At a certain temperature, the solubility product constant* of copper () iodate,

Question

At a certain temperature, the solubility product constant* of copper () iodate, Cu(0312, is 4.06x10-8 M3. Calculate the solubility of this compound for this temperature. Unless stated otherwise all solubility product constants are for water. Answer: Caloulate the solubility of copper () lodate in 0.21 M copper (p nitrate. Kap is 7.4K10-8 M3 "You should know that the Ksp must refer to the copper iodate because all nitrate compounds are soluble and strong electrolytes! Answer: Warm UP Question. What is the initial (before any reaction takes place) lead nitrate concentration when 9.0 mL of 0.237 M lead nitrate is added to 17 mL of 0.0061 M sodium chloride? Answer: For the reaction: PbCl2(s)?Pb2'aq)+2Cl?-(aq), what is Q* when 7.5 mL of 0.099 M lead nitrate is added to 14 mL of 0.025 M sodium chloride? Ksp of lead chioride is 1.6 x 10 M3 Hint given in general feedback Recall: Q is compared to Ksp to determine whether a precipitate forms Answer: Sodium phosphate is added to a solution that contains 0.0062 M aluminum nitrate and 0.017 M calcium chloride. The concentration of the first ion to precipitate (either A3+ or Ca2+) decreases as its precipitate forms. What is the concentration of this ion when the second ion begins to precipitate? Answer:

Explanation / Answer

According to chegg rules we have to answer only first one problem

Cu(IO3)2   <-----> Cu2+   +   2 IO3-
                                     s                 2s

Let assume that solubility is s

Ksp = [Cu2+][IO3-]^2

Ksp = s * (2s)^2

4.06*10^-8 M^3 = 4*s^3

s^3 = 4.06*10^-8 M^3 / 4

s = 2.17*10^-3 M

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