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 .
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 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 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 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)
1) Write the solubility-product expression for the following mercury salts: Hg2Cl2 and HgCl2. 2) Exactly 0.133 mg of AgBr will dissolve in 1.00 L of water. What is the value of Ksp for AgBr? 3) By experiment, it is found that 1.2 x 10-3 mol of lead (II) iodide, PbI2, dissolves in 1.0 L of water at 25°C. What is the Ksp at this temperature? 4) What is the molar solubility of silver chloride in 1.0 L of solution that...
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 [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+, 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...