WorksheetsAcids and Bases Molarity Calculations
Total questions: 13
Worksheet time: 1hrs 1mins
The pH of a substance is defined as:
log[H+]
–log[H–]
-log[H+]
–log[OH–]
Which concentration indicates a basic solution at 298 K?
[OH–] > 1.0 × 10–7
[H3O+] > 1.0 × 10–7
[OH–] = 1.0 × 10–7
[H3O+] = 1.0 × 10-7
A solution of acid A has a pH of 1 and a solution of acid B has a pH of 2. Which statement must be correct?
Acid A is stronger than acid B.
[A]>[B]
The concentration of H+ ions in A is higher than in B
The concentration of H+ ions in B is twice the concentration of
H+ ions in A.
As the [H3O+] in a solution decreases, the [OH-]
increases and the pH increases.
increases and the pH decreases.
decreases and the pH increases.
decreases and the pH decreases.
HCl + KOH --> H2O + KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if 15.0mL of acid neutralized?
Ca(OH)2 + H2CO3 -->
The larger the Ka value for a weak acid, the ______________ the ionization of the weak acid in water.
lower
greater
