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Will Agl(s) precipitate from a solution with
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- Calculate the solubility of copper(II) iodate, Cu(IO3)2 (Ksp = 7.4 108), in (a) water. (b) a 0.10 M copper(II) nitrate solution.arrow_forwardAssuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products): (a) Agl. (b) Ag2SO4. (c) Mn(OH)2. (d) Sr(OH)28H2O (e) the mineral brucite, Mg(OH)2arrow_forwardThe solubility of cadmium oxalate. CdC2O4, in 0.150 M ammonia is 6.1 103 mol/L. What is the oxalate-ion concentration in the saturated solution? If the solubility product constant for cadmium oxalate is 1.5 108, what must be the cadmium-ion concentration in the solution? Now calculate the formation constant for the complex ion Cd(NH3)42+.arrow_forward
- What additional information do we need to answer the following question: How is the equilibrium of solid silver bromide with a saturated solution of its ions affected when the temperature is raised?arrow_forwardWhat is the solubility of silver oxide, Ag2O, in a solution buffered at pH 10.78? The equilibrium is Ag2O(s) + H2O(l) 2Ag+(aq) + 2OH (aq); Kc = 2.0 108.arrow_forwardPredict whether nickel(II) hydroxide, Ni(OH)2, will precipitate from a solution that is 0.0020 M NiSO4, 0.010 M NaOH, and 0.10 M NH3. Note that nickel(II) ion forms the Ni(NH3)62+ complex ion.arrow_forward
- Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products). (a) TlCl. (b) BaF2. (c) Ag2CrO4. (d) CaC2O4H2O (e) the mineral anglesite, PbSO4arrow_forwardAt 25C, 10.24 mg of Cr(OH)2 are dissolved in enough water to make 125 mL of solution. When equilibrium is established, the solution has a pH of 8.49. Estimate Ksp for Cr(OH)2.arrow_forwardSolid Pbl2 (Ksp = 9.8 109) is placed in a beaker of water. After a period of time, the lead(II) concentration is measured and found to be 1.1 103 M. Has the system reached equilibrium? That is, is the solution saturated? If not, will more Pbl2 dissolve?arrow_forward
- 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)arrow_forwardCu + Zn^2+ ---> Zn + Cu^2+ Rationalize the possibility of this reaction (Will this reaction take place. Explain)arrow_forwardConsidering that ferrous hydroxide (Fe(OH)2) has a Kps of 6,3 x 10^-18, what is the pH at which precipitation of a 0,01 mol L-1 solution of Fe2+ starts? 6,9 7,7 6,6 6,1 6,4arrow_forward
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