A solution is prepared by adding 51.7 mL concentrated hydrochloric acid and 20.7 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.] [H+] = M [OH-] pH = = Submit Answer M Try Another Version
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![A solution is prepared by adding 51.7 mL concentrated
hydrochloric acid and 20.7 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.]
[H+] :
=
[OH-] =
=
pH =
Submit Answer
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Answer:-
This question is answered by using the simple concept of calculation of pH of the resulting solution using the formula. Firstly molar concentration of each acid is calculated using the molarity formula
Molarity = moles x 1000/volume(mL)
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