Asked by Andre
A solution is prepared by adding 50.3 mL of concentrated hydrochloric acid and 16.6 mL of concentrated nitric acid to 300 mL of 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 and has a density of 1.42 g/mL.]
Answers
Answered by
DrBob222
First thing calculate the molarity of HCl and HNO3.
HCl: 1.19 g/mL x 1000 mL x 0.38/molar mass HCl = approx 12M but you need to do it more accurately.
HNO3: 1.42 g/mL x 1000 mL x 0.70/molar mass HNO3 = approximately 16M.
mol H^+ from HCl = 50.3 x 12M = ?
mol H^+ from HNO3 = 16.6 mL x 16 M = ?
Total mols H^+ = sum of the two.
(H^+) = moles/L soln.
Convert to OH^- and pH.
HCl: 1.19 g/mL x 1000 mL x 0.38/molar mass HCl = approx 12M but you need to do it more accurately.
HNO3: 1.42 g/mL x 1000 mL x 0.70/molar mass HNO3 = approximately 16M.
mol H^+ from HCl = 50.3 x 12M = ?
mol H^+ from HNO3 = 16.6 mL x 16 M = ?
Total mols H^+ = sum of the two.
(H^+) = moles/L soln.
Convert to OH^- and pH.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.