Calculate for the equilibrium or solubility constant of the dissolution of 0.065 m M2SO4 with the reaction: M2SO46) + M2+ + so,²- The data for calculation are as follows: I (ionic strength) = 0.08 Species Mean activity coefficient NazSO4 0.71 MCI 0.52 NaCl 0.83 CuCl2 0.44 KCI 0.85 CuzSO4 0.46 Hint: Use the Mean Salt Method which uses the behavior of KCI where for MCI, Y+McI = [(YM+)(rcr-)] V±mci = [(Ym+)(Yxci)jž

Calculate for the equilibrium or solubility constant of the dissolution of 0.065 m M2SO4 with the reaction: M2SO46) + M2+ + so,²- The data for calculation are as follows: I (ionic strength) = 0.08 Species Mean activity coefficient NazSO4 0.71 MCI 0.52 NaCl 0.83 CuCl2 0.44 KCI 0.85 CuzSO4 0.46 Hint: Use the Mean Salt Method which uses the behavior of KCI where for MCI, Y+McI = [(YM+)(rcr-)] V±mci = [(Ym+)(Yxci)jž

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter9: Aqueous Solutions And Chemical Equilibria

Section: Chapter Questions

Problem 9.10QAP

See similar textbooks

Similar questions

Calculate a the solubility product constant for Ag2CO3 and b the value of Kw using the following data: Ag2CO3(s)+2e2Ag(s)+CO32(aq)E=0.47VAg+(aq)+eAg(s)E=0.7996VO2(g)+2H2O(l)+4e4OH(aq)E=0.401VO2(g)+4H+(aq)+4e2H2O(l)E=1.229V
Please calculate for the equilibrium or solubility constant of the dissolution reaction below:
Calculate the solubility of silver acetate.1 (CH;COOA9) in water at 25 °C, assuming * .the DHLL to apply; Ksp = 0.004 M²
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that changes inthe initial concentrations of the common ions can be neglected.(a) AgCl(s) in 0.025 M NaCl(b) CaF2(s) in 0.00133 M KF(c) Ag2SO4(s) in 0.500 L of a solution containing 19.50 g of K2SO4(d) Zn(OH)2(s) in a solution buffered at a pH of 11.45
Calculate Kn for each salt in an aqueous solution at 25 °C in which u = 0.0100 M. Use the table of K, values and a Compound Formula Kp barium phosphate Ba, (PO,), 3.40 x 10-2 cobalt(II) phosphate Co, (PO,), 2.05 x 10-3 La(IO,), 7.50 x 10-12 table of activity coefficients to solve this problem. lanthanum iodate ZNCO, magnesium Mg,(PO,)1.04 x 10-24 phosphate potassium periodate KIO, 3.71 x 10 scandium hydroxide Sc(OH), 2.22 x 10-31 A SCN 1.03 x 10-12 Sc(OH), %3D silver thiocyanate Y(10,), 1.12 x 10-10 ZNCO, 146 x I10-10 yttrium iodate zinc carbonate Co, (PO,), Kp
Assuming that no equilibria other than dissolution are involved, calculate the concentration of all solute species in each of the following solutions of salts in contact with a solution containing a common ion. Show that it is notappropriate to neglect the changes in the initial concentrations of the common ions.(a) TlCl(s) in 0.025 M TlNO3(b) BaF2(s) in 0.0313 M KF(c) MgC2O4 in 2.250 L of a solution containing 8.156 g of Mg(NO3)2(d) Ca(OH)2(s) in an unbuffered solution initially with a pH of 12.700
Calculate the solubility of CaF2 (aq) in a solution, that is 0.015 molar in MgSO4 (aq). Compare your result to the one you obtain by using concentration instead of activities. Take the solubility product as 3.9 × 10 ^-11
For the aqueous Hg(NH,), complex K, = 1.8 × 101º at 25 °C. K; =1 Suppose equal volumes of 0.0010M Hg(NO,), solution and 0.20M NH, solution are mixed. Calculate the equilibrium molarity of aqueous Hg“ ion. 2 Round your answer to 2 significant digits. M ?
I need ans within 15 minutes my best wishes ton
(a) I f t he molar solubilit y o f CaF2 at 35 °C i s1.24 x 10-3 mol/L, what is Ksp at this temperature? (b) It isfound that 1.1 x 10-2 g SrF2 dissolves per 100 mL of aqueoussolution at 25 °C. Calculate the solubility product forSrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 x 10-10. What isthe molar solubility of Ba(IO3)2?
For the aqueous [Hgl, complex K,6.76 x 10 at 25 "C. Suppose equal volumes of 0.0092M Hg(NO,), solution and 0.20M Nal solution are mixed. Calculate the equilibrium molarity of aqueous Hg lon. 2+ Round your answer to 2 significant digits.
If you want to dissolve 0.225 grams of AgBr, what volume of 0.0138M Na2S2O3 in mililiters, should be used