10. What is the hydrogen ion concentration of a solution with a pH of 10.33? d. 4.68 X 10-4 e. 2.14 X 10-11 f. 4.68 X 10-11 a. b. C. 11. The conjugate of a very weak base is a(n) Very weak acid Weak acid Strong acid a. b. C. 2.14 X 10-3 4.68 X 10-3 2.14 X 10-4 a. NaCl(aq) and NaOH(aq) b. NH3(aq and NH4Cl(aq) C. HNO3(aq) and NaNO3(aq d. e. f. 12. Which of the following pairs of chemicals could be used to produce a buffer solution? Choose ALL that apply. a. b. C. Very weak base Weak base Strong base d. Mg(OH)2(aq) and H3PO4 4(aq) 2- e. HCO3 (ag) and CO₂² (aq) f. HCl(aq) and HCO3¯(aq) 13. Which of the following contains two electrodes? Choose ALL that apply. Electrolytic Cell Galvanic Cell Oxidation Half-Cell d. Reduction Half-Cell Battery Electrolyte e. f.

10. What is the hydrogen ion concentration of a solution with a pH of 10.33? d. 4.68 X 10-4 e. 2.14 X 10-11 f. 4.68 X 10-11 a. b. C. 11. The conjugate of a very weak base is a(n) Very weak acid Weak acid Strong acid a. b. C. 2.14 X 10-3 4.68 X 10-3 2.14 X 10-4 a. NaCl(aq) and NaOH(aq) b. NH3(aq and NH4Cl(aq) C. HNO3(aq) and NaNO3(aq d. e. f. 12. Which of the following pairs of chemicals could be used to produce a buffer solution? Choose ALL that apply. a. b. C. Very weak base Weak base Strong base d. Mg(OH)2(aq) and H3PO4 4(aq) 2- e. HCO3 (ag) and CO₂² (aq) f. HCl(aq) and HCO3¯(aq) 13. Which of the following contains two electrodes? Choose ALL that apply. Electrolytic Cell Galvanic Cell Oxidation Half-Cell d. Reduction Half-Cell Battery Electrolyte e. f.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

The pK, for HCN(aq) is 9.21. What is the pH of a 1.245 M solution of NaCN? O a. 11.95 O b. 1.24 O c. 11.65 O d. 2.35 O e. 11.25
A solution is prepared by diluting 10.1 g HNO 3 (MW=63 g/mol) with water to a volume of 1.5 L. What is the pH of this solution? a. 2.24 b. -0.80 c. 0.97 d. 0.80 e. 1.83
13. What is the pH of a 0.0 1 5M Ca(OH)2 solution? a. 1.52 b. 12.18 c. 12.48 d. 1.82
13. If the pH of a 0.45 M ammonia solution is 11.73, what is the ionization percent of the base? А. 12.0% В. 4.3 % С. 1.2 % D. 11.73 % E. 7.0 %
If the pH of a solution is 3.65, what is the concentration of the [H'] ions? A. 1.23x10-5M O B. 2.24×104M C. 3.65x10-7M D. 4.47x10 11M
How is the equilibrium constant for a weak acid? A. Small B.Large C. neutral
Calculate the pH of a 0.35 M solution of pyridine (C5H5N; Kb = 1.7 x 10^-9) A. 4.61 B. 4.77 C. 9.39 D. 9.23 E. none of these
10. Calculate pH of a 0,45 M ammonia solution if the ionization percent is 1.2 %? A. 2.27 B. 1.57 C. 11.73 D. 0.35 E. 7.00
9. Trace the solution that has the lowest pH. A. 0.1 M HNO3 В. О.1 М Са(ОН)2 С. 0.1 М СНЗСООН D. 0.1 M CHзСОONa
What is the pH of .00055 M soln of NaOH? A. 3.3 B. 1.3 E-3 C. 10.7 D. 1.55 E-7
T he pH of aqueous 0.050M trimethylamine is 11.24, what is the K b of this base? Trimethylamine dissociates similar to ammonia in aqueous solutions. a. 6.6 x 10-22 b. 2.76 c. 6.3 x 10-5 d. 1.7 x 10-3 e. 5.8 x 10-12
Acids and Bases. Fill the missing.