The solubility of Ag2CrO4 (Ksp = 1.2 x 10-12) is several times greater than that of AgCl (Ksp = 1.82 x 10-10), so the red precipitate cannot form until all the chloride ions have effectively been removed from the solution. If a student uses 1 mg of K2CrO4 Aas an indicator for 100 mL of sample solution, what is the concnetrion of chloride ion in the solution when the red precipitate (Ag2CrO4) starts to form?

Q: Complete the following solubility constant expression for SrCO 3.

A: SrCO3 ionises as : SrCO3 ----------> Sr2+ + CO32- Solubility product Ksp = [Sr2+][CO32-] Let the…

Q: If 18.0 mL of 9.22x10-4 M Ca(CH3COO)2 are added to 18.0 mL of 7.80x10-5 M (NH4)2SO4, will solid…

A: Answer: For the precipitation of sparingly soluble salt to begin its ionic product should be equal…

Q: A 45.0 mL sample of 0.015 M calcium chloride, CaCl2, is added to 55 mL of 0.010 M sodium sulfate,…

A: Given : Concentration of CaCl2 = 0.015 M Volume of CaCl2 solution = 45.0 mL = 0.045 L…

Q: Determine the molar solubility of Cu(IO4)2 in 0.20 M NaIO4? ((Ksp of Cu(IO4)2 = 1.4 x 10−7) (a)…

A:

Q: The concentrations of Ag*(aqg) and Pb2*(aq) are both 0.050 M in a particular solution. A NaCl…

A: [Ag+] = 2.309x10-9

Q: Will a precipitate form when 25 mL of 0.20M Ba(NO3)2 is mixed with 15 mL of 0.20M NaOH? (Ksp Ba(OH)2…

A:

Q: A 750 mL solution contains o.350 M K2Cro4, and a.350 M Na2SO4. A concentrated Ba(NO3)2 is slowly…

A: Ksp : At normal temperature, if the solubility of a salt is 0.1mol / Lit then that salt is called…

Q: 135.0mL of 0.500M Al(NO3)3 is reacted with 50.0mL of 5.65M CuCO3 as shown below. What is the maximum…

A: Answer:- This question is answered by using the simple concept of stoichiometry which involves the…

Q: Will a B(OH)₃ precipitate form if 150.0 mL of 0.002 M BX₃ is mixed with 250.0 mL of pH 0 Ba(OH)₂…

A: Ksp of B(OH)3 = 1.9 × 10-13 Molarity of BX3 = 0.002 M Volume of BX3 = 150 mL or 0.15 L BX3…

Q: 1.) A solution is prepared by mixing together 75.00 mL of 0.150 M Pb(NO3)₂ and 50.00 mL of 0.925 M…

A:

Q: A solution contains 5.21x10-3 M potassium carbonate and 1.05x10-2 M ammonium sulfide. Solid…

A: Using solubility product expression and comparing the solubility constant values, concentration of…

Q: f 27.5 mL of 1.63x10-9M of FeCl3 is added to 98.6mL of 2.58x10-9 M NaOH, will a precipitate of…

A: The question is based on the concept of solubility product principle. it  states that a weak…

Q: If 0.15 M NaOH is slowly poured into a beaker containing 0.14 MCa(NO3)2 and. 0.25 M Fe(NO3)2, which…

A: Given,Concentration of NaOH solution = 0.15 MConcentration of CaNO32 solution = 0.14…

Q: 9. If 50.0 mL of a 0.0010 M CaCl₂ solution were added to 50.0 mL of 0.010 M Na₂SO4 solution, would a…

A: 9.) Answer:

Q: What is the solubility (g L-1) of lead(II) Iodide in otherwise pure water, given that the solubility…

A:

Q: When 22.0 mL of a 1.02 × 10-4 M potassium hydroxide solution is combined with 22.0 mL of a 7.55 ×…

A: To determine whether a precipitate will form when 22.0mL of  1.02×10−4 M potassium hydroxide…

Q: If 18.0 mL of 6.09×104 M Pb(NO3)2 are added to 25.0 mL of 9.30×105 M NH Br, will solid PbBr2 (Ksp =…

A: We know if the Ionic product is more than solubility product then precipitate forms.If ionic product…

Q: If a solution contains 0.0020 mol CrO2 of per liter, what concentration of Ag ion must be reached by…

A: The dissociation of solid Ag2CrO4 isThe solubility product Ksp expression is

Q: At what pH will Fe(OH)3(s) begin to precipitate from 2.25 × 10-³ M FeCl3? Ksp for Fe(OH)3 is 2.79 ×…

A: Answer: Fe(OH)3 is a sparingly soluble compound and for a sparingly soluble compound, at the…

Q: Excess solid Na₂CO₃ is added to a solution containing 0.300 M (each) Mg²⁺ and Zn²⁺ ions. Ksp for…

A: The solubility of a compound describes the dissolution of the compound in the solvent. In…

Q: Solid Na2SO4 is added slowly to a solution that is 0.38M in Pb(NO3)2 and 0.58M in Ba (NO3)2. In what…

A: Each of Pb(NO3)2, and Ba(NO3)2 is completely soluble in water and respectively produces  1 Pb2+(aq),…

Q: What is the molar solubility of nickel(II) sulfide in 0.091 M KCN? For NiS, Ksp= 3.0 x 10-19 For…

A: Given, Ksp for NiS = 3.0 × 10-19 Kf for Ni(CN)42- = 1.0 × 1031 Concentration of KCN = 0.091 M

Q: A solution is 0.013 M Fe3+ and is in a buffer solution that is 0.150 M CH3COOH and 0.250 M NaCH3COO.…

A: For precipitation Ionic product of salt must be greater than its Ksp (solubility product) value.

Q: A solution contains 1.03x10-² M lead nitrate and 1.06x10-2 M aluminum acetate. Solid ammonium…

A: Using solubility product constant values, concentration of lead ion can be calculated.

Q: How might you separate a precipitate containing the following mixture: Q2 BaF2(s) + AgCl (s) .…

A: Agcl is solunle In Liq NH3 solution. It forms a complex.and with adding conc nitric acid the ppt…

Q: The solubility product of Ag2CrO4 is 32x10-12. What is the concentration of CrO4 ions in that…

A: Ag2CrO4  ⇌ 2 Ag+ +CrO4-2 solubility product (Ksp) =[Ag+]2 ×[CrO4-2 ]where[Ag+] = concentration of…

Q: 1a) Does a precipitate form when you add 55.5 g of NaCl to 250.0 mL of 0.35 M Pb(NO3)2? (Ksp for…

A: In this case determine ionic product or Qsp and If Qsp < Ksp then precipitate is formed otherwise…

Q: What is the concentration of Fe²+ in a saturated solution of Fe(OH)₂ if its solubility is 1.59x10-5…

A: Answer:- This question is answered by using the simple concept of calculation of concentration using…

Q: Lead (II) fluoride has a Ksp value of 2.7x10-8. What is the concentration of Pb2+ and F- ions in a…

A: The solubility product constant (Ksp) describes the equilibrium between a solid and its constituent…

Q: come first Calculate the percentage

A:

Q: Excess solid Na₂CO₃ is added to a solution containing 0.650 M (each) Mg²⁺ and Zn²⁺ ions. Ksp for…

A:

Q: An aqueous solution contains Cu+, Tl+, Hg+, and Ti+ with each ion at a concentration of 0.15M.…

A: Given: The solubility of compounds given as AgCl = 1.8 x 10−10TiCl = 1.8 x 10−4PbCl2 = 1.7 x…

Q: ₃ precipitate form if 150.0 mL of 0.002 M BX₃ is mixed with 250.0 mL of pH 9.0 Ba(OH)₂ solution at…

A: The concentration of B+3 from BX3=0.002MAfter mixing total volume of solution =250mL+150mL400mLThe…

Q: What is the maximum concentration of sodium carbonate (Na2CO3) that will dissolve in 1.0x10-5 M…

A:

Q: A 20.0-mL sample of 0.00200 M AgNO3 is added to 20.0 mL of 0.0100 M NalO3. What is the equilibrium…

A: Answer:When solutions of 2 different substances are mixed and formation of precipitate takes place…

Q: Will a precipitate form when 100.0 mL of 7.2 x 10-4 M Mg(NO3)₂ is added to 100.0 mL of 1.0 × 10¯…

A: Answer:For a sparingly soluble compound, when ionic product Q becomes greater than KSP that's when…

Q: The solubility-product constant for barium permanganate, Ba(MnO4)2, is 2.5 * 10-10. Assume that…

A: Given, Ksp=2.5×10-10 [Ba2+][MnO4-]2=2.5×10-10[Ba2+]=2.0×10-8

Q: A 25.0-mL sample of 0.00200 M AgNO3 is added to 25.0 mL of 0.0100 M NaIO3. What is the + equilibrium…

A: The balanced net ionic reaction is:

Q: A 3.90-L solution of 1.80x10^-3 M Pb(NO3)2 is mixed with a 0.60-L solution of 0.76 M NaCL. Calculate…

A:

Q: A solution contains 5.21x103 M potassium carbonate and 1.05x10-2 M ammonium sulfide. Solid…

A:

Q: Predict wether a precipitate will form upon mixing 75.0 mL of NaOH solution with pOH of 2.58 with…

A: Given that pOH = 2.58 Concentration of OH– = 10–pOH = 10–2.58 = 0.00263 M

Q: Solid Na, SO4 is added slowly to a solution that is 0.76M in Pb(NO3), and 0.55M Ba (NO3)2. In what…

A: