Name:

1. What information is provided by a balanced chemical equation?

2. Name two acids that are strong electrolytes and one that is a weak electrolyte. Name two
    bases that are strong electrolytes and one that is a weak electrolyte (Place answers in the
    chart below).

3. Balance the following equations:

4. Which compound or compounds  in each of the following groups is (are) expected to be
     soluble in water?

(a) Select From Below Iron(II) oxide Iron(II) chloride Iron(II) carbonate          (b) Select From Below Silver(I) iodide Silver(I) phosphate Silver(I) nitrate           (c) Select From Below Sodium chloride Lithium carbonate Potassium permanganate

5. Give the formula for:

6. Name two water-soluble and two water-insoluble compounds containing Cu⁺² ions.

     Water soluble:    Water insoluble:

7. Oxalic acid. which is found in certain plants, can provide two hydrogen ions in water.
     Write balance equations (like those for sulfuric acid on page 172) to show how oxalic
     acid can supply one and then a second hydrogen ion.

8. Write a balanced equation for the reaction between magnesium oxide and water and between
    nitrogen dioxide and water. Identify the acetic and basic anhydride.

9. Balance each of the following equations and then write the net ionic equation:

(a) Zn(s)  +  HCl(aq)  --->  H₂(g)  +  ZnCl₂(aq)
     Net ionic equation:

(b) Mg(OH)₂(s)  +  HCl(aq)  --->  MgCl₂(aq)  +  H₂O(l)
     Net ionic equation:

(c) HNO₃(aq)  +  CaCO₃(s)  ---> Ca(NO₃)₂(aq)  +  H₂O(l)  +  CO₂(g)
    

41. Balance these equations and then classify them as acid/base, precipitation, or
     gas forming reactions.

(a) K₂CO₃(aq)  +  Cu(NO₃)₂(aq)  ---->  CuCO₃(s)  +  KNO₃(aq)
     Classification:

(b) Pb(NO₃)₂(aq)  +  HCl(aq)  ---->  PbCl₂(s)  +  HNO₃(aq)
     Classification:

(c) MgCO₃(s)  +  HCl(aq)  ---->  MgCl₂(aq)  +  H₂O(l)  +  CO₂(g)
     Classification:

10. Predict the products of each of the precipitation reactions below and then
     balance. Identify the precipitate.

(a) NiCl₂(aq)  +  (NH₄)₂S(aq)  ---->
    

(b) Mn(NO₃)₂(aq)  +  Na₃PO₄(aq) ---->
    

51. Complete and balance the following acid/base reactions. Name the reactants and
      products.

(b) HClO₄(aq)  +  NH₃(aq)  ---->
    

11. The following reaction can be used to prepare iodine in the laboratory (see photo).
      Determine the oxidation numbers for each atom in the following equation:

      2NaI(s)  +  2H₂SO4(aq)  + MnO₂(s) ---->  Na₂SO₄(aq)  +  MnSO₄(aq)  +  I₂  + 2H₂O(l)

12. Vitamin C is the simple compound C₆H₈O₆. One method for determining the amount of
      vitamin C in a sample is to react the sample with bromine, Br₂.

        C₆H₈O₆(aq)  +  Br₂(aq)  ---->  2HBr(aq)  + C₆H₆O₆(aq)

      What is being oxidized and reduced in the above reaction? What is the oxidizing agent
      and reducing agent?

 13. Describe how you would prepare 300.0 ml of 0.500 M K₂Cr₂O_7.

14. If it takes 38.55 ml of 0.120 M HCl to titrate  50.0 ml Na₂CO₃, according to 
     the following equation, what is the molarity of Na₂CO₃?

            Na₂CO₃(aq)  +  2HCl(aq)  --> 2NaCl(aq)  +  CO₂(g)  +  H₂O(l)

15. Calculate the pH of a solution of 0.150 M H₂SO₄.

16. What is the hydrogen ion concentration in a solution with a pH of 4.59?