1. Please, consider saturated sodium chloride solution, NaCl(aq). Quite a bit of sodium chloride can be dissolved in water, about 6 moles/L. The number of moles of ions in the solution is ....
a. 0 M
b. 3 M
c. 6 M
d. 9 M
e. 12 M
2. In the saturated solution of NaCl, the type of particles in the solution is (are) ....
d. atoms and ions
e. molecules and ions
3. What happens if we increase the concentration of Cl- by adding some concentrated hydrochloric acid (12M HCl)?.
a. the number of Cl- ions increases
b. there is a less saturated solution
c. all of ions are still in the saturated solution
d. NaCl crystal is produced
e. all ions precipitate to form crystal
4. The solubility of NaCl in water at room temperature is ....
a. 1 moles/L
b. 3 moles/L
c. 6 moles/L
d. 9 moles/L
e. 12 moles/L
5. To determine the solubility of solute in water, a solution must be prepared that is ….
6. Which condition is essential to prepare a saturated solution of an ionic salt?
a. excess solute
b. any amount of solute
c. any amount of solvent
d. a temperature of 250C
e. a fixed volume of solvent
7. The solubility of a solute is best determined from which type of solution?
a. Any solution at 250C
b. A saturated solution
c. An unsaturated solution
d. A supersaturated solution
e. A concentrated solution
8. Molecular solutions do not conduct electricity because they contain ….
a. molecules only
b. cations and anions
c. molecules and anions
d. molecules and cations
9. Which of the solutes below is both ionic and most soluble?
10. Which of the solutes below is molecular?
11. Which one of the following would form an ionic solution when dissolved in water?
12. Which of the solutes below can form an ionic solution with the highest conductivity?
13. Which of the following solutes will produce a molecular solution?
14. In a 500 mL sample of 0.020 M K3PO4, the [PO43-] is ….
a. 0.005 M
b. 0.010 M
c. 0.020 M
d. 0.030 M
e. 0.040 M
15. What is the [Cl-] when 1.50 g of NaCl is dissolved in enough water to make 1000. mL of solution?
a. 0.0150 M
b. 0.0128 M
c. 0.0256 M
d. 0.330 M
e. 0.0390 M
16. What is the concentration of the ions in 3.0 L of 1.0 M Al2(CO3)3 ?
a. 0.33 M 0.50 M
b. 0.66 M 1.0 M
c. 2.0 M 3.0 M
d. 3.0 M 4.5 M
e. 3.5 M 5.0 M
17. In an experiment, 0.500 mol of Fe(NO3)3 is dissolved in water to produce a 2.00L solution. The [NO3-] in this solution is ….
a. 0.250 M
b. 0.500 M
c. 0.750 M
d. 1.50 M
e. 2.00 M
18. What will be the [Cl-] when equal volumes of 0.10 M MgCl2 and 0.30 M AlCl3 are combined?
a. 0.30 M
b. 0.35 M
c. 0.55 M
d. 0.90 M
e. 1.10 M
19. Which value best represents the total ion concentration when 0.10 moles of K3PO4 is present in 0.5 L of solution?
a. 0.1 M
b. 0.2 M
c. 0.4 M
d. 0.6 M
e. 0.8 M
20. In 1.5 M (NH4)2SO4 , the ion concentrations are ….
a. [NH4+]=0.75M and [SO42-]=0.75M
b. [NH4+] =1.5M and [SO42-] =1.5M
c. [NH4+] = 1.5M and [SO42-]=3.0M
d. [NH4+] =3.0M and [SO42-]=1.5M
e. [NH4+] = 3.0M and [SO42-]=3.0 M
21. The equation that represents the equilibrium in a saturated solution of Fe2(SO4)3 is ….
b. Fe2(SO4)3(s)⇄ 2Fe2+(aq)+3SO42-(aq)
c. Fe2(SO4)3(s)⇄ 3Fe3+(aq)+2SO42-(aq)
22. Which of the following represents the equilibrium in a saturated solution of Cr2(SO4)3?
a. Cr2(SO4)3(s) ⇄ Cr2+(aq) + SO43-(aq)
b. Cr2(SO4)3(s) ⇄ Cr3+(aq) + SO42-(aq)
c. Cr2(SO4)3(s) ⇄ 2Cr2+(aq)+3SO43-(aq)
d. Cr2(SO4)3(s) ⇄2Cr3+(aq)+3SO42-(aq)
23. Which of the following is commonly used to describe the solubility of a solute?
a. mass of solute/moles of solute
b. moles of solution/mass of solute
c. mass of solute/volume of solution
d. mass of solution/volume of solutee. moles of solution/volume of solvent
24. Which of the following units is commonly used to describe solubility?
25. Which of the following would best describe the solubility of a solute?
a. litres per gram
b. moles per litre
c. grams per mole
d. grams per seconde. moles per grams
26. The Ksp expression for a saturated solution of Ca3(PO4)2 is ….
a. Ksp = [Ca2+][PO43-]
b. Ksp = [Ca2+]3[PO43-]2
c. Ksp = [Ca2+]2[PO43-]3
d. Ksp = [3Ca2+][2PO43-]
e. Ksp = [3Ca2+]3[2PO43-]2
27. The Ksp expression for calcium hydroxide is ….
a. Ksp = [Ca2+][OH-]2
b. Ksp = 1 / [Ca2+][OH-]2
c. Ksp = [Ca2+][2OH-]2
d. Ksp = 1 / [Ca2+][2OH-]2
28. If equal volumes of 0.2 M KBr and 0.2M FeSO4 are mixed, then ….
a. no precipitate will be observed
b. a precipitate of FeBr2 will be observed
c. a precipitate of K2SO4 will be observed
d. a precipitate of both K2SO4 and FeBr2 will be observed
29. Which of the following occurs when equal volumes of 0.20 M MgS and 0.20 M ZnSO4 are mixed?
a. A precipitate does not form
b. A precipitate of ZnS forms
c. A precipitate of MgSO4 forms
d. Precipitates of MgSO4 and ZnS form
30. What will happen when equal volumes of 0.20 M (NH4)2S(aq) and 0.20 M Sr(OH)2(aq) are mixed?
a. SrS precipitates.
b. NH4OH precipitates.
c. Both NH4OH and SrS precipitate.
d. No precipitate forms.
31. The complete ionic equation for the reaction between MgCl2(aq) and AgNO3(Aq) is ….
a. Ag+(aq) + Cl-(aq) → AgCl(s)
b. 2AgNO3(aq) + MgCl2(aq) → 2AgCl(s) + Mg(NO3)2(aq)
c. 2Ag+(aq)+Mg2+(aq)+2NO3-(aq) +2Cl-(aq) → MgCl2(s) + 2Ag+(aq)+2NO3-(aq)
d. 2Ag+(aq)+2NO3- (aq) +Mg2+(aq)+2Cl-(aq) → 2AgCl(s) + Mg2+(aq)+ 2NO3- (aq)
32. A precipitation reaction occurs when equal volumes of 0.2 M Pb(NO3)2 and 0.2 M KI are mixed. The net ionic equation for this reaction is ….
a. Pb2+(aq) + 2I-(aq) → PbI2(s)
b. PbI2(s) → Pb2+(aq) + 2I-(aq)
c. K+(aq) + NO3-(aq) → KNO3(s)
d. KNO3(s) → K+(aq) + NO3-(aq)
e. Pb(NO3)2(s) → Pb2+(aq) + NO3- (aq)
33. Which equation represents the correct reaction between Na2CO3 and Ba(NO3)2?
a. Na+(aq) + NO3-(aq) → NaNO3(s)
b. Ba2+(aq) + CO32-(aq) → BaCO3(s)
c. Na2CO3(s) → 2Na+(aq) + CO32-(aq)
d. Ba(NO3)2(aq) + Na2CO3(aq) → BaCO3(aq) + 2NaNO3(s)
34. If the solubility of Pb (OH) 2 is 0.155g/L, then the concentration of each ion in a saturated solution of a Pb(OH) 2 is ….
a. [Pb2+] = 0.155 g/L and [OH-] = 0.155 g/L
b. [Pb2+] = 0.052 g/L and [OH-] = 0.103 g/L
c. [Pb2+] = 6.43 x 10-4 mol/L and [OH-] = 1.29 x 10-3 mol/L
d. [Pb2+] = 6.43x10-4mol/L and [OH-] = 6.43 x 10-4 mol/L
35. Which of the following precipitates may form when equal volumes of AgNO3, SrCl2, and Na2CO3 are mixed together?
a. SrCO3 and AgCl
b. Ag2CO3 and AgCl
c. SrCO3 and Ag2CO3
d. SrCO3, Ag2CO3, and AgCl