17. Acid and Base Equilibrium
pH of Strong Acids and Bases
30PRACTICE PROBLEM
Laboratory preparation of carbon dioxide (CO2) gas is often carried out by reacting limestone (CaCO3) with hydrochloric acid (HCl). The limestone dissolves completely into the acid solution and produces CaCl2, H2O, and CO2. Determine the volume (in mL) of a pH 1.100 HCl solution that could dissolve a 1.15 g piece of limestone. Could the same piece of limestone neutralize a 350 mL sample of HCl solution with a pH of 1.100? If not, what fraction can it neutralize?
Laboratory preparation of carbon dioxide (CO2) gas is often carried out by reacting limestone (CaCO3) with hydrochloric acid (HCl). The limestone dissolves completely into the acid solution and produces CaCl2, H2O, and CO2. Determine the volume (in mL) of a pH 1.100 HCl solution that could dissolve a 1.15 g piece of limestone. Could the same piece of limestone neutralize a 350 mL sample of HCl solution with a pH of 1.100? If not, what fraction can it neutralize?