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| Buffer | 50 mins | 0 completed | Learn |
| Acid and Base Titration Curves | 32 mins | 0 completed | Learn |
| Weak Acid Strong Base Titrations | 34 mins | 0 completed | Learn |
| Weak Base Strong Acid Titrations | 17 mins | 0 completed | Learn |
| Strong Acid Strong Base Titrations | 10 mins | 0 completed | Learn Summary |
| Titrations of Diprotic and Polyprotic Acids | 27 mins | 0 completed | Learn |
| Ksp | 58 mins | 0 completed | Learn |
| Additional Practice |
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| Equivalence Point |
| Acid Base Indicators |
| Selective Precipitation |
| Formation Constant |
| Additional Guides |
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| Henderson Hasselbalch Equation |
An aqueous solution contains dissolved C6H5NH3Cl and C6H5NH2. The concentration of C6H5NH2 is 0.50 M and pH is 4.20.
b. Calculate the pH after 4.0 g NaOH(s) is added to 1.0 L of this solution. (Neglect any volume change.)
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