The solubility product constant of
Ag4[Fe(CN)6] is Ksp = 1.55 x
10–41. Select the expression for the solubility product
constant.
Let x be the molar solubility.
A. Ksp = [Ag+]4[Fe(CN)6-4] = 256x5
B. Ksp = [Ag+]4[Fe(CN)6-4] = x4
C. Ksp = [Ag+]4[Fe(CN)6-4] = x5
D. Ksp = [Ag+][Fe(CN)6-4] = x2
The solubility product constant of Ag4[Fe(CN)6] is Ksp = 1.55 x 10–41. Select the expression for...
What is the molar solubility of AgCl (Ksp = 1.80 x 10-10) in 0.330 M NH3? (Kf of Ag(NH3)2* is 1 x 107) IM What is the equilibrium constant for the solubility of FeCO3 (Ksp = 2.1 x 10-11) in NaCN? (Kf of Fe(CN)64-is 1.0 x 1035)
Calculate the molar solubility of: a. ZnC2O4 Ksp = 2.70 x 10-8 e. PbCO3 Ksp = 7.39 x 10-14 b. Ag2S Ksp = 6.00 x 10-51 f. Al(OH)3 Ksp = 1.81 x 10-5 c. BaCrO4 Ksp = 1.22 x 10-10 g. CaF2 Ksp = 5.29 x 10-9 d. Mg3(PO4)2 Ksp = 1.01 x 10-25 h. Fe4[Fe(CN)6]3 Ksp = 3.34 x 10-41
1. Calculate the solubility product constant, Ksp, for strontium fluoride if 1.2×10-3mol of F-ion is present in 2.0 L of a saturated strontium fluoride solution. A.9.0×10-8 B.2.7×10-11 C.6.9×10-9 D.1.1×10-10 E.1.4×10-6 2. Choose the correct equilibrium constant expression (Ksp) for the dissolution of Ag2S . (is the answer D?) A. [ Ag2S ] Ksp = [ Ag+]2 [ S2-] B. Ksp = [ Ag+][ S2-]2 C. [ Ag+] [ S2-] Ka = [ Ag2S ] D. Ksp = [ Ag+]2 [...
The solubility-product constant (Ksp) for Cacoz at 25°C is 3.4 x 10-9. What is the molar solubility of this substance in 0.12 M Caci, at 25°C?
a Ni(CN)2, nickel cyanide Ksp-3.0 x 10-23 Molar solubility mo/L [Ni2+] . CN Solubility g/L bPbla, lead(lI) odide Ksp8.7 x 10-9 Molar solubility mo/L Solubility g/L We were unable to transcribe this image
17.78 Copper(II) ferrocyanide, Cu2Fe(CN)6, dissolves to give and [Fe(CN)6Jions; Kgp for Cu2Fe(CN)6 equals 1.3 X 10-16. Calculate: (a) the molar solubility, and (b) the solubility grams per liter of copper(II) ferrocyanide. Cu2+ in
Part A Use the molar solubility, 1.08 x 10-5 M in pure water to calculate Ksp for BaCrO4 Express your answer using three significant figures. Y AL OO ? Ksp = Submit Request Answer Part B. Use the molar solubility, 1.55 X 10' M in pure water to calculate Ksp for Ag, SO3 Express your answer using three significant figures. AED O ? Ksp = Submit Request Answer Part C Use the molar solubility, 2.22 x 10-8 M in pure...
1. Silver chloride, AgCl, has a solubility product constant, Ksp = 1.8 x10-10 at 25°C. What is its solubility in pure water? 2. Silver chloride, AgCl, has a solubility product constant, Ksp = 1.8 x 10-10 at 25° C. What is its solubility in the presence of 0.10 molar sodium chloride?
a) 4.9 x 10'M b)24x10 M c)5.8x 1010 M )1.2 x 10 M 19. Which one of the following compounds will have the lowest molar solubility in pur water? b) CuS, Ksp 1.27x103 d) ZnS, Ksp = 1.6 x 10-24 a) PbS, Ksp 9.04 x 102 e) Al(OH)s, Ksp 3 x 1034 What is the molar solubility, i.e. [Fe , in a saturated aqueous solution of 20. Fe(OH)20) Fe(OH(s)Fe2+(aa) + 201H (ag), Ksp 4.87 x 101" a) 2.44 x 1017...
At 25 0C the solubility product constant, Ksp, for strontium sulfate, SrSO4, is 7.6 x 10-7. The solubility product constant for strontium fluoride, SrF2, is 7.9 x 10-10. (a) What is the molar solubility of SrSO4 in pure water at 25 0C? (b) What is the molar solubility of SrF2 in pure water at 25 0C? (c) An aqueous solution of Sr(NO3)2 is added slowly to 1.0 litre of a well-stirred solution containing 0.020 mole F- and 0.10 mole SO42-...