The Ksp for Ca 2(s) is 4.0x01. Calculate the solubility of CaF2(s). Ignore any potential reaction...
References CHEMWORK The Kp for CaF2(8) is 4.0x10-" Calculate the solubility of CaF2(s). Ignore any potential reaction of the ions with water. Solubility for CaFz(s) = mol/L Submit Show Hints
Calculate the molar solubility of CaF2 in each of the following solvents. Ignore any potential reactions of the ions with water. Ksp = 4.0 x 10-11 a) water b) 0.25 M NaF
[References] CHEMWORK The Ksp for SrSO4(s) is 3.2x10-7. Calculate the solubility of SrSO4(s). Ignore any potential reaction of the ions with water. Solubility for SrSO4(s) = mol/L Sun
Calculate the molar solubility of CaF2 in a solution containing 0.871 M of Ca(NO3)2. The Ksp value for CaF2 is 1.46×10−10. Express the molar solubility to three significant figures and include the appropriate units. S =
Calculate the molar solubility of CaF2 in a solution containing 0.357 M of Ca(NO3)2. The Ksp value for CaF2 is 1.46×10−10. Express the molar solubility to three significant figures and include the appropriate units.
Assuming that the solubility of PbBr2(s) is 2.1x10 mol/L at 25°C, calculate the Ksp for this salt. Ignore any potential reactions of the ions with water.
Calculate the molar solubility of CaF2 in a solution containing 0.647 M of Ca(NO3)2. The Ksp value for CaF2 is 1.46×10−10. Express the molar solubility to three significant figures and include the appropriate units.
Calculate the molar solubility of CaF2 in a solution containing 0.325 M of Ca(NO3)2. The Ksp value for CaF2 is 1.46×10−10. can you also explain me how to solve for X toward the end of the problem
Assuming that the solubility of PbCl2(s) is 1.6x10-2 mol/L at 25°C, calculate the Ksp for this salt. Ignore any potential reactions of the ions with water. Ksp = _______ The solubility of Pb(IO3)2(s) in a 2.00x10-2 M KIO3 solution is 7.7x10-8 mol/L. Calculate the Ksp value for Pb(IO3)2(s). Ksp = _______
Consider the dissolution of CaF2 in aqueous solution: CaF2 (s) ⇌ Ca(+2) (aq) + 2F(-) (aq). If we start with 1M of undissolved CaF2 in a solution that already contains 0.015M of F(-) ions, what is the solubility of CaF2 at 298.15K in terms of molarity? (Hint: Look at the final simulated concentration of Ca(+2).) A. 3.7E-7 M B. 2.5E-6 M C. 1.2E-5 M