1. Using the criteria for double displacement reactions, together with the solubility table, predict whether a double displacement reaction will occur in each example below. If the reaction will occur, complete and balance the equation properly indicating gases and precipitates. If you believe no reaction will occur, write no reaction as the right-hand side of the equation. All reactants are aqueous solutions.
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Equation
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___K2S (aq)+ ___CuSO4 (aq)→
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___NH4OH (aq)+ ___Na2CrO4 (aq)→
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___KOH (aq)+ ___NH4Cl (aq)→
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___NaC2H3O2 (aq) + ___HCl(aq)→
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___Na2CrO4 (aq) + ___Pb(C2H3O2)2 (aq)→
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___(NH4)2SO4 (aq) + ___NaCl(aq)→
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___BiCl3 (aq)+ ___NaOH(aq)→
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___KC2H3O2 (aq)+ ___CoSO4 (aq)→
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___Na2CO3 (aq) + ___HNO3 (aq)→
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___ZnBr2 (aq) + ___K3PO4 (aq)→
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2. Write the chemical formulas for the reactants of each reaction given below. Then write the potential products on the product side. Circle each product that removes ions from solution, and note how: a precipitate (ppt), a gas or a slightly ionized compound (water is a common example). If the reaction occurs, balance the equation. If no ions are removed from solution, draw a light line through the potential products and write NR for no reaction.
a. lead (II) nitrate and potassium chloride
b. ammonium sulfate and hydrochloric acid
c. phosphoric acid and potassium hydroxide
d. sodium sulfite and sulfuric acid
e. iron (III) nitrate and potassium hydroxide.