CHEM 24112 Chapter Notes - Chapter 7: Barium Chloride, Ammonium Sulfate, Potassium Sulfate

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Homework 7.2: Net Ionic Equations and Acid-Base Reactions

1. What is a net ionic equation? What species are shown in such an equation, and which species are

not shown?

2. What are spectator ions? Write an example of an equation in which spectator ions are present and

identify them.

3. Write balanced net ionic equations for the reactions that occur when the following aqueous

solutions are mixed. If no reaction is likely (i.e. there is no driving force), so indicate.

a. silver nitrate, AgNO3, and potassium chloride, KCl

b. nickel (II) sulfate, NiSO4, and barium chloride, BaCl2

c. ammonium phosphate, (NH4)3PO4, and calcium chloride, CaCl2

d. hydrofluoric acid, HF, and potassium sulfate, K2SO4

e. calcium chloride, CaCl2, and ammonium sulfate, (NH4)2SO4

f. lead (II) nitrate, Pb(NO3)2, and barium chloride, BaCl2

4. What is meant by a strong acid? Are the strong acids also strong electrolytes? Explain.

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PLEASE HELP LAB WORK DUE MONDAY MORNING, KINDLY SHOW ALL WORKINGS AND CALCULATIONS

TOPIC: METATHESIS REACTIONS AND NET IONIC EQUATIONS.

Write the Molecular equation, Complete Ionic equation, and Net Ionic equation for the following reactions:

(1). Copper(II) sulfate + Sodium carbonate.

(2). Copper(II) sulfate + Barium chloride.

(3). Copper(II) sulfate + Sodium phosphate

(4). Sodium carbonate + Sulfuric acid

(5). Sodium carbonate + Hydrochloric acid

(6). Cadmium chloride + Sodium sulfide

(7). Cadmium chloride + Sodium hydroxide

(8). Nickel chloride + Silver nitrate

(9). Nickel chloride + Sodium carbonate

(10). Hydrochloric acid + Sodium hydroxide

(11). Ammonium chloride + Sodium hydroxide

(12). Sodium acetate + Hydrochloric acid

(13). Sodium sulfide + Hydrochloric acid

(14). Lead nitrate + Sodium sulfide

(15). Lead nitrate + Sulfuric acid

(16). Potassium chloride + Sodium nitrate

Fill the questions according to Data Table 7-2

5. balanced formula equation: for each combination of solutions that produced new product. write correct chemical formulas for the new compounds that could form from the ions present. Indicate which of the new compunds is a precipitate. If no reaction occurs, write NR.

6. complete ionic equation: write complete ionic equations for the precipitation reactions that you observed. show the reactants as ions, the precipitate as a solid, and the spectator ions as unchanged. balance each equation for mass and change. the total charge should be zero on each side of the equation.

7. net ionic equation: write the net ionic equations for each reaction in the preceding question.

CHEM 24112 Chapter Notes - Chapter 7: Barium Chloride, Ammonium Sulfate, Potassium Sulfate

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