Consider the solubility of CaSO4 (Ksp = 2.4E-5). Find [Ca2+] in 0.013 M KNO3. Approach: 1....
The Ksp of CaSO4 is 2.4x10-5. What is the molar solubility of CaSO4 in 0.11 M aqueous Ca(NO3)2? 0 2.2x104 4.9x10-3 8.7x10-6 1.5x10-2 1.8x10-5
Calculate the solubility of CaSO4 (Ksp = 2.4 x 10^-5) in distilled water and in 0.025 M K2SO4 (include acitvity effects). The ionic diameter for Ca^2+ is 0.6, and the ionic diameter for SO4^2- is 0.4.
Determine the molar solubility of CaSO4 in a solution containing 9.0×10−2 M K2SO4. Ksp (CaSO4) = 7.1×10-5. 8.4×10-3 M 5.0×10-9 M 7.9×10−4 M 2.2×10−3 M 6.4×10−6 M
Consider a solution that is 1.3×10−2 M in Ba2+ and 1.8×10−2 M in Ca2+. Ksp(BaSO4)=1.07×10−10 Ksp(CaSO4)=7.10×10−5 *Part A: If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? If sodium sulfate is used to selectively precipitate one of the cations while leaving the other cation in solution, which cation will precipitate first? A) Ba2+ (ANSWER) B) Ca2+ *Part B: What minimum concentration of Na2SO4 is required...
Please explain Solubility Equilibria and the Solubility Product Constant. Below you will find key questions. 1. Know that the solubility product constant, Ksp, defines the equilibrium constant for the dissolution of an ionic compound into its constituent ions. 2. Calculate the molar solubility of an ionic compound in pure water using the Ksp expression and an ICE table. 3. Know that the solubility of an ionic compound is lower in a solution containing a common ion than in pure water....
Write the chemical equation for the
solubility equilibrium and the Ksp expression for each
compound please help and explain steps
AgI First, write the solubility equilibrium for Agi. Include physical states in your answer: ? Edit Next, write the solubility product constant for Agi: OK = [Ag+][I-12 sp sp Ksp = ([Ag+][1-)) / [AgI] Okn = [Agl] / [[Ag+][1-1) Ksp = [Ag+][1-) AuCl3 First, write the solubility equilibrium for AuCl3. Include physical states in your answer: |? Edit Next, write...
Consider a saturated solution of La(OH)3 in 0.10 M KNO3 at 25 °C. For La(OH)3, Ksp = 2.0 x 10-21. Including activities, calculate the concentration of lanthanum ions What is the pH in this saturated solution? Again, include activities. Why is the answer in part (b) still not the pH you'd measure for an actual saturated solution of lanthanum hydroxide?!
1 1 3 points A group of ionic compounds have the following solubility constants. Which would be the most soluble? Mg(OH)2 Ksp = 2.06x10-12 CaCo3 Ksp - 4.96X10-9 CaSO4 Ksp = 7.10x10-5 BaF2 Ksp = 2.45x10-6
Part A.) Ksp(Li2CO3) = 8.2x10-4, Ksp(LiF) = 1.8x10-3 Consider a solution that is 0.155 M in CO32- and 0.364 M in F-. If lithium nitrate is used to selectively precipitate one of the anions while leaving the other anion in solution, what % of the first ion remains in solution at the moment when the second ion starts precipitating? Enter your answer numerically to three sig figs. Part B.) If 500.0 mL of 0.1 M Ca2+ is mixed with 500.0...
Date: Name: Experiment 10: Solubility Product PRE-LABORATORY QUESTIONS 1. Write the net ionic equilibrium equation for the dissolution of KHC.H06 in water. 2. Write the solubility product constant expression for KHC4H406. 3. Why is it not necessary to record the exact mass of KHT placed into the flasks? 4. The solubility of calcium oxalate, CaC204, is 4.8x10 mol/L. What is its Ksp? 5. The solubility product constant for MgF2 is 3.4x10-1. What is its solubility?