The answer is Option B. PQ-23. AgBr has very low solubility in water. Silver ions form...
Question 52 1 pts AgBr has very low solubility in water. Silver ions form a complex ion with thiosulfate, Ag*(aq) + 25,032(aq) =(Ag(S203)213(aq) If sodium thiosulfate is added to a saturated solution of AgBr in equilibrium with solid AgBr, how will the concentrations of free Ag (aq) and Br"(aq) change? What is the equilibrium expression for the reaction below? Fe2O3(s) + 3CO(g) = 2Fe(s) + 3CO2(g) K - [Fe] [co, (Fe,0][co] K - [Fe20][co [Fe] [co,]
The solubility of AgBr in water is 5.74×10-7 M, but increases in the presence of thiosulfate ion. Calculate the solubility of AgBr when the solid is added to a solution that is 0.795 M in thiosulfate ion. For AgBr, Ksp = 3.30×10-13 and for Ag(S2O3)23-, Kf = 2.00×1013. Solubility = M
all 5&6 5.) Solid silver bromide , AgBr, can be dissolved by adding concentrated aqueous ammonia to give the water- soluble silver-ammonia complex ion. AgBr(s) + 2NH,(aq) U Ag(NH), (aq) + Br(aq) (a) Show that this equation is the sum of two other equations, one representing the dissolution of AgBr into its component ions and the other representing the formation of the silver-ammonium complex from silver ion and ammonia (b) Calculate the equilibrium constant for the above reaction K,(AgBr) =...
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 =...
The solubility of AgBr in water is 5.7410-7 M, but increases in the presence of thiosulfate ion. Calculate the solubility of AgBr when the solid is added to a solution that is 0.692 M in thiosulfate ion. For AgBr, Ksp-3.30x10-13 and for Ag(S203)2, Kr-2.00x1013] Solubility
H. Complex Ions 1. Silver chloride has very low solubility in water (Ks of 1.6 x 10-19), however, it is highly soluble in an ammonia solution due to the formation of the complex ion [Ag(NH3)21 (Kr" 1.7 X 10) Given this information, calculate the molar solubility of AgCl in 2.25 M ammonia. 2. Calculate the molar solubility of Cul in 0.92 M KCN. (Ksp of Cul is 1.1 x 10-12, Kp of [Cu(CN)2] is 1.0 x 1016).
Unexposed silver halides are removed from photographic film when they react with sodium thiosulfate (Na2S2O3, called hypo) to form the complex ion Ag(S2O3)23-. The reaction with silver bromide is: AgBr(s) + 2 S2O32- (aq) ⇌ Ag(S2O3)23- (aq) + Br- (aq) The equilibria that need to be considered are: Ag+ + 2 S2O32- (aq) ⇌ Ag(S2O3)23- (aq) Kf = 4.7 x 1013 AgBr(s) ⇌ Ag+ (aq) + Br- (aq) Ksp = 5.0 x 10-13 What mass of Na2S2O3 is required to...
Be sure to answer all parts. Commercial silver-plating operations frequently use a solution containing the complex Ag+ ion. Because the formation constant (Kf) is quite large, this procedure ensures that the free Ag+ concentration in solution is low for uniform electrodeposition. In one process, a chemist added 9.0 L of 5.0 M NaCN to 90.0 L of 0.17 M AgNO3. Calculate the concentration of free Ag+ ions at equilibrium. See your textbook for Kf values. × 10 M (Enter your...
Please help asap =) 2. Lead(II)chloride is insoluble in water Kap PbCn 1.7x10-) and silver chloride is very insoluble in water (Ksp Agci 1.8x10-10). The reactions when they go into solution are: AgCl(s) ←→ Ag+(aq) + Cl-(aq) PbCl2(s)艹Pb+2(aq) + 2 Cl-(aq) a. What are the expressions for the equilibrium constants, Kop for the above reactions? b. Explain why it is possible to dissolve more lead(I)chloride in solutions in which the concentration of the silver ion is present. c. Explain what...
please answer all 4 SP TCalculate the molar solubility of AgBr (Ksp - 5.0 x 1013) in a 0.17 M CaBr2 solution. CaBr is 100% soluble. +2 Ca +28r 6 CaBiz 4. The following pictures represent solutions of AgCl, which may also contain ions other than Ag+ and Cl- which are not shown. Gray spheres represent Ag' ions and dotted spheres represent Cl' ions. If solution (1) is a saturated solution of AgCl, which of solutions (1-4) represents the solution...