C) In ideal solution the activity coefficient is unity and ionic strength is zero. So there is no effect on solubility.
But if we consider non ideal solution ionic strength plays important role on solubility. Upon increasing ionic strength activity coefficient decreases. At a particular temperature solubility product is constant. In order to keep solubility product constant solubility must have to be increased. That is why for non ideal solution concentration of Ag+ increases.
Solid silver bromide (AgBr) will disassociate slightly in water to produce Agand Br". AgBr(s) + Agfaq) + Brīaq) Ksp = 1...
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1. Solid silver bromide (AgBr) will disassociate slightly in water to produce Ag and Br. AgBr(s) +- Agtaq) + Braq) Ksp = 1.3 x 10-5 a. Calculate the equilibrium concentration of Ag if the solution if the solid AgBr is dissolved in pure water. Assume that the solution is behaving ideally (y = 1) b. Now let's explore the reaction if we take into account non-ideal behavior. Calculate the concentration of Ag in...
Free Response Show your calculation approach. Clarity of approach and relevant equations is necessary for partial credit b. Now let's explore the reaction if we take into account non-ideal behavior. Calculate the concentration of Ag" in solution if the solid if the AgBr is dissolved in a solution with an ionic strength of 0.1 (-0.1). Size of Ag' and Br ions (a) are 250 and 300 pm respectively. 1. Solid silver bromide (AgBr) will disassociate slightly in water to produce...
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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) =...
AgBr is sparingly soluble in water and has a Ksp of 5.0 x 10-13. What will be the effect of adding solid NaBr to an aqueous solution of in equilibrium with solid AgBr? Some additional AgBr will precipitate. The Ksp of AgBr will increase. The Agt concentration will remain constant. Additional AgBr will dissolve.
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,]
(aq) (1) Mg(OH)2 is partially dissolved in water: Mg(OH), (s) = Mg2+ (aq) + 2OH Write the Kop expression for Mg(OH)2 : Kp = (2) Solid AgCl is partially dissolved in water: AgCl 2 Ag+ + CI''. If the molar solubility is known as [Ag +) = [CI''] = 1.3x 10 M, AgCl Kip =- (a) 1.3 x 10 (b) 1.69 x 10-10 (c) 2.6 x 10 (d) none of these (3) At 25 °C, the solubility of solid AgCl...