Review of Solubility Equilibrium
1. Identify each of the following as ionic or molecular substance: a. NaCl(aq) ________________________________
b. CH3COOH(aq) ___________________________
c. CCl4(l) _________________________________
d. HNO3(aq) ______________________________
e. C2H6(l) ________________________________
2. A good way to test a liquid to see if it contains ions is to :
3. Define a saturated solution.
4. Define an unsaturated solution.
5. What is meant by solubility?
6. On the “Solubility Table” what, precisely, does the word soluble mean?
7. If 25.0 mL of 0.90 M HCl is added to 125.0 mL of water, what is the final [HCl]?
8. Calculate the [Fe3+] in a 0.25 M solution of Fe2(SO4)3?
9. Calculate the [Na+] in a 0.55 M solution of sodium acetate. (Write the proper formula for sodium acetate first). 10. Calculate the [Na+] in a 0.55 M solution of sodium carbonate. (Write the proper formula for sodium carbonate first.)
11. Calculate the [Na+] in a 0.55 M solution of sodium phosphate. (Write the proper formula for sodium carbonate first.)
12. 300 mL of 0.500 M NaCl is mixed with 400 mL of 0.200 M HCl. Calculate the final total [Cl-].
13. 200 mL of 0.500 NaCl is mixed with 300 mL of 0.200 M CaCl2. Calculate the final total [Cl-].
14. An aqueous solution of Pb(NO3)2 is mixed with an aqueous solution of KBr and a precipitate forms. a. Write a balanced formula equation for this reaction.
b. Write a balanced total ionic equation for this reaction.
c. Write a balanced net ionic equation for this reaction.
15. Devise a procedure to separate the ions in a mixture which contains the following sets of ions. Be specific about what you add and what happens when you add it. Remember, you cannot add single ions, only compounds or aqueous solutions of the compounds. a. Ba2+, Mg2+ and Na+
b. Ag+, Cu2+ and Mg2+
16. Complete the balanced dissociation equation and write the Ksp equation for...
Please join StudyMode to read the full document