Concentrated HCl is 38% HCl (by mass) and has a density of 1.19 g/mL; concentrated HNO3 is 70.% HNO3 (by mass) and has a density of 1.42 g/mL
HCl and HNO3 → strong acids → completely ionize in the solution
Calculate moles H+ from HCl:
HCl → H+ + Cl-
38% HCl (by mass) = 38 g HCl/100 g solution
molar mass HCl = 36.458 g/mol
mass HCl = 22.61 g HCl
moles H+ = 0.6201 mol
Calculate moles H+ from HNO3:
HNO3 → H+ + NO3-
70% HNO3 (by mass) = 70 g HNO3/100 g solution
molar mass HNO3 = 63.018 g/mol
mass HNO3 = 19.88 g HNO3
moles H+ = 0.3154 mol
Total moles H+ = 0.6202 mol + 0.3154 mol
Total moles H+ = 0.9356 mol
A solution is prepared by adding 50.0 mL concentrated hydrochloric acid and 20.0 mL concentrated nitric acid to 300 mL water. More water is added until the final volume is 1.00 L. Calculate [H+], [OH-], and the pH for this solution. [Hint: Concentrated HCl is 38% HCl (by mass) and has a density of 1.19 g/mL; concentrated HNO3 is 70.% HNO3 (by mass) and has a density of 1.42 g/mL.]
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