minimum concentration

Q: Determine the molar solubility of PbSO4 in pure water. Ksp (PbSO4) = 1.82 × 108. a. 1.82 x 10-8 M b.…

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Q: Calculate the molar solubility of Co(OH)3, Ksp = 2.5 x 10-43.

A: Solubility product: In a saturated solution of a sparingly soluble electrolyte, the product of molar…

Q: Should Mg(OH)2(s) precipitate from a solution that is 0.010 M MgCl2 and also 0.10 M NH3?   NH3(aq)…

A: MgCl2 dissociates completely in the solution giving 0.010 M Mg2+ and 0.020 M Cl-1 ions. MgCl2…

Q: Solid Naz SO4 is added slowly to a solution that is 0.33M in Pb(NO3)2 and 0.47M in Ba (NO3)2. In…

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Q: Estimate the solubility of lead(II) iodide in a. moles per liter of pure water. Solubility =…

A: The solubility product, Ksp expression for a salt is the product of the concentrations of the ions,…

Q: Without doing a calculation, predict which of these compounds has the greatest molar solubility in…

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Q: A solution contains 1.48x10-2 M lead acetate and 1.28x10-2 M cobalt(II) nitrate. Solid ammonium…

A: Given: Concentration of Pb(CH3COO)2 = 0.0148 M And concentration of Co(NO3)2 = 0.0128 M

Q: 96 mL of 0.080 M NaF is mixed with 32 mL of 0.20 M Sr(NO3)2. Calculate the concentration of Sr2+ in…

A: Volume = 96 ml of NaF volume = 32 ml of Sr(NO3)2 concentration = 0.080 M NaF concentration = 0.20 M…

Q: A solution contains 1.37x102 M potassium phosphate and 1.21×102 M sodium hydroxide. Solid aluminum…

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Q: A solution is prepared by mixing 50.0 mL of 0.50 M CaCl2 with 50.0 mL of 0.50 M CoCl2. When NaOH is…

A: The concentration of both the metals (Co and Ca) are equal. hence, precipitation of [Co(OH)2]  and…

Q: A solution contains 6.71×10-3 M barium acetate and  1.21×10-2 M calcium nitrate.  Solid potassium…

A: Given information: 6.71×10-3 M barium acetate 1.21×10-2 M calcium nitrate.    KSP for BaF2 is…

Q: Complete the mass balance expression for a saturated solution of Ag,CO3. Ignore any subsequent…

A: Mass balance equation for saturated solution of Ag2CO3

Q: 2. Chromium (III) iodate, Cr(IO3)3, has a solubility product of 5.0 x 10-6. a. Calculate the…

A: a) The reaction will be, CrIO33 ⇔ Cr3+aq + 3IO33-aq The solubility of Cr(IO3)3 is, Ksp = s…

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: calculate the concentration of lead ion in saturated solution of lead chloride dissolve in 0.10 M…

A: Given : Ksp PbCl2 = 1.8×10-4 Concentration of lead chloride dissolve in 0.10 M NaNO3 = ?

Q: A solution contains 0.23 M Pb2+ and 0.45 M Al3+. Calculate the pH range that would allow Al(OH)3 to…

A: Reaction Allow Al(OH)3 to precipitate Al3+(aq)  +  3 O-H(aq)   →    Al(OH)3 (s) Reaction Allow…

Q: What is the molar solubility of nickle sulfide, NiS, in (1.50x10^-1) M ammonia, NH3? Ammonia reacts…

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Q: Argentometric titrations typically use a standard solution of silver ions to form a silver halide…

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Q: Calculate whether a precipitate will form if 1.75 mL of 0.70 M NH3 is added to 2L of 0.85 x 10-3 M…

A: The balanced chemical equation for the formation of zinc (II) hydroxide from ammonia and zinc…

Q: How much lead(II) chloride will precipitate if 185 mL of 0.021  M sodium chloride is added to 235 mL…

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Q: A solution contains 0.24 M Pb2+ and 0.43 M A13+. Calculate the pH range that would allow Al(OH)3 to…

A: Given :  Concentration of Pb+2 = 0.24 M  Concentration of Al+3 = 0.43 M  Ksp of Pb(OH)2 = 1.43 x…

Q: Suppose that we have a solution that is 0.0010 M CI and 0.100 M Cro4 2-. If we add 0.100 M AGNO 3,…

A: Given : [Cl-] = 0.001M [CrO4 ²-] = 0.1M [AgNo3] = 0.1M Ksp of AgCl = 1.6*10-¹⁰ Ksp of Ag2CrO4 =…

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 for silver chromate ( Ag, CrO4) is 9.0 x 10 2. Calculate the solubility of silver chromate…

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Q: In which solution is Fe(CIO4)3 most soluble? 0.400 M NaClO4 Pure water 0.200 M HC1 1.400 M Fe(NO3)3…

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Q: Write the solubility product constant for: A. BaCrO4 B. Ag2CrO4 C. Mg3(PO4)2

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

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Q: Solid NazSO4 is added slowly to a solution that is 0.33M in Pb(NO3)2 and 0.47M in Ba (NO3)2. In what…

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Q: 1. At 25°C calcium fluoride has a solubility product constant Ksp = 3.5 x 10-11. The solubility of…

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Q: The Ksp for AG2SO4 is 1.2x10^-5 and the Ksp for CaSO4 is 4.93x10^-5. How do I find the Ca…

A: Selective precipitation of ions from a solution.Ksp is the solubility product constant which defines…

Q: 4.) A solution contains 7.84 x 10 8 M of copper ion (Cu2*) and has a pH of 9.118. Does copper(II)…

A: Given that:  [Cu2+] = 7.84×10-8M pH = 9.118  Ksp of Cu(OH)2 = 1.10×10-15 Using: pH + pOH = 14 pOH =…

Q: A solution of NaF is added dropwise to a solution that is 0.0144 M in Ba+2 ions.  At what F-…

A: The solubility reaction of BaF2 is  => BaF2 (s) -------> Ba2+ (aq) + 2 F- (aq)  Hence the…

Q: . The Ksp for copper (II) hydroxide is 1.6 x 10-19; calculate the molar solubility and concentration…

A: In this question, we want to determine the Concentration of Cu2+ ion and molar solubility of its…

Q: What is the maximum pH that a 250-mL of 0.025 M CaSO4 solution can attain without precipitating…

A: The solubility product is defined as the product of concentration of ions and each ions is raised by…

Q: A solution is 0.050 M Pb +2. What minimum concentration ( in M) of Cl- is required to begin to…

A: All known compounds can be dissolve in certain solvents whereas they remain insoluble in other…

Q: Determine the molar solubility of Fe(OH)2 in pure water. Ksp for Fe(OH)2 =4.87 x 10^18 a. 4.87 x…

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Q: For manganese(II) hydroxide, Mn(OH)2, Ksp = 1.6 * 10-13. Calculate the molar solubility of Mn(OH)2…

A: Given: Ksp=1.6×10-13 Concentration of NaOH= 0.020M To find: Molar solubility of Mn(OH)2

Q: A solution of HCl is slowly added to a 1.0 L solution that contains 0.00030 M AGNO3 and 0.010 M…

A: Initial concentration of Ag+(aq), [Ag+(aq)] = 0.00030 M Initial concentration of Pb2+(aq),…

Q: Sodium carbonate, Na2CO3, is added dropwise to a solution that contains 1.0 X 10-2 M Ag+ and 5.0 X…

A: NOTE : I assume that in question  5.0 X 10-2 M Cd2+ has been typed incorrectly instead of  5.0 X…

Q: ou are tasked with determining a way to identify the following ions in solution: Na+, Ni2+, Ag+, and…

A: The separations of the givens are as follows:

Q: A solution contains 9.47x10^-3 M nickel (II) acetate and 1.27x10^-2 M zinc nitrate. Solid potassium…

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Q: A solution contains 1.46x102 M silver acetate and 1.43x102 M calcium nitrate. Solid sodium sulfite…

A: Given: Concentration of silver acetate i.e. AgCH3COO = 1.46 × 10-2 M. And concentration of calcium…

Q: Calculate the molar solubility of Hg2C2O4 (Ksp = 1.75 * 10−13) in 0.29 M Hg2(NO3)2.

A: Given information: 0.29 M Hg2(NO3)2 Hg2C2O4 (Ksp = 1.75 * 10−13)

Q: A solution contains 5.61×10 M silver acetate and 5.52x10 M calcium nitrate. Solid sodium sulfite is…

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

Q: Agl (silver iodide, Ksp " 8.51 x 1017, is a low solubility/insoluble salt. Ag(CN)2 has a formation…

A: a) Reaction of AgNO3 and NaI is as follows: AgNO3 + NaI →AgI + NaNO3 As per the reaction 1 mole…

Q: What is the molar solubility of Ca(OH)2? Ksp = 8.0 x 10-6

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Q: 2. A Mg(OH)2 solution has a concentration of 4.0x10-5 M. Calculate the molarity of each ion in…

A: since, 2 mol OH- is produced from 1 mol Mg(OH)2 hence molarity will be doubled for OH-

Q: Ksp of Lead iodide (Pbl2) is 1.4 x 10 8. Calculate the molar solubility of this compound. O 4.5 x…

A: Given Ksp = 1.4 × 10-8

Q: Determine the molar solubility of PBSO4 in pure water. Ksp (PbSO4) = 1.82 x 108. O 1.82 x 10-8 M…

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