Calculate the pH of a solution at 25°C in which the [OH−] = 5.4 x10 −7 M.
A) 4.51
B) 7.05
C) 7.73
D) 6.38
E) 8.40
Subjects
Sections | |||
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Identifying Acids and Bases | 52 mins | 0 completed | Learn Summary |
Arrhenius Acid and Base | 7 mins | 0 completed | Learn Summary |
Bronsted Lowry Acid and Base | 18 mins | 0 completed | Learn Summary |
Amphoteric | 6 mins | 0 completed | Learn |
Lewis Acid and Base | 14 mins | 0 completed | Learn Summary |
pH and pOH | 64 mins | 0 completed | Learn Summary |
Ka and Kb | 21 mins | 0 completed | Learn |
Ionic Salts | 46 mins | 0 completed | Learn |
Diprotic Acid | 31 mins | 0 completed | Learn Summary |
Polyprotic Acid | 24 mins | 0 completed | Learn |
Additional Practice |
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Strong Acid-Base Calculations |
Weak Acids |
Additional Guides |
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Strong Acids and Strong Bases |
Conjugate Acids and Bases |
Weak Bases |
Calculate the pH of a solution at 25°C in which the [OH−] = 5.4 x10 −7 M.
A) 4.51
B) 7.05
C) 7.73
D) 6.38
E) 8.40
We’re being asked to calculate for the pH of a solution in which the [OH-] = 5.4x10-7 M.
The pH and pOH of a compound determine its acidity and basicity.
• pH
▪ pH stands for the negative logarithmic function of hydronium ion concentration
▪ can be calculated using the following equation:
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