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...
ESCUCU SEDIUS QUESTION 11 The following combination of species will result in buffer solution. a. HCO3 and C032 True False QUESTION 12 The complexion CHOHA is formed from a solution that initially contains 3.50 * 10-M CHNO3 and 0.035 MOH. C ag) + 4 OH ) CHOHam) 2 x 1033 2x 10-31 M 2 x 10 30 2x10 26M QUESTION 13 The complexes of new bonded to s u ch as CLIN2 knows com os True False QUESTION 14 Click...
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....