Chemistry I Dr. Saulmon School Year Unit 4: Chemical Reactions Problem Set 8 Thursday, October 9, 2014

Transcription

1 Chemistry I Dr. Saulmon School Year Unit 4: Chemical Reactions Problem Set 8 Thursday, October 9, On the basis of the general solubility rules given in Table 7.1 in your book, predict which of the following substances are likely to be soluble in water. a. Aluminum nitrate b. Magnesium chloride c. Rubidium sulfate d. Nickel(II) hydroxide e. Lead(II) sulfide f. Magnesium hydroxide g. Iron(III)phosphate h. Manganese(II) chloride i. Lead(II) sulfide j. Iron(III) hydroxide k. Potassium fluoride l. Magnesium sulfate m. Iron(II) sulfide n. Potassium carbonate

2 o. Calcium carbonate 2. On the basis of the general solubility rules given in Table 7.1 in your book, predict the identity of the precipitate that forms when aqueous solutions of the following substances are mixed. If no precipitate is likely, indicate which rules apply. a. Iron(III) chloride, FeCl3, and phosphoric acid, H3PO4 b. Barium nitrate, Ba(NO3)2, and sodium sulfate, Na2SO4 c. Potassium chloride, KCl, and iron(ii) sulfate, FeSO4 d. Lead(II) nitrate, Pb(NO3)2, and hydrochloric acid, HCl e. Calcium nitrate, Ca(NO3)2, and sodium chloride, NaCl f. Ammonium sulfide, (NH4)2S, and copper(ii) chloride, CuCl2 g. Sodium carbonate, Na2CO3, and manganese(ii) chloride, MnCl2 h. Potassium sulfate, K2SO4, and calcium acetate, Ca(C2H3O2)2 i. Sodium nitrate, NaNO3, and lithium sulfate, Li2SO4 j. Potassium hydroxide, KOH, and nickel(ii) chloride, NiCl2 k. Sulfuric acid, H2SO4, and barium chloride, BaCl2

3 3. On the basis of the general solubility rules given in Table 7.1 of your book, write a balanced molecular equation for the precipitation reactions that take place when the following aqueous solutions are mixed. Include the state [(aq) or (s)] of the products. If no precipitation reaction is likely for the reactants given, explain why. a. Ammonium chloride, NH4Cl, and sulfuric acid, H2SO4 b. Potassium carbonate, K2CO3, and tin(iv) chloride, SnCl4 c. Ammonium chloride, NH4Cl, and lead(ii) nitrate, Pb(NO3)2 d. Copper(II) sulfate, CuSO4, and potassium hydroxide, KOH e. Sodium phosphate, Na3PO4, and chromium(iii) chloride, CrCl3 f. Ammonium sulfide, (NH4)2S, and iron(iii) chloride, FeCl3 g. Sodium sulfide, Na2S, and copper(ii) chloride, CuCl2 h. Potassium phosphate, K3PO4, and aluminum chloride, AlCl3 i. Sulfuric acid, H2SO4, and barium chloride, BaCl2 j. Sodium hydroxide, NaOH, and iron(iii) chloride, FeCl3 k. Sodium chloride, NaCl, and mercury(i) nitrate, Hg2(NO3)2 l. Potassium carbonate, K2CO3, and chromium(iii) acetate, Cr(C2H3O2)3

4 4. For each of the following precipitation reactions, complete and balance the equation, indicating clearly which product is the precipitate a. Ba(NO3)2(aq) + (NH4)2SO4(aq) b. CoCl3(aq) + NaOH(aq) c. FeCl3(aq) + (NH4)2S(aq) d. CaCl2(aq) + AgC2H3O2(aq) e. Ba(NO3)2(aq) + NH4OH(aq) f. NiCl2(aq) + Na2CO3(aq) 5. For the following pairs of aqueous solutions, (a) write a balanced chemical equation that includes the states [(aq) or (s)] of the reactants and the products, (b) write a complete ionic equation, and (c) write the net ionic equation. a. Silver nitrate and hydrochloric acid b. Copper(II) sulfate and ammonium carbonate c. Iron(II) sulfate and potassium carbonate d. Silver nitrate and potassium nitrate e. Lead(II) nitrate and lithium carbonate f. Tin(IV) chloride and sodium hydroxide

5 g. Calcium chloride and sodium phosphate h. Lead(II) nitrate and barium chloride i. Iron(III) chloride and sodium hydroxide j. Nickel(II) nitrate and ammonium sulfide k. Silver nitrate and potassium chloride l. Sodium carbonate and barium nitrate m. Potassium chloride and mercury(i) nitrate n. Calcium chloride and ammonium sulfate