Silver Nitrate (AgNO3) at a concentration of 0.0500M is being utilized to titrate a mixture of 0.01000 M K2CO3 and 0.01000 M NaIO3.   A) Which anion will precipitate first? Ksp = 3.1 x 10-8 for AgIO3 Ksp = 8.1 x 10-12 for Ag2CO3. Show how you arrived at your answer.   B) Can 95% of the first anion that is precipitated be titrated without causing the precipitation of the second? Show how you arrived at your answer by calculation starting with 50.00 mL of the solution. Be sure to account for dilution in your calculation

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A: [Fe2+] = 0.106 M [Ba2+] = 0.103 M To find the solubility of carbonate solution compares its Ksp…

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Q: What is the solubility of La(IO₃)₃ in a solution that contains 0.100 M IO₃⁻ ions? (Ksp of La(IO₃)₃…

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Q: If 50.0 mL of 0.444 M AgNO3 is mixed with 50.0 mL of 0.00244 M NaBr, does a precipitate form? (Ksp…

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Q: FIPST, Ag2CrO4 or BaCrÓ4? (Ksp for Ag2Cr04 = 2.0 x 10-12; Ksp for BaCrO4 = 1.2 x 10-10) %3D %3D b)…

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Q: Find the solubility of AgI in 3.3 M NH3. (Ksp of AgI = 8.3 10-17 and Kf of Ag(NH3)2+ = 1.7 107)

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Q: What is the [Ag*] in a saturated solution of Ag₂SO4 in 0.20 M Na₂SO₂? Use the Data Tables to find…

A: Given, Na2SO4 concentration =0.20 M

Q: ksp- Is it possible to precipitate 99.0 % of 0.010 M Ce by adding CrO,2 without precipitating 0.010…

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Q: A solution is prepared by mixing 30.0 mL of 0.0100 M Mg(NO3)2 and 25.0 mL of 0.100 M NaF. Calculate…

A: GIVEN:-

Q: 1 Consider a flask containing 50.00 mL of 0.0426 M trimethylamine ((CH3)3NH3). This is titrated with…

A: the pH of the solution can be found using ICE approach.

Q: In which case will a precipitate form? (i) a 0.050 M MnCl2 solution with pH = 8.00 (Does Mn(OH)2…

A: Hi there! Since you have posted multiple questions, we will answer the first question for you.

Q: A 1.0 M Na2SO4 solution is slowly added to 10.0 mL of a solution that is 0.20 M in Ca2+ and 0.30 M…

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Q: What is the molar solubility of CdS in a solution in which [H30*] is held constant at 0.1 M? (Ksp…

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Q: A 30.00-mL solution containing 0.1553 M Na2C2O4 was titrated with 0.1250 M Ca(NO3)2 to precipitate…

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Q: will there be a precipitate in the mixture of 50 ml of Pb(NO3)2 5.0 x 10-3 mol/L  with 100 ml of…

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Q: CrO42- can be used as an indicator when Br- is titrated with Ag+. What concentration of CrO42-…

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Q: 0. Will a B(OH)2 precipitate form if 250.0 mL of 0.01 M B3Y2 is mixed with 50.0 mL of pH 12.0 a(OH),…

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Q: What is the molar solubility of Ag2SO4 in a solution that is 0.0522 M AgNO3? Ksp= 1.40x10^-5

A:

Q: The K sp of an unknown salt, MZ 2, is 2.9 × 10 –11. Calculate the solubility (in mol/L) of MZ 2 in a…

A: Given data contains, Ksp of the unknown salt is 2.9×10-11. The solubility equilibrium of unknown…

Q: Q3:- 15 mL of 0.03 M Pb(NO3)2 is added to 20 mL of 0.2 M NaCl. Predict if precipitate of PbCl2 will…

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Q: 10. A saturated solution of Ba3(AsO4)2 has a Ksp of 1.1 x 10-13. a. Determine the solubility of…

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Q: What is the Cl- concentration just as Ag2CrO4 begins to precipitate when 1.0 M AgNO3 is slowly added…

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Q: 1. The molar solubility of Ag2SO3 is 1.55× 10-4 M. Calculate the Ksp of Ag2SO3. a. 7.45 x 10^-12…

A: Since you have posted multiple questions, we will solve only first question for you. If you want the…

Q: What is the expected result when 100 mL of a solution that is 0.002 M Ca(NO3)2 and 0.002 M Pb(NO3)2…

A: Given that Concentration of Ca(NO3)2 =   0.002 M    Volume = 100ml

Q: What is the molar solubility of Agl Ksp 8.3 x 1017 in the presence of 0.05 M KI? O 2.34 x 10^(-11) M…

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Q: 4) How would your calculated value of Ksp be affected by errors introduced from the following…

A: Ksp is meant for solubility product constant. It is the equilibrium constant for a solid substance…

Q: 10. Will a B(OH)2 precipitate form if 50.0 mL of 0.03 M B3X2 is mixed with 350.0 mL of pH 11.5…

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Q: In which solution will 0.000015 M Pb(NO3)2 form a precipitate?   0.050 M NaF (Ksp of PbF2=3.6x10-8)…

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

A: The equilibrium reaction during dissociation of Cr(IO3)3 can be written as follows : The expression…

Q: 2. What concentration of OH is required to begin the precipitation of Cu(OH)2 from a solution…

A: Given, Concentration of Cu2+ = [Cu2+] = 0.10 M  Ksp for Cu(OH)2 = 2.2 × 10-20 Concentration of OH- =…

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

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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: Calculate the molar solubility of Cr(OH)3 (Ksp = 6.3 × 10-31 at 25 ºC). a. 2.8×10-8 M b. 1.2×10-8 M…

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Q: A 1 L solution contains 0.25 M Ni(NO3)2 and 0.25 M Cu(NO3)2. A. Can the metal ions be separated by…

A: In a solution, when the amount of the solute present in the solution is equal to the exact amount…

Q: A saturated solution of Ca3(PO4)2 has a Ksp of 1.2 x 10-26.    Determine the molar solubility of…

A: Ca3(PO4)2 ↔3Ca+2  + 2PO4-3 K3PO4. ↔3K+ + PO4-3 Ca(NO3)2 ↔Ca+2  + 2NO3-

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for