## Solution Stoichiometry

The following problems are taken from T. L. Brown, H. E. Lemay, B. E. Bursten, & J. R. Burdge, Chemistry: The Central Science, Ninth Edition, Chapter 4. To see the solution to a problem or to return from the solution, click on the number of the problem.

16) Write balanced net ionic equations for the reactions that occur in each of the following cases. Identify the spectator ion or ions in each reaction.

(a) Cr2(SO4)3(aq) + (NH4)2CO3(aq)

(b) AgNO3(aq) + K2SO4(aq)

(c) Pb(NO3)2(aq) + KOH(aq)

58) Assuming that the volumes are additive, indicate the concentration of each ion present in the solution formed by mixing:

(a) 20 mL of 0.100 M HCl and 10.0 mL of 0.500 M HCl

(b) 15.0 mL of 0.300 M Na2SO4 and 10.0 mL of 0.200 M KCl

(c) 3.50 g of NaCl in 50.0 mL of 0.500 M CaCl2 solution

66) What mass of NaOH is needed to precipitate all the Fe2+ ions from 25.0 mL of 0.500 M Fe(NO3)2 solution?

72) In the laboratory 7.52 g of Sr(NO3)2 is dissolved in enough water to form 0.750 L. A 0.100-L sample is withdrawn from this stock solution and titrated with 0.0425 M solution of Na2CrO4. What volume of Na2CrO4 solution is needed to precipitate all the Sr2+(aq) as SrCrO4?

96) A tanker truck carrying 5.0 x 103 kg of concentrated sulfuric acid solution tips over and spills its load. If the sulfuric acid is 95.0% H2SO4 by mass and has a density of 1.84 g/mL, how many kilograms of sodium carbonate must be added to neutralize the acid?

98) A sample of 1.50 g of lead(II) nitrate is mixed with 125 mL of 0.100 M sodium sulfate solution.

(a) Write the chemical equation for the reaction that occurs.

(b) Which is the limiting reactant in the reaction?

(c) What are the concentrations of all ions that remain in solution after the reaction is complete?

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