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General Chemistry: Principles and Modern Applications (11th Edition)
- Calcium nitrate is added to a sodium sulfate solution that is 0.0150 M. (a) At what concentration of Ca2+ does a precipitate first start to form? (b) Enough Ca(NO3)2 is added to make [ Ca2+ ]=0.0075 M. What percentage of the original sulfate ion has precipitated?arrow_forwardA 3.20-L solution of 1.25 103 M Pb(NO3)2 is mixed with a 0.80-L solution of 5.0 101 M NaCl. Calculate Q for the dissolution of PbCl2. No precipitate has formed. Is the solution supersaturated, saturated, or unsaturated?arrow_forwardHow do the concentrations of Ag+ and CrO42- in a saturated solution above 1.0 g of solid Ag2CrO4 Change when 100 g of solid Ag2CrO4 is added to the system? Explain.arrow_forward
- What is [Br-] just as AgCl begins to precipitate when 1.5 M AgNO3 is slowly added to a solution containing 0.050 M Cl- and 0.050 M Br-?arrow_forwardMixtures of metal ions in aqueous solution can sometimes be separated by selective precipitation. What is selective precipitation? If a solution contained 0.10 M Mg2+, 0.10 M Ca2+, and 0. 10 M Ba2+, how could addition of NaF be used to separate the cations out of solutionthat is, what would precipitate first, then second, then third? How could addition of K3PO4 be used to separate out the cations in a solution that is 1.0 M Ag+, 1.0 M Pb2+, and 1.0 M Sr2+?arrow_forwardTo a 0.10-M solution of Pb(NO3)2 is added enough HF(g) to make [HF]=0.10M. (a) Does PbF2 precipitate from this solution? Show the calculations that support your conclusion. (b) What is the minimum pH at which PbF2 precipitates?arrow_forward
- When 5 M ammonia is added to a solution containing Cu(OH)2(s), the precipitate will eventually dissolve in solution. Why? If 5 M HNO3 is then added, the Cu(OH)2 precipitate re-forms. Why? In general, what effect does the ability of a cation to form a complex ion have on the solubility of salts containing that cation?arrow_forwardA solution is made up by adding 0.632 g of barium nitrate and 0.920 g of lanthanum nitrate, to La(NO3)3 enough water to make 0.500 L of solution. Solid sodium iodate, NalO3, is added (without volume change) to the solution. (a) Which salt will precipitate first? La(IO3)3 (Ksp=7.501012) or BAIO3 (Ksp=4.0109)? (b) What is [IO3-] when the salt in (a) first begins to precipitate?arrow_forwardThe 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?arrow_forward
- What mass of Ca(NO3O)2 must be added to 1.0 L of a 1.0-M HF solution to begin precipitation of CaF2(s)? For CaF2, Ksp = 4.0 1011 and Ka, for HF = 7.2 104. Assume no volume change on addition of Ca(NO3)2(s).arrow_forwarda If the molar solubility of beryllium(II) hydroxide is 8.6 107 M in pure water, what is its Ksp value? b What is the molar solubility of beryllium(II) hydroxide in a solution that is 1.50 M in NH3 and 0.25 M in NH4Cl? c Account for the differences in molar solubility in parts a and b.arrow_forwardConsider a 2.0-L aqueous solution of 4.17 M NH3, where 21.0 g of NH4Cl are dissolved. To this solution, 4.8 g of CaCl2 are added. (a) What is [OH-] before CaCl2 is added? (b) Will a precipitate form? (c) What is [Ca2+] after equilibrium is established?arrow_forward
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