Question 2 2.1 The Ksp of Cu3 (PO4), is 1.00 x 10-37. Estimate the solubility of this salt in units of g. L. You must show any reaction equation(s) that you may think are necessary. If a sample of solid Cu3(PO4)2 is stirred into exactly one litre of a 0.550M solution of K3P04, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence. 2.2

Question 2 2.1 The Ksp of Cu3 (PO4), is 1.00 x 10-37. Estimate the solubility of this salt in units of g. L. You must show any reaction equation(s) that you may think are necessary. If a sample of solid Cu3(PO4)2 is stirred into exactly one litre of a 0.550M solution of K3P04, how will the solubility of the salt compare with the answer that you have obtained in question 2.1? Explain you answer in a short sentence. 2.2

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Chapter21: Chemistry Of The Main-group Elements

Section: Chapter Questions

Problem 21.195QP

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A mixture of xenon and ?uorine was heated. A sample of the white solid that formed reacted with hydrogen to yield 81 ml of xenon (at STP) and hydrogen ?uoride, which was collected in waiter, giving a solution of hydro?uoric acid. The hydro?uoric acid solution was titrated, and 68.43 mL of 0.3172 M sodium hydroxide was required to reach the equivalence point. Determine the empirical formula for the white solid and write balanced Chemical equations for the reactions involving xenon.
The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
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We began the chapter with an informal discussion of how the mineral fluorite (as shown) is formed. Fluorite, CaF2, is a slightly soluble solid that dissolves according to the equation: CaF2(s) ⇌ Ca2+(aq) + 2F−(aq)The concentration of Ca2+ in a saturated solution of CaF2 is 2.15 × 10–4 M; therefore, that of F– is 4.30 × 10–4 M, that is, twice the concentration of Ca2+. What is the solubility product of fluorite?
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