4.1 & 4.2: General properties of aqueous solutions and Precipitation Reactions:
4.1 & 4.2: General properties of aqueous solutions and Precipitation Reactions:
1. (Brown 4.11) When asked what causes electrolyte solutions to conduct electricity, a student responds that it is due to the movement of electrons through the solution. Is the student correct? If not, what is the correct response?
2. (Brown 4.15) Specify what ions are present in solution upon dissolving each of the following in water:
a. ZnCl2 c. (NH4)2SO4
b. HNO3 d. Ca(OH)2
3. (Brown 4.16 ) Specify what ions are present upon dissolving each of the following substances in water.
a. MgI2 b. Al(NO3)3 c. HClO4 d. NaCH3COO
4. (Brown 4.19) Using solubility guidelines , predict whether each of the following compounds is soluble or insoluble in water.
a. MgBr2 d. Sr(OH)2
b. PbI2 e. ZnSO4
c. (NH4)2CO3
5. (Brown 4.20 w/ additional) Predict whether each of the following compounds is soluble in water:
a. AgI f. Sr(NO3)2
b. Na2CO3 g. CuSO4
c. BaCl2 h. CuCl2
d. Al(OH)3 g. PbS
e. Zn(CH3COO)2
6. Complete the following double replacement (exchange ) reactions.
Be sure to balance them.
a. MgCl2 + Ba(NO3)2 →
b. Al2(CrO4)3 + (NH4)2SO4 →
c. K2SO4 + SrCl2 →
d. FeCl3 + KOH →
e. HCl + AgNO3 →
f. K2SO4 + Ba(NO3)2 →
7. (Brown 4.21) Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction.
a. Na2CO3 and AgNO3
b. NaNO3 and NiSO4
c. FeSO4 and Pb(NO3)2
8. (4.22 Brown) Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction
a. NaCH3COO and HCl
b. KOH and Cu(NO3)2
c. Na2S and CdSO4
9. Write balanced molecular equations, complete ionic equations and net ionic equations for each of the following reactions. All reactants are aqueous. Determine whether the products are aqueous or precipitates.
a. Hydrochloric acid , HCl, reacts with silver nitrate, AgNO3, to produce
1. (Brown 4.11) When asked what causes electrolyte solutions to conduct electricity, a student responds that it is due to the movement of electrons through the solution. Is the student correct? If not, what is the correct response?
2. (Brown 4.15) Specify what ions are present in solution upon dissolving each of the following in water:
a. ZnCl2 c. (NH4)2SO4
b. HNO3 d. Ca(OH)2
3. (Brown 4.16 ) Specify what ions are present upon dissolving each of the following substances in water.
a. MgI2 b. Al(NO3)3 c. HClO4 d. NaCH3COO
4. (Brown 4.19) Using solubility guidelines , predict whether each of the following compounds is soluble or insoluble in water.
a. MgBr2 d. Sr(OH)2
b. PbI2 e. ZnSO4
c. (NH4)2CO3
5. (Brown 4.20 w/ additional) Predict whether each of the following compounds is soluble in water:
a. AgI f. Sr(NO3)2
b. Na2CO3 g. CuSO4
c. BaCl2 h. CuCl2
d. Al(OH)3 g. PbS
e. Zn(CH3COO)2
6. Complete the following double replacement (exchange ) reactions.
Be sure to balance them.
a. MgCl2 + Ba(NO3)2 →
b. Al2(CrO4)3 + (NH4)2SO4 →
c. K2SO4 + SrCl2 →
d. FeCl3 + KOH →
e. HCl + AgNO3 →
f. K2SO4 + Ba(NO3)2 →
7. (Brown 4.21) Will precipitation occur when the following solutions are mixed? If so, write a balanced chemical equation for the reaction.
a. Na2CO3 and AgNO3
b. NaNO3 and NiSO4
c. FeSO4 and Pb(NO3)2
8. (4.22 Brown) Identify the precipitate (if any) that forms when the following solutions are mixed, and write a balanced equation for each reaction
a. NaCH3COO and HCl
b. KOH and Cu(NO3)2
c. Na2S and CdSO4
9. Write balanced molecular equations, complete ionic equations and net ionic equations for each of the following reactions. All reactants are aqueous. Determine whether the products are aqueous or precipitates.
a. Hydrochloric acid , HCl, reacts with silver nitrate, AgNO3, to produce