Please answer these questions: -Calculate the molar solubility of Cr2(CrO4)3 (Ksp = 6.47 x 10-22) in...
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...
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.
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...
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?
Calculate the molar solubility of BaSO4 (Ksp for BaSO4 2.2x10^-10) A) in water B) in a solution 4.00M SO4 2- (Use ICE table when solving)
Be sure to answer all parts. Find the molar solubility of BaCrO4 (Ksp 2.1 x 10 10) in (a) pure water x 10 М (b) 2.3 x 103 M Na2 CrO4 x 10 М
he solubility product (Ksp) of PbBr2 is 8.9 X 10. Please calculate the molar solubility in: A) Pure water B) 0.20 M Pb(NOs)2 Pb Brs) Pbap +2 Br 8.9- M0T 2 LOZJLES . 45 25 O.Zts Zs 4.45./05 4 4s 0.2x0.2+s 13:105- J S0-60334 9. The solubility of an ionic compound MX (molar mass = 346 g/mol) is 4.63 X 103 g/L. What is the Ksp for this compound? HoW
Calculate the molar solubility, S, of Ag2(Cros) in a 0.414 MK (CrO4) solution. Note that K2 (Cro) is highly soluble and the Ksp of Ag2 (CrO ) is 9.00 x 10-12 S 3.73e-12
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...
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