Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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A saturated AgClAgCl solution was analyzed and found to contain 1.25 x 10-5 M Ag+AgX+ ions. Use this value to calculate the Ksp of AgCl
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- It is found that 8.70e-09 g of Ga(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ga(OH)3.The Ksp of Y2(CO3)3 at 25 oC is 1.03e-31. What is the molar solubility of Y2(CO3)3?arrow_forwardA saturated solution of magnesium fluoride, MgF2, was prepared by dissolving solid MgF2 in water. The concentration of Mg2+ ion in the solution was found to be 1.18×10−3 M . Calculate Ksp for MgF2.arrow_forwardSolid Ag2CO3 is added to water until no more solid Ag2CO3 dissolves. What is the silver ion concentration for the saturated solution of Ag2CO3, if the Ksp for Ag2CO3 is 8.39x10-12? (Ignore any ion hydrolysis.) 4.06 x 10-4 M 2.03 x 10-4 M 2.90 x 10-6 M 1.28 х 104 м 2.56 x 10-4 M None of thesearrow_forward
- The equilibrium concentration of sulfide ion in a saturated zinc sulfide solution is M. (Assume that Ksp (ZnS) = 2.0 × 10-25.)arrow_forwardMeasurement of the concentration of Fe 3+ ions in a saturated solution of Iron(III) chloride was found to be 0.35 M. Calculate the Ksp of Iron(III) chloride.arrow_forwardSuppose a student mixes 5.00 mL of 2.00 x 10 M Fe(NO,), with 4.00 mL of 2.00 x 10- M KSCN and 1.00 ml of water The student then determines the [FENCS] at equilibrium to be 9.25 x 10 M. Find the equilibrium constant for the following reaction. Show all your calcula- tions for each step. Fe + SCN -FENCS Step 1. Calculate the initial number of moles of Fe" and SCN (use Equation 12). moles of Fe* 100105 moles of SCN 80410-6 S00ML o DosooL 2.00101M SCN 400ML . 000400 L 2 00 104u mol Fest •2.0010M D0osooL 1.0e10-5 mel mot sCN 0u D00400L 2.001O 8.0210.6molarrow_forward
- 2- The concentration of SO, in a saturated solution of Hg2SO4 is 5.54x10-3 mol/L at a certain temperature. Calculate the Ksp for the compound at this temperature.arrow_forwardCalculate AG° and K at 25°C for the reactions. а. 7H2O + 2 Cr3+ + 3 Cl2 = Cr207²- + 6 CI¯ + 14H+ 0.03 V cełl AG° = kJ K = b. Cu²+ (aq) + Ba(s) Ba2+ (aq) + Cu(s) ɛ° = 3.24 V AG° kJ К - С. Cl2 (g) + 2 Br (aq) = Br2 (9) + 2 Cl¯ (aq) e° = 0.27 V AG° = kJ K = d. 3H2 O(1) + 5 IO4 (ag) + 2 Mn²+ (aq) = 5 103 (aq) + 2 MnO4¯(ag) + 6H† (ag) = 0.09 V E cel || AG° kJ K =arrow_forwardPlease use the values in the resources listed below instead of the textbook values. Perform the following calculations involving concentrations of iodate ions. (a) The iodate ion concentration of a saturated solution of Ce(IO3)4 was found to be 7.35X10 mol/L. Find the Ksp: 4.0 (b) Find the concentration (in M) of iodate ions in a saturated solution of Ra(IO3)2. (Ksp = 1.16X 10-9) 4.0) Marrow_forward
- Please answer the following neatly, clearly and thoroughly! Thanksarrow_forwardCalculate molar solubility of AgCl in pure water. The K for Silver Chloride is: 1.83 x 10 10 O 183e-10 0 135e-5 O 1.35e+5arrow_forward1. The Ksp for Mg(OH)2 is 5.6 x1012. Determine the molar solubility of Mg(OH)2 in a solution of 0.010 M Ca(OH)2.arrow_forward
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