SPECTROPHOTOMETRIC DETERMINATION OF A SOLUBILITY PRODUCT CONSTANT A) Write the Equation for the dissolving of solid AgCrO4 in water and the Ksp expression for equilibrium.  B) Calculate the molar solubility of BaCrO4. Ksp = 2.1 X 10^-10. Show the equilibrium setup and the calculation.  C) Calculate the molar solubility of BaCrO4 in the presence of 0.020 M Na2CrO4. Show the equilibrium setup and calculation.

Q: Two chromate salts, barium chromate (BaCrO4) and silver chromate (Ag2CrO4) are considered for…

A: Solubility is the ability of a substance to dissolve.   Solubility product constant(Ksp) is the…

Q: When 22.0 mL of a 6.20 x 10-4 M aluminum chloride solution is combined with 22.0 mL of a 9.73 x 10-4…

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Q: The Ksp for CaF2 is 3.9 * 10-11 at 25 °C. Assuming equilibrium is established between solid and…

A: In order to calculate the solubility we first write down the given data: Ksp= 3.9*10-11. Solubility…

Q: What is the molar concentration of Ag+ when an excess of solid Ag2SO4 is added to 0.1063 M Na2SO4 so…

A: Solubility product It is the equilibrium constant for a sparingly soluble salts.  Solubility product…

Q: of lead(II) carbonate, PBCO3, is 7.40 × 10-14. Calculate the molar solubility, S, of this compoun…

A: Ksp of PbCO3 = 7.40*10-14   Then,

Q: Equal volumes of a 5.28 x 10-4 M nickel (II) nitrate solution and a 3.18 x 10-3 M sodium carbonate…

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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: A 50.0 mL of 0.250 M Ca(NO3)2 solution is added to 100.0 mL of 0.150 M NaF solution and as a results…

A: The objective of this question is to determine molar solubility and equilibrium concentrations in a…

Q: When 15.0 mL of a 3.96 x 10-4 M potassium sulfate solution is combined with 22.0 mL of a 7.85 x 10-4…

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Q: Write out the correspoding solubility equilibrium equations that would give rise to a chromate…

A: Precipitate are the insoluble solids which are obtained from a solution when there is a reaction…

Q: Calculate the solubility of AgBr in 225 mL of water to which 0.15 g of NaBr has been added. AgBr(s)…

A: Since we have NaBr in solution which has a common Br ion with AgBr hence the concentration of Br-…

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: The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20.  Suppose a chemist mixed 33.23 mg…

A: 3Mg2+ + 2 AsO43-  ------> [Mg3(AsO4)2] Ksp = 2.00 X 10-20 Mg2+(aq)  = 33.23 mg =  33.23  * 10-3 g…

Q: indicate final answer) a. b. C. d. e. f. 9- h. Moles of HCI added (mol) Moles of OH- in saturated…

A: Saturated Ca(OH)2 solution is sparingly soluble in water and is in equilibrium with Ca2+ and OH- as…

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: Oxalic acid forms a precipitate with calcium ion Ca2+ (aq) + C2H204(ag) + H20(1) -> CaC2O4*H20 (s)…

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Q: Determine the value of Ksp for Mg(CN)2 by constructing an ICE table, writing the solubility constant…

A: Answer: Mg(CN)2 is a sparingly soluble salt, therefore it is considered that all its dissolved…

Q: A student is calculating the concentration of her standard solutions in order to create the…

A: Given: Volume of Fe3+ = 2.00 mL Concentration of Fe3+ = 0.183 M Volume of SCN- = 225 μL = 0.225 mL…

Q: Calcium fluoride has a Ksp of 3.2 x 10-11. Would you expect to see a precipitate if you mix 0.100 L…

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Q: In a saturated solution of MgF2 at 18°C, the conctration of Mg2+ is 1.21*10^-3 molar.  a)Write the…

A: (a) The equilibrium equation for saturated solution of MgF2 is represented as follows, The…

Q: a) A saturated solution of barium fluoride, BaF2, was prepared by dissolving solid BaF2 in water.…

A:

Q: Use the reaction quotient to predict whether a precipitate will form. If 15.0 mL of 3.74×104 M Cal2…

A: The objective of the question is to predict whether the precipitate will occur or not.

Q: Lead thiocyanate, Pb(SCN)2. has a Kap value of 2.00 × 10 5. Pa Call Exp

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Q: A 50.0 mL aqueous solution of an NH3/NH4Cl buffer has a pH of 9.12. If 1.3 x 10–3 g of Fe(NO3)3 is…

A: Since the pH is 9.12  Hence pH = 14 + log[OH-] = 9.12  => [OH-] = concentration of OH- ions in…

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: Ksp for Agl = 1.2 x 10-17. Calculate the molar solubility of Agl in 1 x 104 molar AgNO3 solution.…

A: AgI⇌Ag+  + I-  let ,intial concentration of Ag+=x , I- =xIn AgNO3 solutionAgNO3⇌Ag+  +NO3- 10-4 M…

Q: The Ksp of PbSO4 is 1.82 x 10-8 at 25 °C. What concentration of Pb(NO3)2(aq) is required to…

A: Answer: Sparingly soluble salt begins to get precipitated when its solubility product becomes equal…

Q: Consider the following mixtures of chemicals. Complete the table by writing balanced equations and…

A: The equation will be:

Q: The Solubility Product Constant for iron(III) hydroxide is 6.3 × 10-38. Solid sodium hydroxide is…

A: Step 1: Step 2: Step 3: Step 4:

Q: The Solubility Product Constant for cobalt(II) sulfide is 5.9 × 10-²¹. The molar solubility of…

A:

Q: When 12.0 mL of a 3.44 x 10-4 M ammonium sulfide solution is combined with 15.0 mL of a 6.15 x 10-4…

A: We will calculate Q first , then compare with K.

Q: When 25.0 mL of a 6.89 × 10-4 M potassium sulfide solution is combined with 18.0 mL of a 3.42 x 10-4…

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Q: What is the molar solubility of silver chloride in 0.65 M NH3(aq)? Solubility

A: “Since you have asked multiple question, we will solve the first question for you. If youwant any…

Q: You are trying to separate calcium ions (Ca2+) from lead ions (Pb2+), both present in a mixture and…

A: From the given salt of sulfate, PbSO4 will precipitate first because of the lower solubility which…

Q: The Ksp value for calcium sulfate [CaSO4] is 2.40 X 10-5 and a professor made 1825 mL of a CaSO4(2g)…

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Q: You prepare a solution by mixing 400.0 mL of 1 x 10-4 M Mg(NO3)2  and 500.0 mL of 1.00 x 10-4 M NaF.…

A: Solubility product for MgF2 can be writte as Ksp =Mg2+F-2 Now, to determine weather precipitate…

Q: What is the solubility product constant (Ksp) expression for the dissolution of CaCl2​?   below are…

A: Given We know about the solubility What is the solubility product constant (Ksp) expression for the…

Q: A 100-mL sulfide-containing water sample was titrated with 12.15 mL of 0.041 M AgNO3 to determine…

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Q: Ksp for Ca(OH)2 is 1.3 x 10-6.  A solution has a concentration of 0.0020 M Ca2+ and 0.0040 M OH-.…

A: The solubility product constant for Ca(OH)2 is = 1.3 x 10-6 The concentration of calcium ion is =…

Q: Nickel iodate, Ni(IO3)2 is being precipitated out of a 1.00 L solution.  If the concentration of…

A: Given,  Volume of Ni(IO3)2 solution in L = 1.00 L  Concentration of Ni2+ = [Ni2+] = 0.381 M…

Q: Part A: A saturated solution of barium fluoride, BaF2, was prepared by dissolving solid BaF2 in…

A:

Q: Determine the concentrations of each zinc-containing species in a solution saturated with solid…

A: Given, (OH)- = 6.1 x 10-7 M ksp Zn(OH)2 = 3 x 10-16  β1 Zn(OH)+= 2.5 x 104 β3 Zn(OH)3- = 7.2 x 1015…

Q: a Calculate the molar solubility of silver thiocyanate, AgSCN, in pure water ( Ksp 1.0 × 10-¹2).…

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Q: A saturated solution of Mg(OH)2 at 25°C is prepared by equilibrating solid Mg(OH)2 with water.…

A: Given-Solutions of Mg(OH)2  Solution of conc. NaOHKsp ( Mg(OH)2 ) = 1.2 × 10-11 To find- The…

Q: Calculate the solubility of zinc (II) hydroxide in a solution maintained at (i) pH= 5.3 (ii) pH=…

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Q: CO₂ is bubbled into a 1.0 L solution containing 0.100 M each of Mg(NO3)2 and Sr(NO3)2. Assume that…

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