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- What compound, if any, will precipitate if when 50 ml of 1.0x10─5 M Sr(OH)2 is added to 75 ml of 1.0x10─5 M CuSO4? Ksp SrSO4 = 3.2x10─7 , Ksp Cu(OH)2 = 2.2x10─20 What are the final concentrations of Cu2+(aq) and Sr2+(aq) in the solution? Zinc ion reacts with excess CN─ to form a colorless complex ion, Zn(CN)4─2, which has a formation constant Kf = 4.2x1019. Calculate the concentration of Zn2+ in a solution prepared by mixing equal volumes of 5.0x10─3 M Zn(NO3)2 and 0.10 M NaCN. [Ignore the hydrolysis of CN─(aq).] Calculate the molar solubility of Al(OH)3 in 0.30 M NaOH; Kf for Al(OH)4─ = 3x1033 and Ksp for Al(OH)3 = 3.0x10─34We began the chapter with an informal discussion of how the mineral fluorite (as shown) is formed. Fluorite, CaF2, is a slightly soluble solid that dissolves according to the equation: CaF2(s) ⇌ Ca2+(aq) + 2F−(aq)The concentration of Ca2+ in a saturated solution of CaF2 is 2.15 × 10–4 M; therefore, that of F– is 4.30 × 10–4 M, that is, twice the concentration of Ca2+. What is the solubility product of fluorite?If a sample of silver coin weighing 0.5230 g gives a precipitate of AgCl (143.45) weighing 0.3559 g, the weight of AgBr (187.90) that could have been obtained from the same weight of sample is 0.89 grams. true or false?
- Sufficient sodium cyanide, NaCN, was added to 2.5x10^-2 M silver nitrate, AgNO3, to give a solution that was initially 0.193 M of a cyanide ion, CN-. What is the concentration of silver ion, Ag+, in this solution after Ag(CN)2- forms? The formation Kfconstant for the complex ion Ag(CN)2- is 5.6x10^18. Concentration = MGive the chemical equation for the dissociation of Mg3(PO4)2? b.) What is the molar solubility of Mg3(PO4)2? c.)What are the equilibrium concentration of the ions?A solution contains 0.04500.0450 M Ca2+ and 0.09500.0950 M Ag+. If solid Na3PO4 is added to this mixture, which of the phosphate species would precipitate out of solution first? -Ca3(PO4)2 -Ag3PO4 -Na3PO4 When the second cation just starts to precipitate, what percentage of the first cation remains in solution?
- For the aqueous [Cu(NH3)4 ] 2+ complex kf =5.6 x1011 at25°C .Suppose equal volumes of 0.0062M Cu(NO3)2 solution and 0.88M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Cu2+ ion.Round your answer to 2 significant digits.A similar experiment as this lab is done as following: 0.456 g of solid AgCl is added a 25 mL solution of a 1.05 M ligand L to form complex AgL+. AgCl (s) + L (aq) → AgL+ (aq) + Cl- (aq) When the reaction is complete, 0.315 g of solid AgCl remains. Assume the total volume of the resultant solution is the same as the volume of the ligand solution. Ksp of AgCl in water is 1.83 x 10-10. 3.What is the equilibrium concentration of [L]eq? Group of answer choices A, 2.01 mol/L B,2.45 mol/L C, 1.01 mol/L D, 0.405 mol/LSilver and ammonia may react to form Ag(NH₃)₂⁺ complex (Kf = 1.66 x 107). A 500 mL of 10 mol Ag⁺ and 500 mL of 0.70 mol NH₃ are mixed together. Write the complexation reaction. Write the formation constant expression. What is the concentration of the complex at equilibrium? What is the concentration of the metal at equilibrium?
- For the aqueOuS [Ni(NH3)6] 2+ complex Kf= 5.50 x 10^8 at 25 °C. Suppose equal volumes of 0.0016 M Ni(NO3)2 solution and 0.28 M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ni2+ ion. Round your answer to 2 significant digits.A similar experiment as this lab is done as following: 0.456 g of solid AgCl is added a 25 mL solution of a 1.05 M ligand L to form complex AgL+. AgCl (s) + L (aq) → AgL+ (aq) + Cl- (aq) When the reaction is complete, 0.315 g of solid AgCl remains. Assume the total volume of the resultant solution is the same as the volume of the ligand solution. Ksp of AgCl in water is 1.83 x 10-10. 2. What are the equilibrium concentrations of [AgL+]eq and [Cl-]eq? Group of answer choices A, 0.0394 mol/L B, 12.5 mol/L C, 0.0154 mol/L D, 0.394 mol/LChromium(III) hydroxide, Cr(OH)3, is highly water insoluble. Its molar mass is 103.02 g/mol. a.) Write the chemical equation for dissolving Cr(OH)3 in water. b.) Calculate the mass solubility of Cr(OH)3 in pure water. c.) Calculate the mass solubility of Cr(OH)3 in a solution containing 0.221 M Cr(NO3)3(aq). d.) Calculate the mass solubility of Cr(OH)3 in 0.350 MM NaOH(aq).