the solubility product of AgBr(s) is 1.48 ×10^-13. what is the concentration of Ag+ in a saturated solution of AgBr?

Question

Question

Answer 1

Answer #1

Ag Br(s) Agt + Bri Ksp = [Agt] [BMC) 1.48X16 13 = x. x X = 3.85 X167M [Ag+)= x= 3.85 x107m

Answer 2

Similar Homework Help Questions

Consider a saturated AgBr solution that is also 0.050 M Ca(NO3)2. Ca(NO3)2(aq) + Ca2+ (aq) +...

Consider a saturated AgBr solution that is also 0.050 M Ca(NO3)2. Ca(NO3)2(aq) + Ca2+ (aq) + 2NO3 (aq) AgBr(s) Ag+ (aq) + Br-(aq) The thermodynamic solubility product (Kop) of AgBr is 5.0 x 10-13. What must be the molarity of Ag+ in the solution?
Consider a saturated AgBr solution that is also 0.050 M Ca(NO3)2. Ca(NO3)2(aq) + Ca2+ (aq) +...

Consider a saturated AgBr solution that is also 0.050 M Ca(NO3)2. Ca(NO3)2(aq) + Ca2+ (aq) + 2NO3(aq) AgBr(s) + Ag+ (aq) + Br (aq) The thermodynamic solubility product (Kyp) of AgBr is 5.0 x 10-13. What must be the molarity of Ag+ in the solution?
3 (5 pts). The solubility product reaction for AgBr is AgBAg Ag+e Ag (s) Eo -0.799...

3 (5 pts). The solubility product reaction for AgBr is AgBAg Ag+e Ag (s) Eo -0.799 the solubility product of AgBr. Br. Use the reactions V and AgBr () +eAg (s)+Br E 0.071 V to compute

A saturated solution of calcium iodate contains 2.37 g/L of Ca(IO3)2. (a) What is the solubility...

A saturated solution of calcium iodate contains 2.37 g/L of Ca(IO3)2. (a) What is the solubility of calcium iodate in mol/L? (b) What are the concentrations of Ca2+ and IO3 – ion, respectively, in the saturated solution? (c) Calculate the Ksp value for Ca(IO3)2. Part b ) Silver ion, Ag+ , readily forms complex ion, Ag(S2O3)2 3– , with thiosulfate, S2O3 2– , according to the following equation: Ag+ (aq) + 2S2O3 2– (aq) ⇌ Ag(S2O3)2 3– (aq); Kf =...
What is the solubility of AgBr in 0.05 M NaCN? Ksp(AgBr) = 5.0 x 10-13 and...

What is the solubility of AgBr in 0.05 M NaCN? Ksp(AgBr) = 5.0 x 10-13 and Kr(Ag(CN)2') = 1.0 x 1021 LIS-ntion of drico Coel is always spontaneous, never
Consider the following information at 25 ºC: AgBr(s) + e- → Ag(s) + Br-(aq) Eº(AgBr(s),Ag(s)) =...

Consider the following information at 25 ºC: AgBr(s) + e- → Ag(s) + Br-(aq) Eº(AgBr(s),Ag(s)) = 0.07133 V Ag+(aq) + e- → Ag(s) Eº(Ag+(aq),Ag(s)) = 0.7996 V What is the value of the solubility product equilibrium constant Ksp(AgBr) of silver bromide? AgBr(s) ↔ Ag+(aq) + Br-(aq) Ksp(AgBr)

5. (15 marks) What is the solubility of AgBr (Ksp = 5.0*10-13) in the following solutions:...

5. (15 marks) What is the solubility of AgBr (Ksp = 5.0*10-13) in the following solutions: a) pure water. b) in a solution of 1.0 M NH3 (K,= 1.6x107 for [Ag(NH3)2]t).
1. The concentration of Ag+ ion is a saturated aqueous solution of Ag2CrO4 was found potentiometrically...

1. The concentration of Ag+ ion is a saturated aqueous solution of Ag2CrO4 was found potentiometrically equal to 1.56 x 10-4 M. Calculate the solubility in grams per liter and its solubility product. 2. The solubility product of a compound with a general formula M2X was found equal to 3.58 x 10-13 on the basis of solubility measurements and on the assumption that the ions formed are M7 and X-2. A more careful determination of the ionic species determined that...
a. The solubility product, Ksp, for AgI is 8.3 x 10-17. What is the concentration of...

a. The solubility product, Ksp, for AgI is 8.3 x 10-17. What is the concentration of iodide ion (I- ) in solution saturated in silver iodide. b. What would the concentration of silver(I) ion (Ag+ ) be for a saturate solution of AgI which is also 0.20 M in NaI (soluble, of course)

The Ksp of AgBr is 5.4x10^-13. What is the molar solubility of AgBr? The Ksp of...

The Ksp of AgBr is 5.4x10^-13. What is the molar solubility of AgBr? The Ksp of AgBr is 5.4 x 10-13. What is the molar solubility of AgBr? 8.64 x 10-13 7.35 x 10-7 2.43 x 10-12 Not enough information 5.4x 10-13