# Problem: 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.]

###### FREE Expert Solution

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 HNO3strong acids → completely ionize in the solution

Calculate moles Hfrom 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 Hfrom 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

0.

moles H+ = 0.3154 mol

Total moles H+0.6202 mol + 0.3154 mol

Total moles H+ = 0.9356 mol

Calculate [H+]: ###### Problem Details

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.]