Ag2S dissociates as:
Ag2S(s) <-> 2 Ag+(aq) + S2-(aq)
[Ag+] will be twice that of S2-
In given question both the concentrations are same.
So, the answer is false
Answer False
Question 12 The following compounds precipitates from a solution with the concentrations indicated. Ag2S: [Ag+] =...
Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.) (a) CaCO3: [Ca2+] = 0.003M, [CO32−] = 0.003M (b) Co(OH)2: [Co2+] = 0.01M, [OH–] = 1 × 10–7 M (c) CaHPO4: [Ca2+] = 0.01M, [HPO42−] = 2 × 10–6 M (d) Pb3(PO4)2: [Pb2+] = 0.01M, [PO43−]= 1 × 10–13 M
Which of the following compounds precipitates from a solution that has the concentrations indicated? (See Appendix J for Ksp values.) (a) CaCO3: [Ca2+] = 0.003 M, [CO3 2−] = 0.003 M (b) Co(OH)2: [Co2+] = 0.01 M, [OH–] = 1 × 10–7 M (c) CaHPO4: [Ca2+] = 0.01 M, [HPO4 2−] = 2 × 10–6 M (d) Pb3(PO4)2: [Pb2+] = 0.01 M, [PO4 3−] = 1 × 10–13 M
D2. (8 pts) Determine whether the following compound precipitates from a solution that has the concentrations indicated. [Pb"+-0.0030 M, [1] Pbl2 (s)Pb2 (aq) 2 I (aq) 1.3 x 10" M Kip8.7 x 10
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
Consider a solution that is 1.34 x 10^-5 M in Ag(NO3). Which of the following concentrations of KCl will result in the precipitation of AgCl? (Ksp = 1.8 x 10^-10) Please show work and all steps.
With which of the following solutions would a 3.5 x 10M solution of Ag+ ions NOT form a precipitate? Formula Ksp A) 5.0 * 10M CH AgCI 1.8 x 10-10 B) 5.0 * 10%MPO Ag3PO4 8.9 x 10-17 C) 5.0 * 10-MBT AgBr 5.0 x 10-13 D) 5.0 * 10-MCO AgaCO3 8.1 x 10-12
Problem 2: Find the concentrations of Ag, CN, and HCN in a saturated solution of AgCN whose pH is somehow fixed at 9.00. Consider the following equilibria: Ksp = 2.2 x 10-16 AgCN(s) CN + H20 Ag+ + CN- HCN(aq) + OH- Kb = 1.6 x 10-5
pls explain :) QUESTION 12 Which of the following compounds will have a different solubility with a change in pH? 1.AgNO3 2. CaCl2 O 3. Ca(OH2 4. CuCI O5. Hg2Cl2 QUESTION 5 The K sp of AgCl at 25 °C is 1.6x10-10 Consider a solution that is 2.0 x 10-6M NaCl and 1.0x 104 M AgNO 3 1.Q > Ksp and a precipitate will not form O 2.Q< Ksp and a precipitate will not form 3. The solution is saturated...
1. 200 mL of an aqueous solution contains 0.030 M concentrations of both Pb2+ and Ag+. If 100 mL of 6.0 x 10-2 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The Ksp values for PbCl2 and AgCl are 1.7 x 10-5 and 1.8 x 10-10] 2. Which of the following is the expression for the solubility product of Ba3(AsO4)2? 3. The pKa of a weak acid is 6.50. What...
1. 200 mL of an aqueous solution contains 0.030 M concentrations of both Pb2+ and Ag. If 100 mL of 6.0 x 102 M NaCl is added to this solution will a precipitate form? If so, what will the precipitate be? The Ksp values for PbCl2 and AgCl are 1.7 x 105 and 1.8 x 10-19 2. Which of the following is the expression for the solubility product of Baz(AsO4)2? a. Ksp=[Ba2+[AsO4? 12 b. Ksp=[3 x Ba2+[2 x AsO42-12 c....