Honors Chemistry: Acid/Base Q-Set : Name:______

1. Name the following:

H2S:______HClO2:______

H2C2O4:______H3PO4:______

2. Give formulas for the following:

Hydrophosphoric acid:______sulfurous acid:______

Nitrous acid:______chromic acid:______

3.a) Write out the following reaction: hydrochloric acid reacts with gaseous ammonia to produce a solution of ammonium chloride.

b) Write the net ionic equation for the reaction above.

4.a) Write out the following reaction: a solution of sulfuric acid reacts with aqueous barium hydroxide to produce water and a solid precipitate of barium sulfate.

b) Write the net ionic equation for the reaction above.

5. What is the [H+] in a 0.50 M Ba(OH)2 solution?

6. What is the [OH-] in a 0.045 M hydrobromic acid solution.

7. What is the pH of a 2.3 x 10-4 M HCl solution?

8. What is the pH of a solution containing a [OH-] of 1.9 x 10-3M?

9. What is the [H+] of solution with a pH of 8.15 ? What is the pOH of this solution?

10. What is the pH of a 3.0 M NH3 solution? (Kb = 1.8 x 10-5)

11. What is the pH of a 1.15 M hydroazoic acid solution (HN3) ? (Ka = 1.9 x 10-5)

12. A solution of HF has a pH of 3.3. What is the [HF] if its Ka = 6.8 x 10-4 ?

13. A. Calculate the pH of a buffer system (1 liter) made up of a 0.600 M HC2H3O2 and a 0.650 M NaC2H3O2 solution.

(Ka= 1.74 x 10-5)

B. What will the pH of this system be if 0.105 mol of HCl is added?

14. An acid solution has a H+ concentration of 0.005 M. If methyl yellow was added to this solution, what color would it be? What about methyl orange? SHOW WORK

Indicator / pH range / Color below range / Color above range
Methyl Yellow / 2.9-4.0 / yellow / blue
Methyl Orange / 3.2-4.4 / red / yellow

Methyl Yellow:______Methyl Orange:______

15. In a titration experiment, a team of students found that 15.5 mls of a 0.35 M NaOH solution was required to completely neutralize 55.0 mls of a solution of H2SO4. Calculate the molarity of the acid solution.

16. What are the conjugate bases of the following:

H2SO4

HF

HC2H3O2

HSO3-

17. Identify conjugate acid-base pairs; label everything as either a B-L acid or a B-L base, and predict which direction it will proceed in:

H2PO4- + C2H3O2- ÜÞ HC2H3O2 + HPO42-

18. Compare and contrast Arrhenius’s definitions for acids and bases with Bronsted-Lowry definitions for acids and bases. Explain why the compound CH3NH2 is a B-L base, but wouldn’t be considered an Arrhenius base.

19. Do the following salts make acidic, basic or neutral solutions?:

a) NH4Br:______c) NaNO2:______

b) KNO3:______d) MgCl2:______

20. What is the concentration of H+ in each of the acids below:

2.0M HC2H3O2 Ka= 1.8 x 10-5

2.0M HNO3 Ka= very large

2.0 M H2C6H7O6 Ka1= 8.0 x 10-5 Ka2 = 1.6 x 10-12

21. You have a buffer system (assume 1.00 L) made of 0.78M formic acid (HCHO2) and 0.60M sodium formate (NaCHO2). The Ka for HCHO2 is 1.78 X 10-4.

(a) Calculate its pH.

(b) Calculate its pH after 0.10 mol HCl(g) is bubbled into it.