At some other temperature, a solid sample of Ca(OH)2 is shaken with 0.0100 M CaCl₂. Once equilibrated, some solid Ca(OH)₂ remains undissolved. The solution is filtered and a 20.00 mL sample requires 39.04 mL of 0.0100 M HCI to neutralize it. Calculate the value for Ksp of Ca(OH)₂ from this data. Ksp =

Lead(II) nitrate is added slowly to a solution that is 0.0100 M in Cl− ions. Calculate the concentration of Pb2+ ions (in mol / L) required to initiate the precipitation of PbCl2. (Ksp for PbCl2 is 2.40 × 10−4.)

What is the molar solubility of Fe(OH)3 in a solution buffered at pH = 4.29? See the Solubility Product Constant Table. 4.0 8.1e-9 What is the molar solubility at pH = 9.00? 4.0 6.00-23 X M Substance Ksp at 25 °C Aluminum Al(OH)3 1.9 x 10-33 Barium Ba(OH)2 BaCO3 BaSO4 XM 5.0 x 10-3 8.1 x 10-9 1.1 x 10-10 Ba3(PO4)2 3.4 x 10-23 Cadmium Cd(OH)2 CdCO3 CdS Calcium 2.5 x 10-14 5.2 x 10-12 8.0 x 10-27 Ca(OH)2 5.5 x 10-6 CaCO3 4.8 x 10-⁹ Ca3(PO4)2 1.0 x 10-26 CaF2 3.9 x 10-11 Chromium CO(OH)2 COS Cr(OH)3 6.3 x 10-31 Cobalt 1.6 × 10-15 4.0 x 10-21 Copper Cu(OH)2 Cu₂S CUCO3 CuS Iron Fe(OH)2 FeS Fe(OH)3 FePO4 Lead Pb(OH)2 PbF2 PbCl₂ PbBr₂ Pbl2 PbCrO4 PbSO4 PbS 2.2 x 10-20 1.6 x 10-48 1.4 x 10-10 6.3 x 10-36 Mg(OH)2 8.0 x 10-16 6.3 x 10-18 2.5 x 10-39 9.9 x 10-29 2.8 x 10-16 3.7 x 10-8 1.7 x 10-5 6.3 x 10-6 6.5 x 10-⁹ 1.8 x 10-14 1.7 x 10-8 8.4 x 10-28 Magnesium 1.8 × 10-11 Manganese Mn(OH)2 MnCO3 MnS Nickel Ni(OH)2 Silver AgCl AgBr Agl AgCN Ag₂S Ag₂ CrO4 Ag3PO4 Tin Sn(OH)2 SnS Zinc ZnCO3 Zn(OH)2…

The pH of a saturated solution of iron(II) hydroxide, Fe(OH)2, was found to be 9.07. From this, find Ksp for iron(II) hydroxide. K sp

Calculate the solubility at 25 °C of Ni(OH)2 in pure water and in a 0.0170M NaOH solution. You'll find K sp Round both of your answers to 2 significant digits. solubility in pure water: solubility in 0.0170 M NaOH solution: 0- 00 x10 X ☐☐ 5 010 data in the ALEKS Data tab.

you are given a 1.00 ml solution of 0.100 m Cl- and told to verify the chloride concentration by gravimetric analysis. 1.00 ml of 0.500 m ag+ is added to this solution and the resultant AgCl quantitatively precipitated. based on the ksp expression, calculate the concentration of the cl- that remains in solution.

By controlling the pH of an aqueous solution it is possible to control the formation of a precipitate (thesolid form) for a slightly soluble ionic compounds. As an example, consider an aqueous solution with[Zn2+] = 2.3 x 10^-4 M. Note that the solubility product for zinc hydroxide (Zn(OH)2) is Ksp = 4.1 x 10^-17.a) At what value for pH will Zn(OH)2 solid first form?b) What percent of the initial concentration of Zn2+ ion will have formed solid at pH = 9.00?

The solubility product, Ksp, for Fe(OH)3 is 1.6 × 10–39. What is the solubility of Fe(OH)3 in a buffer solution with pH = 10, in moles per litre?   A) 1.1 × 10–9 mol.L–1  B) 4.0 × 10–23 mol.L–1 C) 8.8 × 10–11 mol.L–1 D) 1.6 × 10–27 mol.L–1

Potassium hydroxide is used to precipitate each of the cations from their respective solution. Determine the minimum concentration of KOHKOH required for precipitation to begin in each case. 1. 0.010 MM CaCl2CaCl2 (Ksp=4.68×10−6Ksp=4.68×10−6 for Ca(OH)2Ca(OH)2) 2. 0.0020 MM Fe(NO3)2Fe(NO3)2 (Ksp=4.87×10−17Ksp=4.87×10−17 for Fe(OH)2Fe(OH)2) 3. 0.0016 MM MgBr2MgBr2 (Ksp=2.06×10−13Ksp=2.06×10−13 for Mg(OH)2Mg(OH)2)

What is the maximum possible concentration of Ba2+ ions in a NaOH solution if the concentration of OH– is maintained at 0.100 M? The solubility product constant of Ba(OH)2 is Ksp = 5.0 × 10–3