18. In order to answer this question, we need to know the molar solubility of Sr3(PO4)2 which is 1.0*10-31. We need to write down the dissociation equation and set up the ICE chart.
Sr3(PO4)2 ç=====è 3 Sr2+ + 2 PO4
Let x mole/L be the molar solubility of Sr3(PO4)2. Then the solubility of Sr2+ and PO43- will be 3x and 2x as per the dissociation equation. Also, we have 0.025 M Sr(NO3)2 which furnishes 0.025 mole/L Sr2+. Therefore,
Ksp = [Sr2+]3[PO43-]2 = (0.025 + 3x)3(2x)2 where Ksp is the solubility product of Sr3(PO4)2. We need to make an assumption here: x << 0.025 and hence [Sr2+] = 0.025. Therefore,
1.0*10-31 = (0.025)3(2x)2 = (1.5625*10-5).(4x2) = 6.25*10-5.x2
=è x2 = 1.6*1027
=è x = 4.0*10-14
The molar solubility of Sr3(PO4)2 in 0.025 M Sr(NO3)2 is 4.0*10-14 M (ans).
19. The molar solubility of Zn(OH)2 is 5.7*10-3 mol/L at a certain temperature. The dissociation of Zn(OH)2 occurs as
Zn(OH)2 ç==è Zn2+ + 2 OH-
[Zn2+] = 5.7*10-3 mol/L
[OH-] = 2*5.7*10-3 mol/L; this is as per the dissociation equation. Therefore,
Ksp = [Zn2+][OH-]2 = (5.7*10-3).(2*5.7*10-3)2 = 7.407*10-7 ≈ 7.41*10-7 (ans).
The molar solubility of CuCl in water is 1.0*10-3 mol/L. The dissociation of CuCl takes place as
CuCl ç===è Cu+ + Cl-
[Cu+] = 1.0*10-3 mol/L
[Cl-] = 1.0*10-3 mol/L; this is as per the dissociation equation. Therefore,
Ksp = [Cu+][Cl-] = (1.0*10-3).(1.0*10-3) = 1.0*10-6 (ans).
025 M Sr(NOh M Sr(NO,) 3)2- Calculate the molar solubility of Sr,(PO)h in 0.025 M S...
QUESTION 1 If the solubility of iron(III) hydroxide Fe(OH)3 is s, what is the value of Ksp equal to? Ksp = 353 Ksp=9s3 Ksp = 954 Ksp = 354 Ksp = 2754 QUESTION 2 At a certain temperature the Ksp of Ni(OH)2 is 5.68 x 10-16. What is the molar soliubility of nickel(l) hydroxide in water in units of M (mol/liter)? Express your answer in scientific notation.
b. calculate the molar solubility(s) and from that the Ksp of Ba(OH)2 at 0*c. c. calculate the delta G* for the dissolution of Ba(OH)2 from the Ksp calculated in part b, at 0*c. Section: Date: Pre-Lab Questions 1. A 10.0 mL sample of Balohi, at Or is itrated with 200 M HCL and 5.22 ml of the acid are used to reach the yellow endpoint. a. Calculate the concentration of OH in the 10.0 mL sample of BalOH) at O'C....
Determination of a Solubility Product and Observation of the Common lon Effect . Calculate the molar solubility in mol/L for Zn(OH): in water. Zn(OH): has a Kap value of 1.8 x 10. Also, fill in the provided ICE table in solving this problem. Zn(OH)2(s)Zn2 (ag)20H (aq) Initial concentration (M Change in concentration (M) Equilibrium concentration (M From the molar solubility in question 1, calculate the concentration of OH ions in solution, and the pH of the solution. . Two 10.0...
Calculate the molar solubility of Fe(OH)3, Ksp=4 x10^-38, Molar solubility = mol/L
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...
What is the molar solubility of AgCl in 0.025 M CaCl2? For AgCl, Ksp = 1.6 x 10-10. You can assume that molar solubility, s, is very small. Select one: a. 1.6 x 10-11 M b. 3.2 x 10-9 M c. 8.5 x 10-12 M d. 2.5 x 10-10 M e. 6.2 x 10-13 M
Calculate the molar solubility of Zn(OH)2 given that Ksp at 25°C is 3.00×10-16. Calculate the solubility (in grams per litre) of Zn(OH)2.
(a) If the molar solubility of Ca3(PO4)2 at 25 oC is 4.53e-08 mol/L, what is the Ksp at this temperature? Ksp = (b) 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. Ksp = (c) The Ksp of Ag2C2O4 at 25 oC is 5.40e-12. What is the molar solubility of Ag2C2O4? solubility = mol/L
Questions: 1. Calculate the Ksp for PbBr2 if its molar solubility is 2.14 x 10-2 M at 25°C. 2. Calculate the molar solubility of CaF2 (Ksp = 4.0 x 10-11) in a 0.025 M NaF solution. 3. Solid sodium sulfate, Na2SO4, is added slowly to a solution that is 1.0 x 10-4 in both Ba2+ and Pb2+ until [SO42-] reaches 1.0 x 10-4 M. Would either BaSO4 (Ksp = 1.1 x 10-10) or PbSO4 (Kop -1.7 x 10-8) precipitate under...
My Notes (a) If the molar solubility of Cd3(PO4)2 at 25 oC is 1.19e-07 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 1.08e-09 g of Fe(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Fe(OH)3. Ksp = (c) The Ksp of Ga(OH)3 at 25 oC is 7.28e-36. What is the molar solubility of Ga(OH)3? solubility = mol/L