1. The document provides 7 chemistry problems involving calculations of pH, concentrations of products and reactants from acid-base reactions involving strong acids and bases, and identification of types of acids. 2. Problems 1-3 involve calculating the pH of strong acid solutions given molar concentrations. 3. Problems 4-6 require using given volumes, molarities, and extent of ionization to calculate concentrations of products and reactants. 4. Problems 7-9 ask about common weak bases, relationships between types of acids, and identification of more acidic salt solutions.

1. GENERAL CHEMISTRY-II (1412)
S.I. # 24
Calculate the pH of each of the following strong acid solutions:
1. 0.00835 M HNO3
2. 0.525 M HClO4
3. 5.00 mL of 1 M HCl diluted to 0.500 L
4. a mixture formed by adding 50.0 mL of 0.020 M HCl to 150 mL of
0.010 M HI.
5. A 0.100 M solution of brmoacetic acid (BrCH2COOH) is 13.2% ionized.
Calculate [H+] , [BrCH2COO-], and [BrCH2COOH].

2. 6. How many moles of HF (Ka = 6.8 x 10-4) must be present in 0.200 L to form a
solution with a pH of 3.25?
7. What are tow kinds of molecules or ions that commonly function as weak bases?
8. If a substance is a Lewis acid, is it necessarily a Bronsted-Lowery acid? Is it
necessarily an Arrhenius acid? Explain.
9. Which member of each pair produces the more acidic aqueous solution:
a. ZnBr2 or CdCl2
b. CuCl or Cu(NO3)2
c. Ca(NO3)2 or NiBr2