Answer:-
Solubility product(Ksp) is the equilibrium in between a solid substance and its respective ions in the solution.
5. Calculate the solubility product of Agi at 25°C given the following data: £°(V) Agl(s) +...
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Calculate the solubility product of silver iodide at 25 degree C given the following data: AgI(s) + e^- rightarrow Ag(s) + I^- I_2(s) + 2e^- rightarrow 2I^- Ag^+ e^- rightarrow Ag(s) A) 2.9 times 10^- 3 B) 1.9 times 10^- 4 C) 2.1 times 10^- 12 D) 9.0 times 10^- 17 E) 2.4 times 10^- 24 E degree (V) - 0.15 + 0.54 + 0.80
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021 for [Ag(CN)2], calculate the equilibrium constant for the reaction: Agl(s) + 2 CN (aq)[Ag(CN2] (aq) + I'(aq) c) Calculate the molar solubility of Agl in a 0.100 M NaCN solution.
(20 marks) 5. Consider Agl(s), Ksp -8.3x10-17 a) Calculate the molar solubility of Agl in pure water. b) Considering the complex formation constant K 1.0x1021...
Calculate E for the following electrochemical cell at 25 degree C Pt(s)|Sn^2+ (aq, 0.5 M), Sn^4+ (aq, 0.50 M)||I^- (aq, 0.15 M) | AgI(s) | Ag(s) given the following standard reduction potentials. Agl(s) + e^- rightarrow Ag(s) + I^-(aq) E degree = -0.15 V Sn^4+ (aq) + 2 e^- rightarrow SN^2+ (aq) E degree= +0.15 V.
Consider the cell AgcAglo | Agen Ag(s) +0.80 V at which has the standard reduction potentials E°(anode) -0.15 V and E (cathode) 25°C. Calculate (a) the solubility constant of Agl and (b) its solubility at 25°C.
A12a The cell
Ag //AgCl (sat’d), KCl (1.00 M) //NiL2 (0.0250 M), NaL (0.150 M)
//Ni
has a voltage of -0.767 V. What is the overall formation constant
of NiL2?
Given:
AgCl(s) + e Ag(s) + Cl- Eo = +0.222 V Ni2+ + 2e Ni(s)
Eo = -0.257 V
A12b Consider the following standard reduction potential:
Ag+ + e Ag(s) Eo = +0.800 V AgI(s) + e Ag(s) + I- Eo = -0.164
V
Calculate the solubility constant, Ksp at...
The equilibrium constant for the reaction Agl(s) — Ag+ (aq) +1 (aq) is the solubility product constant, Ksp = 8.3 x 10-17 at 25°C. Calculate AG for the reaction when [Ag+]=1.5 x 10-3 M and [Br] =1.5 x 10-2 M. Is the reaction spontaneous or nonspontaneous at these concentrations? AG = 98 kJ/mol, spontaneous AG = 92 kJ/mol, nonspontaneous AG = -65 kJ/mol, spontaneous AG = 65 kJ/mol, nonspontaneous AG = -92 kJ/mol, spontaneous
Given the following standard reduction potentials Ag+(aq) + e- ↔ Ag(s) E = 0.80 V AgCN(s) + e- ↔ Ag(s) + CN-(aq) E = -0.01 V Calculate the solubility product of AgCN at 25°C. 4.3 &αχυτε; 10−14 2.3 &αχυτε; 1013 2.0 &αχυτε; 10−14 5.1 &αχυτε; 1013 None of the above
Be sure to answer all parts. Calculate the molar solubility and the solubility in g/L of Agl at 25°C. The Ksp of Agl is 8.3 x 10-17. x 10 M Enter your answer in scientific notation. x 10 g/L Enter your answer in scientific notation.
Calculate the cell potential for the following cell at 25 ° C Cd (s) | Cd (NO3) 2 (aq, 0.010 M) || KBr (aq, 0.050 M), Ag + (aq) | AgBr (s) | Ag (s) using normal potentials E⦵ (Cd 2+ / Cd) = -0.40 V and E⦵ (Ag + / Ag) = 0.80 V, and the solubility of AgBr, which is 7.7 · 10-13.
Given that, for Agi, at 25°C, Ksp = 1.5x10-16: What is the solubility (g/mL) of Agi in water at 25°C? Submit Answer Tries 0/5 20.0 mL of 0.060 M Nal is mixed with 20.0 mL of 0.120 M AgNO3. What is [I"] in the supernatant solution at equilibrium, at 25°C? Submit Answer Tries 0/5 What is the solubility (mass/volume) of AgI in this supernatant solution? Submit Answer Tries 0/5