Question 7 Solubility Rules for Some Ionic Compounds in Water Seluble compounds Almost all salts of Na", K, NH4 Salts of nitrate (NO, ), chlorate (CIO, ), perchlorate (CIO,), acetate (CH3 CO,) Almost all salts of Cl, Br, I Exceptions (not soluble): halides of Ag, Hg, , Ph2+ Salts containing F Exceptions (not soluble): fluorides of Mg+, Ca, Sr+ Ba+. Pb?+ Salts of sulfate (So,) Exceptions (not soluble): sulfates of Ca+, Sr+, Ba", Pb2, Ag Insoluble compounds Most salts of carbonate (CO,), phosphate (PO,), oxalate (C,0,), chromate (Cro,), sulfide (S-) Exceptions (soluble): salts of NH* and the alkali metal cations, and Bas Most metal hydroxides and oxides Exceptions (soluble): alkali metal hydroxides and Ba(OH)2 and Sr(OH), A. Write the net ionic equation for the following molecular equation. Pb(NO3)2 (aq) +K2CO3 (aq) PbCO3(s) + 2KN03(aq) (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + B. The following molecular equation represents the reaction that occurs when aqueous solutions of lead(II) nitrate and zinc chloride are combined. Pb(NO3)2 (aq) + ZnCl2 (aq) → PbCl2 (s) + Zn(NO3)2 (aq) Write the balanced net ionic equation for the reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + C. When aqueous solutions of iron(III) sulfate and sodium carbonate are combined, solid iron(III) carbonate and a solution of sodium sulfate are formed. The net ionic equation for this reaction is: (Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds.) Be sure to specify states such as (ag) or (s). If a box not needed leave it blank.
Question 7 Solubility Rules for Some Ionic Compounds in Water Seluble compounds Almost all salts of Na", K, NH4 Salts of nitrate (NO, ), chlorate (CIO, ), perchlorate (CIO,), acetate (CH3 CO,) Almost all salts of Cl, Br, I Exceptions (not soluble): halides of Ag, Hg, , Ph2+ Salts containing F Exceptions (not soluble): fluorides of Mg+, Ca, Sr+ Ba+. Pb?+ Salts of sulfate (So,) Exceptions (not soluble): sulfates of Ca+, Sr+, Ba", Pb2, Ag Insoluble compounds Most salts of carbonate (CO,), phosphate (PO,), oxalate (C,0,), chromate (Cro,), sulfide (S-) Exceptions (soluble): salts of NH* and the alkali metal cations, and Bas Most metal hydroxides and oxides Exceptions (soluble): alkali metal hydroxides and Ba(OH)2 and Sr(OH), A. Write the net ionic equation for the following molecular equation. Pb(NO3)2 (aq) +K2CO3 (aq) PbCO3(s) + 2KN03(aq) (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + B. The following molecular equation represents the reaction that occurs when aqueous solutions of lead(II) nitrate and zinc chloride are combined. Pb(NO3)2 (aq) + ZnCl2 (aq) → PbCl2 (s) + Zn(NO3)2 (aq) Write the balanced net ionic equation for the reaction. (Use the lowest possible coefficients. Be sure to specify states such as (aq) or (s). If a box is not needed, leave it blank.) + C. When aqueous solutions of iron(III) sulfate and sodium carbonate are combined, solid iron(III) carbonate and a solution of sodium sulfate are formed. The net ionic equation for this reaction is: (Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds.) Be sure to specify states such as (ag) or (s). If a box not needed leave it blank.
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Transcribed Image Text:Question 7
Solubility Rules for Some Ionic Compounds in Water
Soluble compounds
Almost all salts of Na*, K, NH4
Salts of nitrate (NO, ), chlorate (CIO; ), perchlorate (CI0,), acetate (CH3 CO,)
Almost all salts of Cl", Br, I
Exceptions (not soluble): halides of Ag, Hg, +, Ph2+
Salts containing F
Exceptions (not soluble): fluorides of Mg+, Ca, Sr+ Ba+ Pb?+
Salts of sulfate (So,)
Exceptions (not soluble): sulfates of Ca+, Sr+, Ba, Ph2, Ag
Insoluble compounds
Most salts of carbonate (CO,), phosphate (PO,), oxalate (C20,), chromate (Cro,), sulfide (S)
Exceptions (soluble): salts of NH4" and the alkali metal cations, and Bas
Most metal hydroxides and oxides
Exceptions (soluble): alkali metal hydroxides and Ba(OH)2 and Sr(OH)2
A. Write the net ionic equation for the following molecular equation.
Pb(NO3)2 (aq) + K2CO3 (aq) PbCO3 (s) + 2KNO3 (aq)
(Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.)
B. The following molecular equation represents the reaction that occurs when aqueous solutions of lead(II) nitrate and zinc chloride are combined.
Pb(NO3)2 (aq) + ZnCl2 (aq) → PbCl (s) + Zn(NO3)2(aq)
Write the balanced net ionic equation for the reaction.
(Use the lowest possible coefficients. Be sure to specify states such as (ag) or (s). If a box is not needed, leave it blank.)
C. When aqueous solutions of iron(III) sulfate and sodium carbonate are combined, solid iron(III) carbonate and a solution of sodium sulfate are formed. The net ionic equation for this reaction is:
(Use the solubility rules provided in the OWL Preparation Page to determine the solubility of compounds.)
Be sure to specify states such as (aq) or (s). If a box
not needed leave it blank.
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