Practice: An aqueous solution of HBrO4 has a pH of 4.34. Find the molar concentration of HBrO4 solution.
| Sections | |||
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| Acids Introduction | 9 mins | 0 completed | Learn |
| Bases Introduction | 8 mins | 0 completed | Learn |
| Binary Acids | 16 mins | 0 completed | Learn |
| Oxyacids | 10 mins | 0 completed | Learn |
| Bases | 15 mins | 0 completed | Learn |
| Amphoteric Species | 5 mins | 0 completed | Learn |
| Arrhenius Acids and Bases | 5 mins | 0 completed | Learn |
| Bronsted-Lowry Acids and Bases | 20 mins | 0 completed | Learn |
| Lewis Acids and Bases | 13 mins | 0 completed | Learn |
| The pH Scale | 16 mins | 0 completed | Learn |
| Auto-Ionization | 9 mins | 0 completed | Learn |
| Ka and Kb | 16 mins | 0 completed | Learn |
| pH of Strong Acids and Bases | 10 mins | 0 completed | Learn |
| Ionic Salts | 16 mins | 0 completed | Learn |
| pH of Weak Acids | 30 mins | 0 completed | Learn |
| pH of Weak Bases | 32 mins | 0 completed | Learn |
| Diprotic Acids and Bases | 9 mins | 0 completed | Learn |
| Diprotic Acids and Bases Calculations | 35 mins | 0 completed | Learn |
| Triprotic Acids and Bases | 9 mins | 0 completed | Learn |
| Triprotic Acids and Bases Calculations | 17 mins | 0 completed | Learn |
| Additional Guides |
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| Conjugate Acids and Bases |
The pH of Strong Acids and Bases is determined by their H+ and OH– concentrations
pH of Strong Acids and Bases
Concept #1: Strong Acids and Bases represent strong electrolytes.
Example #1: If the concentration of Ba(H)2 solution is 0.398 M, calculate its pOH.
Practice: Calculate the pH of a 25 mL of 5.45 × 10−2 M LiOH solution.
Practice: HI is a strong acid (Ka = 3.2 × 109). Calculate [H+], [OH−], pH and pOH of a 7.1 × 10−2 M HI solution.
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