CH 102 1st EditionExam # 3 Lectures: 13-18Practice Test!At equilibriuma. the reaction stops.b. ΔG < 0c. ΔG > 0d. the reaction is first order in concentration of reactant.e. the rate of the reaction in the forward direction is equal to the rate of the reaction in the reverse direction.2, Antimony pentachloride decomposes in the gas phase at 448 °C to give antimony trichloride and chloride.SbCl5 (g) → SbCl3 (g) + Cl2 (g)An equilibrium mixture in a 5.00 L vessel contains 3.84 g of antimony pentachloride, 9.14 g of antimony trichloride and 2.84 g chlorine. What is the value of the equilibrium constant, Kc, at 448 °C?a. Kc = 1.35 b. Kc = 0.00145c. Kc = 0.0250 d. Kc = 0.290e. Kc = 6.763 At 700 K the thermal decomposition of sulfur trioxide has a Kp value of 3.3 x 10-5. What is the value of Kc for this reaction at 700 K?2 SO3 (g) ↔ 2 SO2 (g) + O2(g)a. Kc = 3.3 x 10-5b. Kc = 3.0 x 104c. Kc = 1.9 x 10-3d. Kc = 1.7 x 106e. Kc = 5.7 x 10-74 The thermal decomposition of phosgene at 600 K gives carbon monoxide and chloride.COCl2 (g) ↔ CO (g) + Cl2 (g)A reaction mixture initially contains 1.6 M COCl2. Determine the equilibrium concentration of CO if Kc for the reaction is 8.33 x 10-4. a. 2.1 x 10-2 M b. 3.7 x 10-2 Mc. 1.5 x 10-3 M d. 4.2 x 10-4 Me. 1.3 x 10-3 M5. What effect will removing NO2 have on the equilibrium?SO2 (g) + NO2 (g) ↔ SO3 (g) + NO (g)a. The reaction will shift to the right.b. The reaction will shift to the left.c. The equilibrium constant will decrease.d. The reaction will shift to decrease the pressure.e. No change will occur.6. Which of the following is a strong acid?a. acetic acid, pKa = 4.74b. potassium nitratec. ammoniad. sodium fluoridee. perchloric acid7. What is the pH of a 5.43 x 10-3 M solution of nitric acid in water?a. 4.53 b. 1.34c. 5.43 d. 2.27e. 7.00 8. If 50 mL of a 5.43 x 10-3 M solution of perchloric acid in water is mixed with 10 mL of a 1.34 x 10-2 M solution of potassium hydroxide in water, what is the pH of the mixture?a. 1,91 b. 12.73c. 2.64 d. 1.34e. 12.139. Which is the strongest acid? a. Acetic acid, pKa = 4.74b. Formic acid, pKa = 3.75c. Boric acid, pKa1 = 9.14d. hydrocyanic acid, pKa = 9.31e. Phenol, pKa = 9.8910. Which is the strongest base? a. Ammonia, pKb = 4.75b. Aniline, pKb = 9.37c. triethylamine, pKb = 4.74d. pyridine, pKb = 8.75e. piperidine, pKb = 2.8811. What is the pH for a 2.75 x 10-3 molar solution of barbituric acid in water? The value of Ka for barbituric acid is 9.82 x 10-5. a. pH = 5.12 b.pH = 4.01c.pH = 3.41d.pH = 2.51e. pH = 3.3312. What is the pH of a 2.75 x 10-3 M solution of potassium fluoride, KF, in water? The Ka for hydrofluoric acid is 3.55 x 10-5. a. pH = 7.94 b.pH = 9.55c.pH = 5.90d.pH = 4.75e. pH = 4.4513. Which solution is most basic?a. 0.10 M lithium hydroxideb. 0.10 M sodium acetatec. 0.10 M sodium nitrated. 0.10 M ammonium chloridee. 0.10 M hydrochloric acid14. Which of the following solutions is a good buffer system?a.A solution that is 0.10 M acetic acid and 0.10 M lithium acetateb.A solution that is 0.10 M hydrogen fluoride and 0.10 M sodium acetatec.A solution that is 0.10 M hydrogen chloride and 0.10 M ammonium chlorided. A solution that is 0.10 M sodium hydroxide and 0.10 M potassium hydroxidee. None of the above are buffer systems.15. If the pKa of formic acid, HCHO2, is 3.74 and the pH of a solution containing a mixture of formic acid (HCHO2)and sodium formate (NaCHO2) solution is 3.11, which of the following is TRUE?a. [HCHO2] < [NaCHO2]b. [HCHO2] = [NaCHO2]c. [HCHO2] << [NaCHO2]d. [HCHO2] > [NaCHO2]e. It is not possible to make a buffer of this pH from HCHO2 and NaCHO2.16. You wish to prepare an acetic acid, HC2H3O2, buffer with a pH of 4.24. If the pKa of is 4.74, what ratio of potassium acetate to acetic acid (C2H3O2⁻/ HC2H3O2) must you use?a. 0.10 b. 0.50 c. 0.32d. 2.0 e. 2.817. Calculate the pH of a buffer that is 0.020 M HF and 0.040 M LiF. The Ka for HF is 3.5 × 10-4.a. 2.06 b. 3.76 c. 3.46d. 4.86 e. 3.1618. A 1.0 L buffer solution is 0.250 M HC2H3O2 and 0.050 M LiC2H3O2. Which of the following actions will destroy the buffer?a.adding 0.050 moles of LiC2H3O2b.adding 0.050 moles of HC2H3O2c. adding 0.055 moles of HCld. adding 0.055 moles of NaOHe. None of the above will destroy the buffer.19. Which of the following compounds will have the highest molar solubility in pure water?a.PbSO4, Ksp = 1.82 × 10-8b.MgCO3, Ksp = 6.82 × 10-6c.AgI, Ksp = 8.51 × 10-17d.PbS, Ksp = 9.04 × 10-29e.FeS, Ksp = 3.72 × 10-1920. Determine the molar solubility of lead sulfate, PbSO4, (Ksp = 1.82 × 10-8) in pure water.a. 1.82 × 10-8 Mb. 1.35 × 10-4 Mc. 9.1 × 10-9 Md. 3.31 × 10-16 Me. 4.48 × 10-4 M21. Determine the molar solubility of Fe(OH)2 in pure water. The Ksp for ferrous hydroxide is 4.87 × 10-17.a. 2.44 × 10-17 Mb. 1.62 × 10-17 Mc. 4.03 × 10-9 Md. 3.65 × 10-6 Me. 2.30 × 10-6