Given the data below, which pair of compounds are the first to precipitate when hydroxide, OH-, is slowly added?. Salt Fe(OH)2 Mg(OH)2 Mn(OH)2 Zn(OH)2 Fe(OH)2 & Zn(OH)2 Mg(OH)2 & Fe(OH)2 Mn(OH)2 & Fe(OH)2 Mn(OH)₂ & Zn(OH)2 Ksp 1.6 x 10-14 -11 1.2 x 10-1 2.0 x 10-13 4.5 x 10-17
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- . Chromiurn(III) hydroxide dissolves in water only to the extent of 8.21105M at 25 °C. Calculate Kspfor Cr(OH)3at this temperature.Chrome yellow, PbCrO4, is the yellow pigment used in road markings.At 15 °C, the solubility product of PbCrO4 is 1.69 × 10-14 mol2dm-6.(a) Write an expression for the solubility product of PbCrO4. [1](b) Calculate the solubility of PbCrO4 [3](c) On adding concentrated aqueous lead(II) nitrate dropwise to 0.010 mol dm-3 potassiumchromate (VI), what is the concentration of lead(II) ions when the first trace ofprecipitate appears? [3]The solubility of CaCO3 in water is about 7 mg L-1 . Show how one can calculate the solubility product of BaCO3 from this information and from the fact that when sodium carbonate solution is added slowly to a solution containing equimolar concentrations of Ca2+ and Ba2+, no CaCO3 is formed until about 90% of the Ba2+ has been precipitated as BaCO3.
- Sodium sulfate is slowly added to a solution containing 0.0500 M Ca2+(aq) and 0.0260 M Ag+(aq). What will be the concentration of Ca2+(aq) when Ag2SO4(s) begins to precipitate? Solubility-product constants, ?sp, can be found in the chempendix. [Ca2+]= M What percentage of the Ca2+(aq) can be precipitated from the Ag+(aq) by selective precipitation? percentage:(a) If the molar solubility of Tl2S at 25 oC is 5.31e-08 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = (c) The Ksp of BaCO3 at 25 oC is 2.58e-09. What is the molar solubility of BaCO3? solubility = ____ mol/LThe solubility products for a series of hydroxides areBiOOH Ksp = 4.0 X 10-10 = [BiO+] [OH-]Be(OH)2 Ksp = 7.0 X 10-22Tm(OH)3 Ksp = 3.0 X 10-24Hf(OH)4 Ksp = 4.0 X 10-26Which hydroxide has the lowest molar solubility in a solution that is 0.10 M in NaOH?
- (a) If the molar solubility of Cu3(PO4)2 at 25 oC is 1.67e-08 mol/L, what is the Ksp at this temperature?Ksp = _______(b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = _______(c) The Ksp of ScF3 at 25 oC is 5.81e-24. What is the molar solubility of ScF3?solubility = ______ mol/LThe weak base Mg(OH)2 is weak because it is only partially soluble in water at 25 °C (Ksp = 1.8×10−11). a. 0.1 M MgCO3 b. 0.1 M Mg3(PO4)2 c. 0.1 M Mg(NO3)2 d. Pure water From the solubility product equilibrium reaction for Mg(OH)2, which mixture would have the least amount of Mg(OH)2 (s) dissolved? Explain by using Le Châtelier’s principle.1. At a certain temperature* (probably not 25 ºC), the solubility of silver sulfate, Ag2SO4, is 0.023 mol/L. Calculate its solubility product constant for this temperature. SIG. FIG. (required because number is small)*Solubility product constants are very temperature sensitive. They are generally reported at 25 ºC. Not necessarily using this temperature allows me some flexibility. 2. At a certain temperature, the solubility of potassium iodate, KIO3, is 61.7 g/L. Calculate its solubility product constant for this temperature. 3. At a certain temperature, the solubility of cadmium fluoride, CdF2, is 0.144 mol/L. Calculate its solubility product constant for this temperature.
- At 15 °C, the solubility product of PbCrO4 is 1.69 × 10-14 mol2dm-6. (a) Write an expression for the solubility product of PbCrO4.(b) Calculate the solubility of PbCrO4.(c) On adding concentrated aqueous lead(II) nitrate dropwise to 0.010 moldm-3 potassium chromate (VI), what is the concentration of lead(II) ions when the first trace of precipitate appears?At 25°C, 34.9 mg of Ag2CO3 will dissolve in 1.0 L of pure water: Ag2CO3(s) 2 Ag+(aq) + CO32-(aq) What is the solubility product constant, Ksp for this salt?Given: Solubility product for a series of hydroxides: BiOOH Ksp = 4.0 x 10-10 = [BiO+][OH-] Be(OH)2 Ksp = 7.0 x 10-22 Tm(OH)3 Ksp = 3.0 x 10-24 (a) Which hydroxide has the lowest molar solubility in water? (b) Which hydroxide has the highest molar solubility in a 0.10 M NaOH solution?