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CHM116 week 5 disc probs

CHM116 week 5 disc probs - 2 in a solution buffered at pH =...

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Use the K sp values in table 16.2 (p 747) to calculate the “molar solubility” of each of the following compounds in pure water at 25 ºC. a) CuS b) Ag 2 CrO 4 c) Ca(OH) 2 1. Week 5 discussion problems Use the given molar solubilities in pure water to calculate K sp for each of the following compounds: a) BaCrO 4 ; molar solubility = 1.08 x 10 -5 M b) b) Ag 2 SO 3 ; molar solubility = 1.55 x 10 -5 M c) Pd(SCN) 2 ; molar solubility = 2.22 x 10 -8 M 2. Calculate the molar solubility of copper(II) sulfide in each of the following: ( K sp = 1.27 x 10 -36 ) a) In pure H 2 O b) b) In 0.25 M CuCl 2 c) In 0.20 M K 2 S 3.
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Calculate the solubility of Mg(OH)
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Unformatted text preview: 2 in a solution buffered at pH = 10. How does this compare to the solubility of magnesium hydroxide in pure H 2 O? 4. Determine whether or not each of the following compounds will be more soluble in acidic solution than in pure water. a) Hg 2 Br 2 b) Mg(OH) 2 c) CaCO 3 d) AgI 5. A solution containing potassium bromide is mixed with one containing lead acetate to form a solution that is 0.013 M in KBr and 0.0035 M in Pb(CH 3 COO) 2 . Will a precipitate form in the mixed solution? If so, identify the precipitate. 6....
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