If x = molar solubility, Ksp = solubility product, which of the following compounds would have the relationship: 27x4 = Ksp?
a) Bi2S3
b) Ag2CO3
c) AgCl
d) PbI2
e) Ag3PO4
If x = molar solubility, Ksp = solubility product, which of the following compounds would have...
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
4) Calculate the molar solubility of the following compounds: a. CuCI, Ksp = 1.2x106 b. Mg(OH)2, Ksp = 8.9x10-12 c. Ag3PO4, Ksp = 1.8 x10-18 d. Rank these from least soluble to most soluble
Complete Table 1: Ksp data Salt [cation] (M) [anion] (M) molar solubility (M) Ksp AgCl SrSO4 Ag2CO3 Sr(IO3)2 1) Rank the salts in order of increasing molar solubility. 2) Rank the salts in order of increasing Ksp (remember 10–10 < 10–5) 3) If these rankings are not in the same order, why might Ksp not always scale directly with molar solubility? Design experiments in the virtual lab to answer the follow questions, 1). Use the virtual lab to determine the...
Find the molar solubility of PbI2. Ksp=7.1e-9, then given the molar solubility from the previous answer, what is the solubility of PbI2, in grams per litre? Knowing this, would PbSO4 (Ksp=1.6e-8) have a higher molar solubility than PbI2? (I'm thinking PbSO4 would be higher, since the Ksp is larger?)
1)Use the virtual lab to determine the solubility product (Ksp) for the following solids. Show all work for credit. *should be able to use the lab to determine the ion concentrations at equilibrium and use these for the formulas for KSP and then the KSP'S for solubility. The lab is just to help you get the ion concentration (a). AgCl (b). SrSO4 (c). Ag2CO3 (d). Sr(IO3)2 2) What is the solubility of the solids listed in question 1, in moles/liter?...
If the Ksp of Ag2CO3 at 25 oC is 8.46e-12 , what is the molar solubility of Ag2CO3 at this temperature? a) At this temperature the molar solubility of Ag2CO3 is 6.05e-34 mol/L. b) At this temperature the molar solubility of Ag2CO3 is 2.04e-04 mol/L. c) At this temperature the molar solubility of Ag2CO3 is 2.91e-06 mol/L. d) At this temperature the molar solubility of Ag2CO3 is 1.28e-04 mol/L. e) At this temperature the molar solubility of Ag2CO3 is 2.42e-33...
Answer the following questions regarding molar solubility and Ksp. a.) Calculate the molar solubility of Pbly if its Ksp value is 1.4 x 10-8. b.) Calculate the Ksp of AgCl if its molar solubility is 1.33 x 10-5 M.
Which of the following compounds will have the highest molar solubility in pure water? PbSO4, Ksp = 1.82
28. Which of the following compounds will have the highest molar solubility in pare water? A) PbsO4, Ksp-1.82x 10-8 B) MgcOs. Ksp-6.82 106 C) Ag, Ksp-8.51x 10-17 D) Pbs, Ksp-904 × 10-29 E) FeS, Ksp-3.72 10-19 29. Give the expression for the solubility product constant for PbCl2. [PbCl2l IPbCl2l D) Pbci2l 30. Determine the molar solubility of Agl in pure water. Ksp (Agl)-8.51 A) 9.22 x 10-9 M B) 4.26 × 10-17 M C)8.51 10-17M D)2.77 × 10-6 M E)...
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?