Solid potassium chromate (K2CrO4) is slowly added to a solution containing 0.50 mol L-1 AgNO3 and 0.50 mol L-1 Ba(NO3)2. What is the Ag+ concentration when BaCrO4 just starts to precipitate? The Ksp for Ag2CrO4 and BaCrO4 are 1.1 × 10-12 and 1.2 × 10-10, respectively.

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: The Ksp of iron (II) hydroxide is 8.65 x 104 iron (III) hydroxide? -20 What is the molar solubility…

A: The solubility of iron (III) hydroxide can be expressed as: Ksp = Fe3+OH-3Ksp = s3s3Ksp = 27s4

Q: The Kp value for Al(OH)3 is 3.0 x 10-34. Part 1 You answered correctly! Move on to the next part.…

A: Given : Al(OH)3 of the Ksp = 3.0 ×10-34 PH = 9.59   Finds : To calculate the Molar solubility of…

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: 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: 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: ecipitate Another Solid cobalt(II) acetate is slowly added to 75.0 mL of a 0.0317 M potassium…

A: Given,  [KOH] = 0.0317 M  Volume of KOH in mL = 75.0 mL  Now,  Solubility product of Co(OH)2 = Ksp…

Q: Would a precipitate of silver acetate form if 22.0 mL of 0.100 M AgNO3 were added to 45.0 mL of…

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

Q: The magnesium and calcium ions present in seawater have the following concentrations: [Mg2+] = 059 M…

A: The objective of the question is to find the pH at which the selective precipitation of Mg2+ ion…

Q: <Assignment 16-5 + Fractional Precipitation of Metal Carbonates The solubility product constants, K.…

A: [Fe2+] = 1.08 x 10-2 M [cd2+] = 1.59 x 10-2 M

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…

A:

Q: What is the minimum concentration of OH required to precipitate Cu(OH), in this solution? \- b. What…

A: The Solubility Product (Ksp)  for  Cu(OH)2=[Cu2+][OH−]2 -----------1 Now, given that [Cu2+]= 1 x…

Q: A solution contains 0.0480 M Ca²+ and 0.0940 Agt. If solid Na3PO4 is added to the mixture, what is…

A:

Q: following mixture. Ksp for BaSO4 = 1.08 × 10−10, Ksp for SrSO4 = 3.44 × 10−7 I. Add 650 mL of…

A:

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: 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…

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

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: mix 15 ml 0.01 M CaCl2 solution with 25 ml NaOH 0.001 M.A precipitate calcium hydroxide knowing that…

A: In such type of question determine Qsp and compare it with Ksp. If Qsp &gt; Ksp then precipitate is…

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: A student titrates 20.0 mL of 1.0 M NAOH with 2.0 M formic acid, HCOOH (K, = 1.8 x 10-4). How much…

A: we have, 20 mL of 1M NaOH 2M of HCOOH ( Ka= 1.8×10-4)

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…

A:

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: How many grams of sodium sulfate can be added to 595 mL of 1.6 x 10 M barium chloride before a…

A:

Q: Will a precipitate of AgBr form if 5.2 × 10-4 M AgNO3 is mixed with 1.0 × 10-4 M NaBr? The Ksp of…

A: Given: Concentration of AgNO3 = 5.2 x 10-4 M                        (2 significant…

Q: How many grams of sodium sulfate can be added to 310. mL of 1.5 x 10-3 M barium chloride before a…

A: The solubility reaction of BaSO4 is given by  =&gt; BaSO4 (s) ----&gt; Ba2+ (aq) + SO42- (aq)  Hence…

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 molar solubility (in mol L-1¹) of a salt with general molecular formula MX₂ (where M is…

A:

Q: In which solution will 0.0020 M AgNO3 form a precipitate? a 7.1x10-7 M NaBr (Ksp of AgBr=5.0x10-13)…

A: Data given:  Concentration of AgNO3 = 0.0020 M  a. Concentration of NaBr = 7.1×10–7 M (Ksp of AgBr =…

Q: The molar solubility of Ag2 S is 1.26 x 10-16 M in pure water. Calculate the Ksp for Ag2 S. O 1.12 x…

A: Given values -&gt; Solubility = 1.26 × 10^-16 M

Q: The molar solubility of palladium (II) thiocyanate at 25°C is 2.22 x 10-8 M. What is its Ksp value?…

A: molar solubility=S=2.22×10-8M KSP=?

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…

A: Given data, Molarity of B3X2 = 0.03M Volume of B3X2 = 50.0mL = 0.050L pH of Mg(OH)2 = 11.5 Volume of…

Q: Does a precipitate of La(IO3)3 form when 0.25 L of 1.0x10-3 M La(NO3)3 is mixed with 0.15 L of…

A: Given : Concentration of La(NO3)3 = 1.0 X 10-3 M Volume of La(NO3)3 solution = 0.25 L Concentration…

Q: When 200.0 mL of 5.15 x 10-4 M Ba(NO3)2 is added to 150.0 mL of 8.25 x 10-4 M Na2SO4. Ksp(BaSO4) =…

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

Q: -4 When 22.0 mL of a 3.72 × 10-4 M ammonium sulfate solution is combined with 15.0 mL of a 7.43 ×…

A:

Q: hat percent of Ba2+ ions remain  when CaSO4 begins to precipitate from asolution that is 0.05M in…

A: To determine the percent of Ba2+ ions remain when CaSO4 begins to precipitate from the solution.…

Q: Will a precipitate form Ksp = 7.08 x 10-9 for M

A: To determine if the concentration of Mg+2cation and F- anion are high enough to allow for the…

Q: Write a balanced net ionic equation to show why the solubility of Fe(OH)3(s) increases in the…

A: The dissociation reaction for Fe(OH)3 is shown below, Fe(OH)3(s) →Fe3+(aq) + 3OH−(aq)

Q: Calcium hydroxide has a solubility product of Ksp = 5.02 x 10-6. What mass of calcium hydroxide can…

A: The objective of this given question is to calculate the amount of a sparingly soluble salt that can…

Q: pH of the buffer after the addition of the NaOH

A: pKa(CH3COOH) = 4.74 Moles = M × V (L)   Moles of Acetic acid =  M × V(L)     = 0.281 × 0.300   =…

Q: Calculate the solubility of Ag3PO4 in 0.10 M AgNO3? Ksp = 1.1x10^-16

A: Answer:- This question involves the common ion effect which will suppress the solubility. So,…

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