<p>I’ve got this packet of AP Chemistry Ksp problems. If you’re up for it and kindly helpful, please see what you can get for these problems:</p>
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<li>ml of water will dissolve 8.7 mg of silver carbonate. What is the Ksp of silver carbonate?</li>
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<li><p>How many grams of lead II sulfate will dissolve in 400. ml of water if Ksp = 1.6 x 10^-8?</p></li>
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<li>ml 8.2 x 10^-4 M lead II nitrate and 25 ml 4.2 x 10^-6 M KI are mixed. Will lead II iodide precipitate? (Ksp = 7.1 x 10 ^-9)</li>
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<li><p>Find the solubility of barium carbonate in 0.010 M barium nitrate. (Ksp = 8.1 x 10 ^-9 for barium carbonate)</p></li>
<li><p>What is the maximum pH that a .075 M iron II nitrate solution can have and not precipitate FeS when the solution is saturated with hydrosulfuric acid? A saturated hydrosulfuric acid solution is 0.01 M in H2S (Ksp of FeS = 1 x 10^-19, and K1 and K2 for H2S are 1.0 x 10^-7 and 1.3 x 10^-13, respectively).</p></li>
<li><p>A 50. ml volume of solution containing 0.95 g of MgCl2 is mixed with an equal volume of 1.8 M aqueous ammonia. What weight of solid NH4Cl must be added to the resulting solution to prevent the precipitation of Mg(OH)2? (Ksp of Mg(OH)2 = 1.5 x 10^-11, Kb of NH3 = 1.8 x 10^-5)</p></li>
<li><p>A solution 1.0 x 10^-4 M both in Cl- and I- is subjected to the slow addition of silver ion, without effectively increasing the volume.
(a) Which will precipitate first, AgCl or AgI?
(b) At what [Ag+] will the first precipitate appear?
(c) At what [Ag+] will the second precipitate begin to appear?
(d) What will be the concentration of the halide ion first precipitated at the time the second precipitate begins to appear?
(e) What percentage of the original halide ion that first precipitates remains in solution when the second precipitate begins to appear?</p></li>
<li><p>One method for the quantitative determination of [Cl-] is to titrate with standardized silver nitrate using chromate ion as an indicator. The titration reaction precipitates white silver chloride: Ag+ + Cl- → AgCl. When the chloride is virtually exhausted, the next Ag ion added combines with chromate ion, yielding a red silver chromate precipitate that serves as a visible indicator: 2 Ag+ + CrO4(2-) → Ag2CrO4. Ksp for AgCl = 1.6 x 10^-10; Ksp for Ag2CrO4 = 2.2 x 10^-11.
(a) In a certain titration, a 100. ml sample contains 2.5 x 10^-3 mol of Cl-. How many drops (20. drops = 1.0 ml) of 0.10 M AgNO3 will be added before AgCl precipitate first appears?
(b) At what [Ag+] will Ag2CrO4 begin to precipitate if [CrO4(2-)] = 2.6 x 10^-5? Disregard any dilution effect.
(c) What will be the [Cl-] when Ag2CrO4 begins to precipitate?
(d) Again disregarding dilution factors, what percentage of the chloride ion originally present will still be in solution when Ag2CrO4 begins to precipitate?</p></li>
<li><p>Find the solubility of AgSCN (Ksp = 1.2 x 10^-12) in 0.50 M NH3 if Kd = 4 x 10^-8 for Ag(NH3)2. Keep two significant figures.</p></li>
<li><p>You will use .25 M KCN to prevent precipitation of Fe(OH)3 in 6.0 x 10^-4 M Fe(3+) as pH is adjusted to 10.00. What volume of KCN solution is required per liter of Fe(3+) solution? Disregard dilution effects. Ksp = 1.1 x 10^-36 for Fe(OH)3 and Kd = 1.0 x 10^-3 for Fe(CN)6(3-).</p></li>
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