Homework Answers
![X10 0.005 c) ang pag Kip = [ng+]*[pc] l«5 x 17 18 = [49*70.005] [ng= love see (aq) 360x1018 [Ag] = 336 x 1018 [Ag1= 7.1137x1](http://img.homeworklib.com/questions/003743a0-9fb4-11ea-ab1c-513ae249002b.png?x-oss-process=image/resize,w_560)
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What is the maximum concentration of Ag+ in HM 1x10-6 M) to precipitate Ag3PO4 without precipitating...
A solution is prepared in which the Ag+ ion concentration is 2.5 x 10-3 M and...
A solution is prepared in which the Ag+ ion concentration is 2.5 x 10-3 M and the Cl- ion concentration is 3.2 x 10-4 M. Which of the following statements is true given that the Ksp for AgCl is 1.8 x 10^-10? A)No AgCl(s) will precipitate because Qsp<Ksp. B)No AgCl(s) will precipitate because the Ksp value indicates that AgCl is infinitely soluble in water. C)A precipitate of AgCl(s) will form because Qsp>Ksp. D)Insufficient data is given to make a prediction...
A solution of Na3PO4 is added dropwise to a solution that is 0.0810 M in Ag+...
A solution of Na3PO4 is added dropwise to a solution that is 0.0810 M in Ag+ and 0.00171 M in Cu2+. The Ksp of Ag3PO4 is 8.89e-17. The Ksp of Cu3(PO4)2 is 1.4e-37. (a) What concentration of PO43- is necessary to begin precipitation? (Neglect volume changes.) [PO43-] = M. (b) Which cation precipitates first? Ag+ Cu2+ (c) What is the concentration of PO43- when the second cation begins to precipitate? [PO43-] = M.
What is the maximum concentration of Ag+ that can be added to a 0.00670 M solution...
What is the maximum concentration of Ag+ that can be added to a 0.00670 M solution of Na2CO3 before a precipitate will form? (Ksp for Ag2CO3 is 8.10 x 10-12)
What is the maximum concentration of Ag+ that can be added to a 0.00670 M solution...
What is the maximum concentration of Ag+ that can be added to a 0.00670 M solution of Na2CO3 before a precipitate will form? (Ksp for Ag2CO3 is 8.10 x 10-12)
What is the maximum concentration of Ag⁺ that can be added to a 0.00250 M solution...
What is the maximum concentration of Ag⁺ that can be added to a 0.00250 M solution of Na₂CO₃ before a precipitate will form? (Ksp for Ag₂CO₃ is 8.10 × 10⁻¹²)
8) Calculate the following for 2.0 L solution containing [Ag+] = 0.100 M and [Pb2+] =...
8) Calculate the following for 2.0 L solution containing [Ag+] = 0.100 M and [Pb2+] = 0.100 M. Assume no volume changes. (AgCl Ksp = 1.8 x 10-10, PbCl2 Ksp = 1.8 x 10-5). a) At what [Cl-] will each salt precipitate? b) What percent of the Ag+ has precipitated before the Pb2+ begins to precipitate? c) How much sodium chloride must be added (in grams) to precipitate a maximum AgCl before before any PbCl2 begins to precipitate?
A solution is 0.0045 M in both Pb2+ and Ca2+. Solid Na2SO4 is added to precipitate...
A solution is 0.0045 M in both Pb2+ and Ca2+. Solid Na2SO4 is added to precipitate the sulfates. What concentration of SO42‒ is needed to precipitate as much of the Pb2+ without precipitating the Ca2+? Ksp(PbSO4) = 1.6 × 10‒8, Ksp(CaSO4) = 2.4 × 10‒4
Let's say that the cell compartment for Ag+/Ag contains 100.0 mL of 1.0 M solution. Add...
Let's say that the cell compartment for Ag+/Ag contains 100.0 mL of 1.0 M solution. Add 100.0 mL of 1.0 M NaCl to that compartment. Ksp of AgCl is 1.6 x 10^-10 so the Qsp > Ksp and solid AgCl will precipitate out of solution. This silver chloride is in equilibrium with its ions according to the Ksp equilibrium. Calculate [Ag+] (HINT: it will be very small) and then use your result to calculate the cell potential to the hundredths...
If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Ag2CrO4 ( Ksp =...
If a dilute AgNO3 solution is slowly added
to the solution, what is the first compound to precipitate: Ag2CrO4
( Ksp = 1.2×10?12), Ag2CO3 (
Ksp = 8.1×10?12), or AgCl ( Ksp
= 1.8×10?10)?
Problem 17.75 A solution contains three anions with the following concentrations: 0.20 M Cro 0.10 M CO and 0.010 M Cl Part A If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Aga Cro4 Ksp 1.2 x...
6-19. A solution contains 0.050 0 M Ca2+ and 0.030 0 M Ag+. Can 99% of...
6-19. A solution contains 0.050 0 M Ca2+ and 0.030 0 M Ag+. Can 99% of Ca2+ be precipitated by sulfate without precipitating Ag+? What will be the concentration of Ca2+ when Ag,SO4 begins to precipitate?
6-19. A solution contains 0.050 0 M Ca2+ and 0.030 0 M Ag+. Can 99% of Ca2+ be precipitated by sulfate without precipitating Ag+? What will be the concentration of Ca2+ when Ag,SO4 begins to precipitate?
What is the maximum concentration of Ag+ that can be added to a 0.00670 M solution of Na2CO3 before a precipitate will form? (Ksp for Ag2CO3 is 8.10 x 10-12)
What is the maximum concentration of Ag+ that can be added to a 0.00670 M solution of Na2CO3 before a precipitate will form? (Ksp for Ag2CO3 is 8.10 x 10-12)
If a dilute AgNO3 solution is slowly added
to the solution, what is the first compound to precipitate: Ag2CrO4
( Ksp = 1.2×10?12), Ag2CO3 (
Ksp = 8.1×10?12), or AgCl ( Ksp
= 1.8×10?10)?
Problem 17.75 A solution contains three anions with the following concentrations: 0.20 M Cro 0.10 M CO and 0.010 M Cl Part A If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Aga Cro4 Ksp 1.2 x...
6-19. A solution contains 0.050 0 M Ca2+ and 0.030 0 M Ag+. Can 99% of Ca2+ be precipitated by sulfate without precipitating Ag+? What will be the concentration of Ca2+ when Ag,SO4 begins to precipitate?
6-19. A solution contains 0.050 0 M Ca2+ and 0.030 0 M Ag+. Can 99% of Ca2+ be precipitated by sulfate without precipitating Ag+? What will be the concentration of Ca2+ when Ag,SO4 begins to precipitate?
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