1. One process for the commercial production of baking soda, sodium hydrogen carbonate, involves the following reaction: aqueous sodium chloride + gaseous ammonia + solid carbon dioxide + liquid water yields aqueous ammonium chloride + solid sodium hydrogen carbonate. Because they are relatively cheap, sodium chloride and water are typically present in excess. What is the theoretical yield of sodium hydrogen carbonate when one performs such a synthesis using 10.0 grams of ammonia and 15.0 grams of solid carbon dioxide, with excess of water and sodium chloride?
2. The traditional method of analysis for the amount of chloride ion present in a sample was to dissolve the sample in water and then slowly add a solution of silver nitrate. Silver chloride is very insoluble in water, and by adding a slight excess of silver nitrate, it is possible effectively to remove all the chloride ion from the sample. First, write a balanced net ionic equation for this reaction. Then, assume that a sample mass of 1.054 grams contains 10.3% chloride by mass. Then, calculate the mass of silver nitrate must be used to completely precipitate the chloride from the sample. Finally, how many silver chloride molecules will be formed?
1. Write the balanced reaction
NaCl (aq) + NH3 (g) + CO2 (s) + H20 (l) = NH4Cl (aq) + NaHCO3 (s)
Molecular weight of NH3 = 17 (g/mol)
Molecular weight of CO2 = 44 (g/mol)
Number of mole of NH3 = ...
The solution provides detailed calculations and explanations for the problem.