An aqueous solution contains 0.100 M of each Fe+3, Ni+2, and Ag+ and you want to use NaOH(s) to selectively precipitate each metal ion. a) In what order will these metal ions precipitate? b) What is the pH at which each of these metal ions will precipitate? c) After the first precipitate is collected, what is the concentration of the remaining two metal ions in solution? d) After the second precipitate is collected, what is the concentration of the remaining metal ion in solution? e) Is NaOH(s) equally effective for separating the first precipitate as it is for separating the second precipitate? Explain your answer

A solution contains 0.0150 M lead(II) ion. A concentrated sodium iodide solution is added dropwise to precipitate lead iodide (assume no volume change). a At what concentration of I does precipitate start to form? b When [I] = 2.0 103 M, what is the lead-ion concentration? What percentage of the lead(II) originally present remains in solution?

How would the solubility of calcium fluoride be affected by the presence of fluoride ion from another source? What is the solubility of calcium fluoride in a saturated solution of barium fluoride? How does this compare with the value of the solubility of calcium fluoride found in Example 17.4? Is this what you expect?

Some barium chloride is added to a solution that contains both K2SO4 (0.050 M) and Na3PO4 (0.020 M). (a) Which begins to precipitate first: the barium sulfate or the barium phosphate? (b) The concentration of the first anion species to precipitate, either the sulfate or phosphate, decreases as the precipitate forms. What is the concentration of the first species when the second begins to precipitate?

12.109 Copper(II) iodate has a solubility of 0.136 g per 100 g of water. Calculate its molar solubility in water and its Ksp.

A solution is made up by adding 0.839 g of silver(I) nitrate and 1.024 g of lead(II) nitrate to enough water to make 492 mL of solution. Solid sodium chromate, Na2CrO4, is added without changing the volume of the solution. (a) Which salt will precipitate first, Ag2CrO4 or PbCrO4? (b) What is the concentration of the chromate ion when the first salt starts to precipitate?

Crystals of AgBr can be removed from black-and-white photographic film by reacting the AgBr with sodium thiosulfate. AgBr(s)+2S2O32(aq)[Ag(S2O3)2]3(aq)+Br(aq) a What is the equilibrium constant for this dissolving process? b In order to dissolve 2.5 g of AgBr in 1.0 L of solution, how many moles of Na2S2O3 must be added?

The solubility product constant for calcium oxalate is estimated to be 4 109. What is its solubility in grams per liter?

A solution contains 0.00740 M calcium ion. A concentrated sodium fluoride solution is added dropwise to precipitate calcium fluoride (assume no volume change). a At what concentration of F does precipitate start to form? b When [F] = 9.5 104 M, what is the calcium-ion concentration? What percentage of the calcium ion has precipitated?

The Ksp for Q, a slightly soluble ionic compound composed of M22+ and X ions, is 4.5 1029. The electron configuration of M+ is [Xe]6s14f145d10. The X anion has 54 electrons. What is the molar solubility of Q in a solution of NaX prepared by dissolving 1.98 g NaX in 150. mL solution?