the pOH of an aqueous solution of 8.42×10-2 M barium hydroxide? pOH = ------------. [C] What concentration of sodium hydroxide is needed to give an aqueous solution with a pOH of 1.370? Molarity of sodium hydroxide =--------- M (5) [A] Write the Ka expression for an aqueous solution of hydrocyanic acid: (Note that either the numerator or denominator may contain more than one chemical species. Enter the complete numerator in the top box and the complete denominator in the bottom box. Remember to write the hydronium ion out as H3O + , and not as H + ) Ka = ______. [B] Write the Ka expression for an aqueous solution of hydrofluoric acid: Ka = _____ [C] Write the Ka expression for an aqueous solution of acetic acid: Ka = ___ (6) [A] The compound trimethylamine, (CH3)3N, is a weak base when dissolved in water. Write the Kb expression for the weak base equilibrium that occurs in an aqueous solution of trimethylamine Ka = ____ [B] The compound dimethylamine, (CH3)2NH, is a weak base when dissolved in water. Write the Kb expression for the weak base equilibrium that occurs in an aqueous solution of dimethylamine: Ka = ____ [C] The compound ammonia, NH3, is a weak base when dissolved in water. Write the Kb expression for the weak base equilibrium that occurs in an aqueous solution of ammonia: (7) [A] Ka for acetylsalicylic acid (aspirin), HC9H7O4, is 3.00×10-4 . Ka for benzoic acid, C6H5COOH, is 6.30×10-5 . Ka for nitrous acid, HNO2, is 4.50×10-4 . What is the formula for the strongest conjugate base? [B] Ka for benzoic acid, C6H5COOH, is 6.30×10-5 . Ka for hydrocyanic acid, HCN, is 4.00×10-10 . Ka for hydrofluoric acid, HF, is 7.20×10-4 . What is the formula for the strongest conjugate base? [C] Ka for hydrofluoric acid, HF , 7.20 x 10^-4 is-------- . Ka for nitrous acid,HNO2 ,4.50x10^-4 is_______ . Ka for formic acid, CHOOCH,1.85x10^-4 is____ . What is the formula for the strongest acid? (8) [A] The value of Ka for acetylsalicylic acid (aspirin) is 3.00×10-4 . What is the value of Kb, for its conjugate base, C9H7O4 - ? ----------? [B] The value of Ka for benzoic acid is 6.30×10-5 . What is the value of Kb, for its conjugate base, C6H5COO- ----------? [C] The value of Ka for hydrofluoric acid is 7.20×10-4 . What is the value of Kb, for its conjugate base, F - ? -------------? (9) [A] n the laboratory, a general chemistry student measured the pH of a 0.581 M aqueous solution of hydrocyanic acid to be 4.832. Use the information she obtained to determine the Ka for this acid. Ka(experiment) = --------------. [B] In the laboratory, a general chemistry student measured the pH of a 0.581 M aqueous solution of benzoic acid, C6H5COOH to be 2.205. Use the information she obtained to determine the Ka for this acid. Ka(experiment) =-------------. [C] In the laboratory, a general chemistry student measured the pH of a 0.581 M aqueous solution of hypochlorous acid to be 3.860. Use the information she obtained to determine the Ka for this acid. Ka(experiment) =-------------. (10) [A] The hydronium ion concentration of an aqueous solution of 0.58 M benzoic acid, C6H5COOH is [H3O + ] = -------M [B] The hydroxide ion concentration of an aqueous solution of 0.581 M hypochlorous acid is [OH- ] =--------M. [C] The pOH of an aqueous solution of 0.581 M formic acid, HCOOH is . (11) [A] In the laboratory a student measures the percent ionization of a 0.581 M solution of hydrocyanic acid to be 2.54×10-3 %. Calculate value of Ka from this experimental data. Ka = --------. [B] In the laboratory a student measures the percent ionization of a 0.581 M solution of benzoic acid , C6H5COOH to be 1.07 %. Calculate value of Ka from this experimental data. Ka =---------. [C] Calculate the percent ionization of a 0.549 M solution of hydrofluoric acid. % Ionization =--------- % (12) [A] The hydronium ion concentration of an aqueous solution of 0.581 M caffeine (a weak base with the formula C8H10N4O2) is [H3O + ] = ------ M. [B] The hydroxide ion concentration, [OH- ], of an aqueous solution of 0.581 M dimethylamine (a weak base with the formula (CH3)2NH) is-----------M. [C] The pOH of an aqueous solution of 0.581 M caffeine (a weak base with the formula C8H10N4O2) is ------ (13) [A] The pH of an aqueous solution of 0.581 M hydrocyanic acid is -------- [B] The pOH of an aqueous solution of 0.581 M benzoic acid, C6H5COOH is----------- [C] The hydroxide ion concentration of an aqueous solution of 0.581 M hypochlorous acid is [OH- ] = --------M.

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