I found that the molar solubility of Calcium Sulfate is 0.00490 if its Ksp is 2.40x10^-5....
Be sure to answer all parts. The solubility of calcium sulfate at 30°C is 0.209 g/100 mL solution. Calculate its Ksp. Ksp = x 10
Calculate the solubility (g/L) of calcium sulfate, CaSO4 in units of grams per liter. Ksp(CaSO4) = 2.4E-5
The solubility of calcium sulfate at a given temperature is 0.02005 g/L. Calculate the Ksp at this temperature. After you get your answer, take the negative log and enter that (so it's like you're taking the pKsp). (Note: sulfate ion molar mass = 96.07 g/mol)
Which compound listed below has the highest molar solubility in water? Calcium hydroxide Ca(OH)2 Ksp= 5.5x10-6 Calcium oxalate CaC204 Ksp= 2.7x10-9 Calcium phosphate Ca3(PO4)2 Ksp=2.0x10-29 Calcium sulfate CaSO4 Ksp= 9.1x10-6 A. CaC204 B. They are all equally insoluble C. Ca(OH)2 D. Ca3(PO4)2 E. CaSO4
QUESTION 17 1 point The solubility of calcium sulfate at a given temperature is 0.02005 g/L. Calculate the Ksp at this temperature. After you get your answer, take the negative log and enter that (so it's like you're taking the pksp). (Note: sulfate ion molar mass = 96.07 g/mol)
G. Common ion effect 1. What is the molar solubility of calcium hydroxide (Ksp 5.5 x 10) under the following conditions? . In pure water. ii. In water with a pH of 7.25 iii. In water with a pH of 12.50 2. What is the molar solubility of lead (II) fluoride (Ksp 2.7 x 10) under the following conditions? i. In pure water. ii. In a 2.5 x 105 M NaF solution
a) Ksp = 1.2 x 10-5 for Ag2SO4, then calculate its molar solubility. b) If Ksp = 1.2 x 10-5 for Ag2SO4, then calculate its mass solubility in g solute/100g of water. Please answer a & b
Q1: Part 1) The solubility product (Ksp) of AuCl3(s) is 3.2 × 10-25. Calculate the molar solubility of AuCl3(s) in pure water and with the molar solubility found, calculate the solubility of AuCl3(s) in units of mg AuCl3/mL in pure water. The molar mass of AuCl3 is equal to 303.33 g AuCl3/mol AuCl3. Part 2 )Calculate the molar solubility of AuCl3(s) in an aqueous 1.5 M NaCl solution. Q2: Calculate the pH of a solution if 75.0 mL of 0.195...
(a) If the molar solubility of Tl, at 25°C is 5.31e-08 mol/L, what is the Ken at this temperature? Ksp = (b) It is found that 4.68e-06 g of Nd2(CO3)3 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility-product constant for Nd2(CO3)3. Ksp = (c) The Ksp of BaF2 at 25 °C is 1.84e-07. What is the molar solubility of BaFZ? solubility = mol/L
28. -70.1 points 0/4 Submissions Used (a) If the molar solubility of YF3 at 25 °C is 4.23e-06 mol/L, what is the Ksp at this temperature? Ksp =D (b) It is found that 0.0628 g of BaF2 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility-product constant for BaF2. Ksp = (c) The Ksp of Ca3(PO4)2 at 25 °C is 2.05e-35. What is the molar solubility of Ca3(PO4)2? solubility = mol/L