2.1 Estimate the solubility of calcium carbonate at 25°C in the presence of 0.02M CaCl2(aq) (6) 2.2 Will BaSO4 precipitate from a solution containing 2.5 x10 M Ba*2, barium ion, if enough soluble salt, Na2SO4, is added to make the solution 2.5 x104 M in SO42? (6)

(Q49) The molar solubility of bismuth iodide (Bil3) at 35°C is 6.54 x 10-5 M. What is the value of Ksp at this temperature? The balanced chemical equation for the dissociation of bismuth iodide is: Bil3 (s) Bi3+ (ag) + 3 |- (aq). O 7.71 x 10-19 4.28 x 10-9 O 1.83 x 10-17 O 5.49 x 10-17 4.94 x 10-16

At a particular temperature, the solubility of In₂(SO₄)₃ in water is 0.0060 M.   (a) What is the value of Ksp? (b) 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? (c) If solid In₂(SO₄)₃ is added to a solution that already contains 0.150 M In(NO₃)₃, what will the new solubility of the solid be?

7. The Ksp for copper(I) sulfide, Cu2S(s), is 2.5 x 10-48. Cu2S (s) 2 Cu'(aq) + S²(aq) (a) Write a solubility constant expression for Cu2S(s). [2] (b) Calculate its molar solubility in water at 25 degrees Celsius. [6]

(a) If the molar solubility of Nd₂(CO3)3 at 25 °C is 1.00e-07 mol/L, what is the Ksp at this temperature? Ksp = (b) It is found that 8.90e-06 g of Y₂(CO3)3 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility- product constant for Y₂(CO3)3. Ksp = (c) The Ksp of Ag₂C₂04 at 25 °C is 5.40e-12. What is the molar solubility of Ag2C₂04? solubility mol/L

Q2) Q1) what is the concentration of Sr2* in PPm for the solution in equilibrium with the precipitate of SrSO4 ? PKSP(SrOa) =6.55 PKa( HSO4) 1.92 Mw(Sr)=87.6

(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/L

Consider the mixing of 25.00 mL of 0.0500 M Pb(NO3)2 with 25.00 mL of 0.0500 M NaCl and the equilibrium reaction, PbCl2(s) ⇌ Pb2+(aq) + 2Cl-(aq)   Ksp = 1.20 x 10-5 What is the molar concentration of Pb2+ in the resulting mixture? (0.500, 0.025, 0.0125 or 0.100) What is the molar concentration of Cl- in the resulting mixture? (0.500, 0.025, 0.0125 or 0.100) What is the ion product (Q)?  Will a precipitate form? (yes or no)

(b) The solubility product, Ksp of silver chloride, AgCl is 1.0 x 10-10. What is the solubility of AgCI in g L-1?

a) What is the solubility of copper(II) iodate, Cu(IO;)2? Ksp. = 1.4 x 107 at 25 °C %3D b) Will the solubility of Cu(IO3)2 (s) increase, decrease or remain the same if some solid Cu(NO:)2 is added? (copper(II) nitrate is very soluble and completely dissolves) c) Aqueous copper(II) ions, Cu²* to the reaction: (a0), react with aqueous ammonia to form a complex according Cu2+, (a0+ 4NH3 (a) [Cu(NH3)4]* (aq) with a formation constant, Ke= 1.2 x 1013 How will the addition of aqueous NH3 effect the solubility of Cu(IO3)2 (s)? (increase, decrease or no effect)