Solution Found!
How many moles of H+ ions are present in the following
Chapter 4, Problem 16P(choose chapter or problem)
How many moles of \(H^{+}\) ions are present in the following aqueous solutions?
(a) \(1.40 \mathrm{~L}\) of \(0.25 \mathrm{M}\) perchloric acid
(b) \(6.8 \mathrm{~mL}\) of \(0.92 \mathrm{M}\) nitric acid
(c) \(2.6 \mathrm{~L}\) of \(0.085 \mathrm{M}\) hydrochloric acid
Questions & Answers
QUESTION:
How many moles of \(H^{+}\) ions are present in the following aqueous solutions?
(a) \(1.40 \mathrm{~L}\) of \(0.25 \mathrm{M}\) perchloric acid
(b) \(6.8 \mathrm{~mL}\) of \(0.92 \mathrm{M}\) nitric acid
(c) \(2.6 \mathrm{~L}\) of \(0.085 \mathrm{M}\) hydrochloric acid
ANSWER:
Step 1 of 3
Here we have to calculate how many moles of ions are present in the following aqueous solutions.
(a) 1.40 L of 0.25 M perchloric acid
1st we have to write the chemical reaction for the dissociation of perchloric acid (
In the above reaction it has been found that 1 mol of and 1 mole of
In this question it has been given that molarity of 
Mole of formed from
1.40 L of
= 0.35 mol of ion
Thus the aqueous solution of .40 L of 0.25 M perchloric acid contain 0.35 mol of ion.
___________________