1. GENERAL CHEMISTRY-I (1411)
S.I. # 17
1. Write the balanced molecular AND net ionic equations for each of the following
neutralization reactions:
a. Aqueous acetic acid neutralized by aqueous potassium hydroxide
b. Solid chromium(III) hydroxide reacting with nitric acid
c. Aqueous hypochlorous acid and aqueous calcium hydroxide react
2. Define the following:
a. Oxidation:
b. Reduction:
c. Concentration:
d. Molarity:
e. Indicator:
3. Can oxidation occur without accompanying reduction?
4. Determine the oxidation number for the indicated element in each of the
following compounds:
a. Ti in TiO2 ________ b. Sn in SnCl3 ________
c. C in C2O42- ________ d. N in N2H4 ________
e. N in HNO2 ________ f. Cr in Cr2O7 2- ________
5. Which of the following are re-dox reactions? For those that are, indicate which
element is oxidized and which is reduced. For those that are not, indicate whether
they are precipitation or acid base reactions.
a. Cu(OH)2 (s) + 2HNO3 (aq)  Cu(NO3)2 (aq) + 2H2O (l)

2. b. Fe2O3 (s) + 3CO (g)  2Fe (s) + 3CO2 (g)
c. Sr(NO3)2 (aq) + H2SO4 (aq)  SrSO4 (s) + 2HNO3 (aq)
d. 4 Zn (s) + 10 H+ (aq) + 2 NO3- (aq)  4 Zn2+ (aq) + N2O (g) + 5 H2O (l)
6. a. Calculate the molarity of a solution made by dissolving 0.145 mol Na2SO4 in
enough water to form exactly 750 mL of solution. b. How many moles of KMnO4
are present in 125 mL of a 0.0850 M solution? c. How many milliliters of 11.6 M
HCl solution are needed to obtain 0.255 moles of HCl?
8. a. How many grams are present in 50.0 mL of 0.360 M K2Cr2O7? b. If 4.28 g of
(NH4)2SO4 is dissolved in enough water to form 300 mL of solution, what is the
molarity of the solution? c. How many mL of 0.240 M CuSO4 contain 2.25 g of
solute?
9. Indicate the concentration of each ion present in the solution formed by mixing
a) 16.0 mL of 0.130 M HCl and 12.0 mL of 0.600 M HCl, b) 18.0 mL of 0.200 M
Na2SO4 and 15.0 mL of 0.400 M CaCl2 solution.