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- 3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H;O*, CH;COO and CH;COOH at equilibrium. What is the pH of the solution? (Ka = 1.8x10) CH;COOH(aq) = CH;COO (aq) + H;O* (aq) a) Calculate the initial concentration of CH;COOH. (C:12; H:1; 0:16) b) Calculate the concentration of CH;CoO (aq) and H;O* (aq) at equilibrium. c) Calculate pH of the solution.2-11 2.19] A solution has an H+ concentration of 10-5 M. (a) What is the pH of this solution? (b) What is the pOH (Assume that the temperature of the solution is 25°C.) Answer: (a) 5 (b) 9 BM(a) Give the conjugate base of the following Brønsted–Lowry acids: (i) HIO3, (ii) NH4+. (b) Give the conjugate acidof the following Brønsted–Lowry bases: (i) O2-, (ii) H2PO4-.
- What is the conjugate base of boric acid, B(OH)3? (A) OH– (B) B(OH)4– (C) B(O)(OH)22– (D) B(H2O)(OH)2+Predict whether aqueous solutions of the following substances are acidic, basic, or neutral and write hydrolysis equations for the acidic and basic solutions. (a) CsBr; (b) Al(NO3)3; (c) KCN; (d) CH3NH3ClDetermine the pH of each of the following solutions.(a) 0.684 M hypochlorous acid (weak acid with Ka = 3e-08).(b) 0.399 M hydrogen peroxide (weak acid with Ka = 2.4e-12).(c) 0.751 M pyridine (weak base with Kb = 1.7e-09).
- 8) What is the pH of a 0.035 M HNO, solution? HNO3 (aq) + H,0 (1) H;O* (aq) + NO; (aq)COHSOH(ag) + H2On + CeHsO (aq) + H3O*(a9) Ka= 1.12 x 10-10 (a) Phenol is a weak acid that partially dissociates in water according to the equation above. Write the equilibrium-constant expression for the dissociation of the acid in water. (b) What is the pH of a 0.75 M CaHsOH(ag) solution? (C) For a certain reaction involving CaHsOH(ag) to proceed at a significant rate, the phenol must be primarily in its deprotonated form, C3H5O (eg). In order to ensure that the CsHsOH(aq) is deprotonated, the reaction must be conducted in a buffered solution. On the number scale below, circle each pH for which more than 50 percent of the phenol molecules are in the deprotonated form (CoHsO (aq). Justify your answer. 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Justification: (d) CeHsOH(ag) reacts with NaOH(ag). Write a net ionic equation representing this reaction (aka: invasion equation). (e) What is the pH of the resulting solution when 30 mL of 0.40 M CSH5OH(aq) is added to 25 mL of 0.60 M NAOH. Show all work…Ammonia, NH3, is amphoteric. (a) Give the formula for the conjugate acid of NH3. (b) Give the formula for the conjugate base of NH3.
- Determine the pH of each of the following solutions (Ka and Kb values can be found in the appendices of your textbook or online): (a) 0.045 M hypochlorous acid; (b) 0.0068 M phenol; (c) 0.080 M hydroxylamine.The compound methylamine is a weak base like ammonia. A solution contains 0.199 M CH;NH3* and 0.117 M methylamine, CH3NH2. The pH of this solution isDetermine the pH of each of the following solutions. (a) 0.134 M hypochlorous acid (weak acid with Ka = 3e-08). (b) 0.283 M hydrazoic acid (weak acid with Ka = 1.9e-05). (c) 0.879 M pyridine (weak base with Kb = 1.7e-09).
