Reference no: EM131550469

Question: 1. What is pH when when 2.0 mL of 2.00 M Ba(OH)2 is added to 10.0 mL of 1.00 M HNO3?

2. What is the pH when 2.00 mL of 0.200 M KOH is added to 10.0 mL of 0.100 M cinnamic acid, HC9H7O2 (Ka = 3.6 × 10-5)

3. Calculate the pH at the equivalence point when 10.0 mL of 0.100 M HC9H7O2 (Ka = 3.6 × 10-5) is titrated against 0.200 M KOH

4. Calculate the pH at half-equivalence point when 10.0 mL of 0.10 M HClO2 (aq) is titrated against 0.10 M NaOH(aq). The Ka of HClO2 is 0.012.

5. What is pH when 4.0 mL of 2.00 M Ba(OH)2 is added to 10.0 mL of 1.00 M HNO3 is titrated against ?

6. What is the pH when 4.0 mL of 2.00 M HCl is added to 10.0 mL of 1.00 M NH3 (Kb = 1.8 x 10-5)?

7. What is the pH at the half equivalence point 10.0 mL of 1.00 M NH3 (Kb = 1.8 x 10-5) is titrated against 2.00 M HCl?

8. What is the pH at the equivalence point 10.0 mL of 1.00 M NH3

9. The solubility of Calcium carbonate is 5.3 × 10-3g/L. Calculate its solubility product constant

10. Calculate the solubility in g/L for for Aluminum hydroxide (Ksp = 1.00 × 10-33)

11. Calculate the molar solubility of PbCl2 in 0.100 M NaCl(aq). The Ksp of PbCl2 is 1.6 × 10-5

12. Which of the following relationships between the solubility product constant (Ksp) & the molar solubility (X) is correct?

a. Fe(OH)3; Ksp=9X3

b. Ag2CrO4; Ksp=4X3

c. AlPO4; Ksp= 16X4

d. CaCO3; Ksp=27X4

13. Adding of which of the following will increase the solubility of LaF3

a. CaF2

b. NaCl

c. La(NO3)3

d. HNO3

14. Adding of which of the following will decrease the solubility of LaF3

a. CaF2

b. NaCl

c. La(NO3)3

d. HNO3

1. Which of the following cannot constitute a buffer?

a. Aniline (Kb = 4.3 x 10-10) & Anilinium chloride

b. HF & CaF2

c. HNO3 & NaNO3

16. Calculate pH of a buffer made of 0.050 M pyridine, C5H5N (Kb = 2.0 x 10-9) and 0.015 M pyridinium chloride

17. Calculate pH of a buffer made of 0.050 M phenol, HC6H5O (Ka = 1.0 x 10-10) and 0.015 M sodium phenolate, NaC6H5O

18. Calculate pH after the addition of 0.10 mole of NaOH to a 500 mL buffer made up of 0.500 M HF (Ka = 6.8 x 10-4) & 0.500 M NaF?

19. Calculate pH after the addition of 0.10 mole of HCl to a 500 mL buffer made up of 0.500 M HF (Ka = 6.8 x 10-4) & 0.500 M NaF?

(Kb = 1.8 x 10-5) is titrated against 2.00 M HCl?