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- Magnesium fluoride (MgF2, MW = 62.30 g/mol) is slightly soluble in water, with Ksp = 7.4 x 10^-11 at T= 25. C.a) Give the correctly balanced solubility reaction and expression for Ksp for MgF2.b) What mass of magnesium fluoride will dissolve in 1.000 L of pure water?1. a. When excess solid SrCrO4 is shaken with water at 25°C, it is found that 6 x 10^-3 mol dissolves per liter. Use this information to calculate the solubility product constant for SrCrO4. b. The Ksp of BaF2 is 1.8 x 10-7, what is its water solubility in moles per liter.16.The following is a solubility product expression for Ca3(PO4)2: Ksp= Group of answer choices A, [Ca32+][(PO43–)2] B, [Ca2+][2PO43–] C, [3Ca2+]3[2PO43–]2 D, [Ca3+]2[PO42–]3 E, [Ca2+]3[PO43–]2
- Calculate the solubility (in g/L) of silver chromate in water at 25°C if the Ksp for Ag3PO4 is 1.75 × 10-18. Ag3PO4(s) <==> 3Ag+ (aq) + PO43- (aq); Ksp = 27s4, s = _________ mol/L x MM of Ag3PO4 = _________ g/L.Calcium phosphate (Ca3(PO4)2; MM = 310.18 g/mol) has a Ksp of 2.07 × 10−33 at 25 ℃. Write the reaction equation for the dissolution of Ca3(PO4)2 solid Calculate the solubility in mg/L at 25 ℃ in pure water. Neglect other competing equilibria. Calculate the solubility in mg/L at 25 ℃ in the presence of 0.010 M CaCl2. Neglect other competing equilibria. Assume that 3s << 0.010 M. Is the assumption that s << 0.010 M valid? (Yes or No)At a particular temperature, the solubility of In₂(SO₄)₃ in water is 0.0070 M. You have found Ksp to be 1.8 × 10⁻⁹. If solid In₂(SO₄)₃ is added to a solution that already contains 0.200 M Na₂SO₄, what will the new solubility of the solid be? If solid In₂(SO₄)₃ is added to a solution that already contains 0.150 M ln(NO₃)₃, what will the new solubility of the solid be?
- a solution containing 6.25×10–3 M of S2– and 5.63×10–3 M of Cd2+ was prepared. CdS ⇌ Cd2+ + S2- Calculate the Qsp of the mixture (in 3 sig. figures) and In the given scenario, will a precipitate (Ksp = 3×10–28) form?The Ksp of ZnCO3 (MM: 125.38) is 1.20 xx 10^(-10). a) What is the molar solubility of ZnCO3? b) What is the solubility of ZnCO3 in g/L?The Ksp for CoCO3 = 1.0 × 10–10 and the Ksp for PbCO3 = 7.4 × 10–14. When Na2CO3 is added dropwise to a solution containing 0.010 M Co2+ and 0.010 M Pb2+, which ion will precipitate first? What must the [CO32–] be so that the first ion to precipitate comes out of solution, but the second ion does not?
- What is the Cl- concentration just as Ag2CrO4 begins to precipitate when 1.0 M AgNO3 is slowly added to a solution containing 0.015 M Cl- and 0.015 M I-? Ksp for Ag2CrO4 is 1.2 x 10-12.25). The solubility of BiI3 (dissociates to Bi3+ ions and I– ions) is 0.00778 g/L. What is Ksp for this compound? (a) Calculate the solubility of BiI3 in mol/L. (b) Show the reaction of dissociation of BiI3. (c) Show the Ksp expression for BiI3. (d) Calculate the Ksp for this compound?Consider the dissolution of solid Ca3(PO4)2 in an aqueous solution of 0.2 M Ca(NO3)2. Identify which ONE of the following statements is INCORRECT. a. Ca2+ is the common ion. b. The Ksp expression for calculating the solubility of Ca3(PO4)2 is Ksp = 108s5 c. The value of the Ksp for Ca3(PO4)2 remains unchanged d. After addition of Ca3(PO4)2 the Ca2+ concentration remains constant e. All nitrate anions remain in solution