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GENERAL CHEMISTRY(LL)-W/MASTERINGCHEM.
- 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_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_forwardWhen 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_forward
- A 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_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_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_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_forwardYou place 1.234 g of solid Ca(OH)2 in 1.00 L of pure water at 25 C. The pH of the solution is found to be 12.68. Estimate the value of Ksp for Ca(OH)2.arrow_forward
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