Calculate the molar solubility of compounds in the following conditions:
a. MgCO3 (Ksp = 3.49 x 10-8) in a solution containing 0.175 M Na2CO3?
b. BaF2 (Ksp = 1.01 x 10-6) in a solution containing 0.125 M KF?
c. Ag2CrO4 (Ksp = 1.12 x 10-12) in a solution containing 0.450 M Na2CrO4?
d. Cu3(AsO4)2 (Ksp = 7.57 x 10-36) in a solution containing 0.325 M CuCl2?
e. Ca3(PO4)2 (Ksp = 1.99 x 10-29) in a solution containing 0.325 M K3PO4?
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Calculate the molar solubility of compounds in the following conditions: a. MgCO3 (Ksp = 3.49 x...
Explain, with calculations and words, what will happen to the molar solubility of Cu3(AsO4)2 (Ksp = 7.6 x 10-76) in a 0.35 M Na3AsO4 (This is 100% soluble) solution.( ICE table please)
Calculate the solubility of Ca3(PO4)2 in a solution containing 0.0539 M Na3PO4. Ksp=2.0*10^-29 for Ca3(PO4)2
Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water. Part A MX ( K sp = 5.30×10−11) Express your answer in moles per liter. Part B Ag2CrO4 (Ksp = 1.12×10−12) Express your answer in moles per liter. Part C Ni(OH)2 (Ksp = 5.48×10−16) Express your answer in moles per liter.
what is the molar solubility of Ca2+ in a 1.00 M aqueous solution of Ca3(PO4)2 (Ksp for calcium phosphate is 2.0 x 10^-29)
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
Determine the molar solubility of BaF2 in a solution containing 0.0750 M LiF. Ksp, BaF2 = 1.7 X 10-6. Which one of these is the correct answer? BaF2 molar solubility = 2.3 x 10-5 M BaF2 molar solubility = 0.0750 M BaF2 molar solubility = 8.5 x 10-7 M BaF2 molar solubility = 1.2 x 10-2 M BaF2 molar solubility = 3.0 x 10-4 M
Calculate the molar solubility of CaF2 in a solution containing 0.325 M of Ca(NO3)2. The Ksp value for CaF2 is 1.46×10−10. can you also explain me how to solve for X toward the end of the problem
Please answer these questions: -Calculate the molar solubility of Cr2(CrO4)3 (Ksp = 6.47 x 10-22) in a 0.25M Na2CrO4 solution. USE AN ICE TABLE Calculate the molar solubility of AuCl3 (Ksp = 3.2 x 10-25) in a 0.65 M MgCl2 solution. USE AN ICE TABLE
a) The solubility product, Ksp, of Cd3(PO4)2 is 2.5 x 10-33. What is the solubility (in g/L) of Cd3(PO4)2 in pure water? b) The solubility product of Cu(OH)2 is 4.8 x 10-20. Calculate the value of pCu2+, or -log[Cu2+], in an aqueous solution of NaOH which has a pH of 12.38 and is saturated in Cu(OH)2. c) The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if we were to...
Which of the following compounds has the highest molar solubility? A. PbS; Ksp = 8.4 x 10-28 B. PbSO4; Ksp = 1.8 x 10-8 C. PbCO3; Ksp = 1.5 x 10-13 D. PbI2; Ksp = 8.7 x 10-9 E. Pb3(PO4)2; Ksp = 3.0 x 10-44