Practice: Solution contains [Cu2+] = 0.035 M, [Sr2+] = 0.054 M, [Al3+] = 0.23 M. Cu2+ can be separated by selective precipitation using NaOH. What is the minimum concentration of NaOH needed to start precipitation of Cu2+? (Ksp = 2.2 × 10−20 of Cu(OH)2).
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| Intro to Buffers | 20 mins | 0 completed | Learn |
| Henderson-Hasselbalch Equation | 17 mins | 0 completed | Learn |
| Intro to Acid-Base Titration Curves | 13 mins | 0 completed | Learn |
| Strong Titrate-Strong Titrant Curves | 9 mins | 0 completed | Learn |
| Weak Titrate-Strong Titrant Curves | 15 mins | 0 completed | Learn |
| Acid-Base Indicators | 8 mins | 0 completed | Learn |
| Titrations: Weak Acid-Strong Base | 39 mins | 0 completed | Learn |
| Titrations: Weak Base-Strong Acid | 40 mins | 0 completed | Learn |
| Titrations: Strong Acid-Strong Base | 12 mins | 0 completed | Learn |
| Titrations: Diprotic & Polyprotic Buffers | 32 mins | 0 completed | Learn |
| Solubility Product Constant: Ksp | 18 mins | 0 completed | Learn |
| Ksp: Common Ion Effect | 18 mins | 0 completed | Learn |
| Precipitation: Ksp vs Q | 12 mins | 0 completed | Learn |
| Selective Precipitation | 9 mins | 0 completed | Learn |
| Complex Ions: Formation Constant | 18 mins | 0 completed | Learn |
Process of separating specific ions out of a solution by using reagents to form a precipitate.
Concept #1: Selective Precipitation
Successful precipitation of a selected ion depends on the solubility (Ksp) of its salt.
Example #1: Sample of a solution contains 0.405 M CrO42- and 0.628 M S2- ions. These two ions can be precipitated with the use of PbF2. Which ion will precipitate out first and at which concentration?
(PbCrO4 Ksp = 2.0 x 10-16, PbS Ksp = 7.0 x 10-29.)
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