1. 5x10 ^-4 M H ⁺ is equal to a pH of ________.

pH of 5.7 is equal to a [OH ^- ] of ___________M

[OH - ] = 2.9x10 ^-2 ; pOH = _________

0.025 M HCl; pH = ______________

2. What is the pH of a solution that is 0.34M in HOAc and 0.06 M in NaOAc?

3. Calculate the value of the equilibrium constant for the following reaction from the value of Ka=1.8x10 -5 for AcOH.

AcO - (aq) + H + (aq) = HOAc(aq)

4. What is the molar solubility of AgI ( Ksp = 8.3x10 -17 ) in .05 M NaI?

What are the equilibrium concentrations of I-, Na+, and Ag+ in the solutions?

5. At 2000 C, Kc = 4.1x10 -4 for

N2(g) + O2(g) = 2 NO(g)

If the equilibrium concentration of N2 is 0.01 M and of NO is 0.005 M, what is the equilibrium concentration of O2?

6. At 2000 oC, the Kc for the reaction:

N2(g) + O2(g) = 2 NO(g)

is 4.1x10-4. If the initial concentrations of N2 and O2 are 0.80 M and 0.20 M respectively, what is the equilibrium concentration of NO?

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What is the equilibrium concentration of O2?

7. Ammonia (or ammonia hydroxide) is dissolved in water to the extent of 0.08 M and ammonium chloride added to the same solution until its concentration is 0.02 M. What is the pH of this solution?

Kb of NH3 = 1.8x10^-5.

8. Sulfuric acid may be considered to be a strong diprotic acid. When a 0.035 moles of sulfuric acid, H2SO4, is dissolved in 1.00 L of water; what solute species are present and what are their concentrations?

9. a) What is the molecular formula and structure of acetic acid?

b) What reaction takes place when it is dissolved in water?

C) What is the molecular formula and structure of the acetate ion?

d) What reaction takes place when it is dissolved in water? 

10. a) What is the Lewis dot structure for the valance electrons of H2O?

b) What is the Lewis dot structure for the valance electrons of N2?