CHAPTER 16 REGULAR HOMEWORK:
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At a certain temperature* (probably not 25 ºC), the solubility of silver sulfate, Ag2SO4, is 0.010 mol/L. Calculate its solubility product constant for this temperature. 4 SIG. FIG. (required because number is small)
*Solubility product constants are very temperature sensitive. They are generally reported at 25 ºC. Not necessarily using this temperature allows me some flexibility.
At a certain temperature, the solubility of potassium iodate, KIO3, is 38.6 g/L. Calculate its solubility product constant for this temperature.
At a certain temperature, the solubility of cadmium fluoride, CdF2, is 0.083 mol/L. Calculate its solubility product constant for this temperature.
At a certain temperature, the solubility product constant* of copper (II) iodate, Cu(IO3)2, is 7.60×10-8 M3. Calculate the solubility of this compound for this temperature.
*Unless stated otherwise all solubility product constants are for water.
Calculate the solubility of copper (II) iodate in 0.61 M copper (II) nitrate. Ksp* is 7.4×10-8 M3.
*You should know that the Ksp must refer to the copper iodate because all nitrate compounds are soluble and strong electrolytes!
Warm UP Question. What is the initial (before any reaction takes place) lead nitrate concentration when 5.0 mL of 0.247 M lead nitrate is added to 15 mL of 0.0028 M sodium chloride?
For the reaction: PbCl2(s) ↔ Pb2+(aq)+2Cl1-(aq), what is Q* when 2.4 mL of 0.098 M lead nitrate is added to 20 mL of 0.019 M sodium chloride?
Ksp of lead chloride is 1.6 x 10-5 M3.
Hint given in general feedback
*Recall: Q is compared to Ksp to determine whether a precipitate forms.
Remember each solution is diluted by the other solution.
Does a precipitate form for the above conditions?
Pick the correct formula for sodium phosphate, calcium phosphate, and aluminum phosphate. (All must be correct to get credit.)
Select one or more:
The Ksp of aluminum phosphate is 9.8×10-21 M2.
The Ksp of calcium phosphate is 1.3×10-32 M5.
Sodium phosphate is added to a solution that contains aluminum nitrate and calcium chloride. Their concentrations, which are necessary to do this problem, are given in the next question. Which begins to precipitate first?
Sodium phosphate is added to a solution that contains 0.0099 M aluminum nitrate and 0.021 M calcium chloride. The concentration of the first ion to precipitate (either Al3+ or Ca2+) decreases as its precipitate forms. What is the concentration of this ion when the second ion begins to precipitate?
Note that well over 99% of the first ion has precipitated before the second ion starts to precipitate.