Homework Answers
The basic idea behind solving this question is that
if ionic product (Q) is more than solubility product (
i.e Ksp ) then ppt will form otherwise not . ![* Given that, (Ag +] = 3.5X10-4M. For s.ox 10-5M ci- I Q ( Jonic protect) (Agu) = [Ag+] [-] = 3.5x5 x 10 olon der = 1.75x100](http://img.homeworklib.com/questions/4574f2c0-d37c-11eb-9cab-5542fe979b08.png?x-oss-process=image/resize,w_560)
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With which of the following solutions would a 3.5 x 10M solution of Ag+ ions NOT...
A solution is 5.0 x 10-M in each of these ions: Ag+, so -, Cl, and...
A solution is 5.0 x 10-M in each of these ions: Ag+, so -, Cl, and co . Which precipitate will form? Ag2SO4 (Ksp = 1.12 x 10-5) AgCl (Ksp = 1.77 x 10-10 Ag2CO3 (Ksp = 8.46 x 10-12)
For which of the following salts of silver will the concentration of Ag+ ions in a...
For which of the following salts of silver will the concentration of Ag+ ions in a saturated solution have the lowest value? A82SO3 K=1.5 x 10-14 A82CO3, Ksp 8.5 x 10-12 AB2CrOx, Ks-1.1 x 10-12 AgIO.K=3.2 x 10-8 Ag3PO4, K.-8.9x 10-17
10. A solution of AgNO, is slowly added to a mixture containing 0.10 MI, CI, Brand...
10. A solution of AgNO, is slowly added to a mixture containing 0.10 MI, CI, Brand Bros The precipitate, which forms first, is a. Ag! (K 8.3 x 1017) b. AgCI (Rp 1.8 x 101) C. AgBr (Kup 5.0 x 10) d. AgBro (Ksp = 5.5 x 1015) e. More information is needed to determine the salt that precipitates first. Questions 11-14 are free form. Maximum credit is awarded for correct answers with correct units (if applicable) that are supported...
Solid silver nitrate is added slowly to a solution that is 0.0010 M in sodium chloride and 0.0010...
Solid silver nitrate is added slowly to a solution that is 0.0010 M in sodium chloride and 0.0010 M in sodium bromide. What % of the bromide ions remain in solution, ie , unprecipitated, Just before silver chloride begins to precipitate? Kap for AgCI-1.8 x 10-10, Kp for AgBr- 3.3 x 10-13 10. 0.18% 0.018% 0.0010% 0.00010% 0.0018% a. b. c. d. e. 11. Calculate the concentration of F ions in saturated CaF2 solution at 25°C. Kap- 3.9x 10-" a....
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 is 5.0 x 10-5 M in each of these ions: Agt, s02-, Cl-, and...
A solution is 5.0 x 10-5 M in each of these ions: Agt, s02-, Cl-, and CO2- Which precipitate will form? AgCl (K sp = 1.77 x 10-19 Ag2CO3 (Ksp = 8.46 x 10-13) Ag2SO4 (Ksp = 1.12 x 10-5)
4.) Calculate the concentration of ions in the following saturated solutions: a.) [I] in Agl solution...
4.) Calculate the concentration of ions in the following saturated solutions: a.) [I] in Agl solution with (Agt) = 3.7 x 10-?M Ksp Agi = 8.3 x 10-17 b.) [A13+) in Al(OH)3 solution with (OH) = 8.3 x 10M Ksp Al(OH)3 = 1.8 x 10-33 5.) Calculate the heats of combustion for the following reactions from the standard enthalpies of formation listed in Appendix 3: a.) C2H4(g) + 302(8) --> 2CO2() + 2H2O() delta H (kJ/mol): CHA(g) = +52.3 CO2(8)...
We prepare a solution with the following ion concentrations: [Ag+] = 1.0 x 10-6 M and...
We prepare a solution with the following ion concentrations: [Ag+] = 1.0 x 10-6 M and [Cl-] = 1.0 x 10-2 M. If Ksp for AgCl = 1.8 x 10-10, determine which of the following is true. a. a precipitate forms b. a precipitate does not form c. the system is at equilibrium d. not enough information is given to decide
An acidic solution is 2 mM in each of the following metal ions: Zn2+, Cu2+, Co2+,...
An acidic solution is 2 mM in each of the following metal ions: Zn2+, Cu2+, Co2+, Ca2+. a) Which of the metals would precipitate as their hydroxides at pH = 6.00? (Select all that apply. See theappendix.) -zinc -copper -cobalt -calcium b) Which of the metals would precipitate as their hydroxides at pH = 8.00? -zinc -copper -cobalt -calcium c) At what pH do the metal hydroxides begin to participate? Zn(OH)2 ____ Cu(OH)2 ____ Co(OH)2 ____ Ca(OH)2 ____ Substance Ksp...
When 25.0 mL of a 4.80×10-4M potassium sulfate solution is combined with 15.0 mL of a 4.27×10-4M calcium acetate solutio...
When 25.0 mL of a
4.80×10-4M potassium
sulfate solution is combined with 15.0 mL
of a 4.27×10-4M calcium
acetate solution does a precipitate
form? (yes or no)
For these conditions the Reaction Quotient, Q, is equal to ?
The molar solubility of calcium sulfite in a
0.158 M potassium sulfite
solution is ? M.
Solid cobalt(II) acetate is slowly added to
50.0 mL of a 0.0327 M
potassium carbonate solution. The concentration of
cobalt(II) ion required to just initiate
precipitation is...
A solution is 5.0 x 10-M in each of these ions: Ag+, so -, Cl, and co . Which precipitate will form? Ag2SO4 (Ksp = 1.12 x 10-5) AgCl (Ksp = 1.77 x 10-10 Ag2CO3 (Ksp = 8.46 x 10-12)
For which of the following salts of silver will the concentration of Ag+ ions in a saturated solution have the lowest value? A82SO3 K=1.5 x 10-14 A82CO3, Ksp 8.5 x 10-12 AB2CrOx, Ks-1.1 x 10-12 AgIO.K=3.2 x 10-8 Ag3PO4, K.-8.9x 10-17
10. A solution of AgNO, is slowly added to a mixture containing 0.10 MI, CI, Brand Bros The precipitate, which forms first, is a. Ag! (K 8.3 x 1017) b. AgCI (Rp 1.8 x 101) C. AgBr (Kup 5.0 x 10) d. AgBro (Ksp = 5.5 x 1015) e. More information is needed to determine the salt that precipitates first. Questions 11-14 are free form. Maximum credit is awarded for correct answers with correct units (if applicable) that are supported...
Solid silver nitrate is added slowly to a solution that is 0.0010 M in sodium chloride and 0.0010 M in sodium bromide. What % of the bromide ions remain in solution, ie , unprecipitated, Just before silver chloride begins to precipitate? Kap for AgCI-1.8 x 10-10, Kp for AgBr- 3.3 x 10-13 10. 0.18% 0.018% 0.0010% 0.00010% 0.0018% a. b. c. d. e. 11. Calculate the concentration of F ions in saturated CaF2 solution at 25°C. Kap- 3.9x 10-" a....
A solution is 5.0 x 10-5 M in each of these ions: Agt, s02-, Cl-, and CO2- Which precipitate will form? AgCl (K sp = 1.77 x 10-19 Ag2CO3 (Ksp = 8.46 x 10-13) Ag2SO4 (Ksp = 1.12 x 10-5)
4.) Calculate the concentration of ions in the following saturated solutions: a.) [I] in Agl solution with (Agt) = 3.7 x 10-?M Ksp Agi = 8.3 x 10-17 b.) [A13+) in Al(OH)3 solution with (OH) = 8.3 x 10M Ksp Al(OH)3 = 1.8 x 10-33 5.) Calculate the heats of combustion for the following reactions from the standard enthalpies of formation listed in Appendix 3: a.) C2H4(g) + 302(8) --> 2CO2() + 2H2O() delta H (kJ/mol): CHA(g) = +52.3 CO2(8)...
When 25.0 mL of a
4.80×10-4M potassium
sulfate solution is combined with 15.0 mL
of a 4.27×10-4M calcium
acetate solution does a precipitate
form? (yes or no)
For these conditions the Reaction Quotient, Q, is equal to ?
The molar solubility of calcium sulfite in a
0.158 M potassium sulfite
solution is ? M.
Solid cobalt(II) acetate is slowly added to
50.0 mL of a 0.0327 M
potassium carbonate solution. The concentration of
cobalt(II) ion required to just initiate
precipitation is...
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