Open Question
What is the pH of an HCl solution if [H+] = 0.03?
17. Acid and Base Equilibrium
pH of Strong Acids and Bases
Struggling with General Chemistry?
Join thousands of students who trust us to help them ace their exams!Watch the first videoMultiple Choice
What is the concentration of hydronium ions [H3O+] and hydroxide ions [OH−] in a 0.016 mol L−1 solution of HNO3?
A
[H3O+] = 0.032 M, [OH−] = 3.12 × 10^-13 M
B
[H3O+] = 0.008 M, [OH−] = 1.25 × 10^-7 M
C
[H3O+] = 0.016 M, [OH−] = 1.0 × 10^-14 M
D
[H3O+] = 0.016 M, [OH−] = 6.25 × 10^-13 M
Verified step by step guidance1
Identify that HNO3 is a strong acid, which means it completely dissociates in water. Therefore, the concentration of hydronium ions [H3O+] will be equal to the initial concentration of HNO3.
Write the dissociation equation for HNO3: HNO3 → H3O+ + NO3−. This shows that each mole of HNO3 produces one mole of H3O+.
Since the concentration of HNO3 is 0.016 mol L−1, the concentration of [H3O+] will also be 0.016 mol L−1.
Use the water dissociation constant (Kw) to find the concentration of hydroxide ions [OH−]. Kw at 25°C is 1.0 × 10^-14. The relationship is given by Kw = [H3O+][OH−].
Substitute the known values into the equation: 1.0 × 10^-14 = (0.016)[OH−]. Solve for [OH−] to find its concentration.
2:39mWatch next
Master pH of Strong Acids and Bases with a bite sized video explanation from Jules
Start learningRelated Videos
Related Practice
pH of Strong Acids and Bases practice set
Problem sets built by lead tutorsExpert video explanations