Worksheet #5: Double-Replacement Reactions

University:
University of Michigan
Course:
CHEM 125 | General Chemistry Laboratory I
Academic year:

2019
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0

Pages:

2
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customer-8070004

Worksheet #5: Double-Replacement Reactions In these reactions, all you do is look at the names of the reactants, and "switch partners". Just be sure that the new pairs come out with the positive ion named first, and paired with a negative ion. 1. aluminum iodide + mercury(II) chloride Æ 2. silver nitrate + potassium phosphate 3. copper(II) bromide 4. calcium acetate 5. ammonium chloride + 6. calcium nitrate hydrochloric acid 7. iron(II) sulfide 8. copper(II) hydroxide 9. calcium hydroxide 10. calcium bromide + + aluminum chloride + + Æ mercury(I) acetate acetic acid Æ Æ hydrochloric acid + Æ sodium carbonate + + Æ Æ Æ phosphoric acid Æ potassium hydroxide Æ Examine the products of the reactions on this page, and determine in each whether a gas, water, or a precipitate is formed. Use solubility Table B.9 on page R54 at the back of your textbook to determine the solubilities of the reaction products. If there is no gas, water, or precipitate produced, put an "X" through the yield sign, because no reaction occurs. Worksheet #5: Double-Replacement Reactions In these reactions, all you do is look at the names of the reactants, and "switch partners". Just be sure that the new pairs come out with the positive ion named first, and paired with a negative ion. 1. aluminum iodide + mercury(II) chloride Æ aluminum chloride + mercury(II) iodide 2AlI3 2. silver nitrate + + 3HgCl2 potassium phosphate 3AgNO3 3. + calcium acetate + + calcium nitrate + iron(II) sulfide + FeS 8. 2AlCl3 potassium nitrate + 3KNO3 3CuCl2 Æ + 2AlBr3 Æ calcium carbonate Na2CO3 CaCO3(ppt) Æ + sodium acetate + 2NaC2H3O2 + 2HCl hydrochloric acid + 2HCl copper(II) hydroxide + calcium hydroxide Hg2(C2H3O2)2 2NH4 C2H3O2 Æ + Hg2Cl2(ppt) hydrochloric acid Æ calcium chloride + nitric acid Æ Æ Æ CaCl2 + 2HNO3 iron(II) chloride + hydrogen sulfide (g) FeCl2 + H2S acetic acid Æ copper(II) acetate + water + + 2HC2H3O2 Æ Cu(C2H3O2)2 + 2H2O phosphoric acid Æ calcium phosphate + water 3Ca(OH)2 10. + + Cu(OH)2 9. + ammonium chloride + mercury(I) acetate Æ ammonium acetate + mercury(I) chloride Ca(NO3)2 7. Ag3PO4(ppt) Æ sodium carbonate 2NH4Cl 6. 3HgI2(ppt) Æ silver phosphate K3PO4 Ca(C2H3O2)2 5. + copper(II) bromide + aluminum chloride Æ copper(II) chloride + aluminum bromide 3CuBr2 4. 2AlCl3 Æ + 2H3PO4 Æ Ca3(PO4)2 + 6H2O calcium bromide + potassium hydroxide Æ calcium hydroxide + potassium bromide CaBr2 + 2KOH Æ Ca(OH)2 + 2KBr Examine the products of the reactions on this page, and determine in each whether a gas, water, or a precipitate is formed. Use solubility Table B.9 on page R54 at the back of your textbook to determine the solubilities of the reaction products. If there is no gas, water, or precipitate produced, put an "X" through the yield sign, because no reaction occurs.

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