Reactions involving Aqueous Solutions – WS1
1. Write correct formulas for the following and predict which of the following are soluble.
a. Silver carbonate d. Ammonium sulfate g. Rubidium iodide
b. Aluminum hydroxide e. Lead(II) acetate h. Potassium sulfate
c. Copper(I) chloride f. Aluminum nitrate i. Calcium hydroxide
2. Write the formulas and then indicate which of the following compounds are water soluble.
a. Magnesium chloride e. Manganese(II) h. Chromium(III) chloride
b. Magnesium hydroxide carbonate i. Lead(II) sulfate
c. Calcium phosphate f. Silver acetate
d. Lead(II) iodide g. Aluminum sulfate
3. Which ions could be regarded as universally soluble?
4. Distinguish between a solution which is an electrolyte and one which is not.
5. Distinguish between the term metallic conduction and electrolytic conduction.
6. Pure hydrogen chloride is considered to be a non-electrolyte. However, hydrogen chloride is a strong
electrolyte in an aqueous solution. Why?
7. Write dissociation equations for the following soluble salts:
a. KBr b. Ca(NO3)2 c. BaCl2 d. (NH4)2CrO4
8. The following compounds are electrolytes. Write dissociation equations and name each ion in the solution:
a. HI c. K2CO3 e. KNO3
b. CaCl2 d. Ba(OH)2 f. (NH4)2SO4
9. Write ionization equations for the following electrolytes:
a. Lithium hydroxide c. Potassium dichromate e. Ammonium sulfide
b. Nitric acid d. Sodium chlorate f. Sodium carbonate
10. What is the formula for each ion below?
a. Sulfate e. Carbonate i. Phosphate
b. Hydroxide f. Hydrogencarbonate j. Sulfite
c. Permanganate g. Ammonium k. Dichromate
d. Nitrate h. Chromate l. Hydrogensulfate
11. Write complete ionic equations for the reaction between each of the following pairs of solutions:
a. Barium nitrate and potassium sulfate d. Iron(III) nitrate and rubidium carbonate
b. Ammonium chromate and lead(II) nitrate e. Sodium sulfide and lead(II) acetate
c. Aluminum chloride and sodium hydroxide
12. Write net ionic equations for the following reactions that occur:
a. Potassium hydroxide and aluminum chloride d. Aluminum bromide and sodium carbonate
b. Iron(III) sulfate and sodium sulfide e. Sodium chromate and magnesium chloride
c. Bismuth(III) nitrate and ammonium
13. Write net ionic equations for the reactions that occur:
a. Sodium chloride and lead(II) nitrate e. Silver nitrate and calcium acetate
b. Aluminum sulfate and sodium hydroxide f. Ammonium sulfide and manganese(II)
c. Potassium sulfate and barium chloride chloride
d. Sodium phosphate and calcium nitrate
14. What ion(s) could be present in a solution if samples of it gave a precipitate when:
a. Either Cl- or SO42- is added c. SO42- is added but none when Cl- is added
b. Cl- is added but non when SO42- is added
15. What would you expect to see when a solution of sodium sulfate is mixed with a solution of magnesium sulfate?
16. A solution contains Ag+, Cu2+, Fe2+, and Ca2+ ions.
a. Some sodium bromide is added to this solution. Write the net ionic equation for the precipitate(s) that form.
b. The remaining liquid in (a) is separated by filtration. To this liquid, sodium sulfide solution is added. Write
the net equation for the reaction that takes place.
c. To the remaining liquid some sodium carbonate is added and a precipitate forms. Write a net ionic equation
for this reaction.
17. Calculate the molar concentration of the ions from the following strong electrolytes:
a. 0.10 mol of iron(III) chloride is dissolved in 500 mL of solution
b. 0.20 mol of ammonium chlorate is dissolved in 100 mL of solution
18. If 0.50 mol of strontium iodide is completely dissociated in 400 mL of solution, what is the concentration of each
19. If 20.0 g of sodium sulfate is fully dissociated in 2.0 x 10-1 L of solution, what is the concentration of each ion?
20. You dissolve 8.6 g of calcium chloride in a solution whose volume is 0.25 L. Calculate the concentration of each
ion in solution.
21. If 250 mL of solution contains 32.0 g of barium hydroxide, what is the concentration of each ion in the solution?