Add 1ml of 0.18M of HCl (aq) to 1ml of 0.2M of [Ag(NH3)2]Br (aq).
Write the any equation between hcl(aq) + [ag(nh3)2]br(aq) and the overall equation. Calculate k at equilibrium.
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Add 1ml of 0.18M of HCl (aq) to 1ml of 0.2M of [Ag(NH3)2]Br (aq). Write the...
Review equation 16.10 and step B2. Ag+1(aq) and NH3(aq) will form a soluble complex ion. Use rule 3 of Water-Insoluble Salts in Appendix E to determine what would happen if Ag+1(aq) was combined with KOH instead of NH3. Write the net ionic equation with phase subscripts, where K+1 is a spectator ion which is cancelled out. Equation 16.10: Ag^+(aq) + Cl^-(aq) ⇄ AgCl(s) ⇅ 2NH3(aq) [Ag(NH3)2]^+(aq) Step B2: Silver Chloride equilibrium. To the clear solution from part B.1, add 5...
Ag+ forms complex ions with NH3 and S2O32- according to the following equilibria: Ag+(aq) + 2 NH3(aq) = [Ag(NH3)2]+(aq) K = 1.7 x 107 Ag+(aq) + 2 S2O32-(aq) = [Ag(S2O32-)2]3-(aq) K = 2.9 x 1013 Determine the value of K for the equilibrium: [Ag(S2O32-)2]3-(aq) + 2 NH3(aq) = [Ag(NH3)2]+(aq) + 2 S2O32-(aq) Using your K value as a guide, predict what would happen when 1 M NH3(aq) is added to a solution of [Ag(S2O32-)2]3-(aq). Explain your reasoning.
1. Given the two equilibria below, Ag(NH3)2(aq) = Agt(aq) + 2NH3(aq); Kd = 5.9 x 10-8 AgBr(s) Ag+(aq) + Br" (aq); Ksp = 5 x 10-13 what is K, for the following equilibrium? AgBr(s) + 2NH3(aq) = Ag(NH3)2(aq) + Br" (aq) a. 3 x 10-20 b.2.7 x 100 c. 7.2 x 10-11 d. 8.5 x 10-6 e. 1.2 x 105
2. Use the data of Part B for the reaction between NH3 (aq) and HCl (aq), and equation 2 to determine: AH for each run in kJ (AHA), AH per mole of limiting reagent for each run, and the average AH/mol of limiting reagent. Assume that the specific heat capacity of the solution is 4.184 J/gºC, the final volume is 100.0 mL, and the density is 1.03 g/mL. Show one sample calculation in the space below. Run # 1 Run...
Given the following reactions, AgBr(s) Ag (aq) + Br(aq) Ag*(aq)2 CN (aq)=Ag(CN)2(aq) K 1.2E+21 determine the equilibrium constant for the reaction below AgBr(s)2 CN-(aq)= Ag(CN)2 (aq) Brr(aq) Ksp 5.4E-13
The equilibrium constant for the following reaction Ag+(aq) + 2NH3(aq) Ag(NH3)2+(aq) is K = 1.7 × 107 at 25°C. What is ΔG° at this temperature? Question 10 options: a) –1.5 kJ b) –23 kJ c) –41 kJ d) –3.5 kJ e) –18 kJ
Consider the following equilibrium: Ag (aq) 2 NH3(aq) Ag(NH)21'(aq) AH15 k How does each of the following situations affect the position of the equilibrium? 1. Dissolving AgNO in the solution. (Remember that metal nitrates are fully soluble in water 2. 3. 4. and will dissociate upon dissolving: MfNOJy(s)->xMn"(aq) + yNO3-(aq).) Bubbling NH, (g) into the solution. (Remember that NIH, gas is soluble in water) Heating the solution. Dissolving NaCl in the solution, given the following information AgClo Ag(a) Cl(aq) K-1.8x...
Ag+(aq)+2NH3(aq)⇌Ag(NH3)2+(aq) choose the lewis base and lewis acid in the equation
The equilibrium constant for the equation Ag+ (aq) + 2NH, (aq) =[Ag(NH),]+(aq) is Kf = 2.5 x 103 M-2 at 25.0 °C. Calculate the value of AGixn at 25.0 °C. C AG = k Is the reaction spontaneous under standard conditions? kJ/mol J/mol no O yes Calculate the value of AGrxn at 25.0 °C when [Ag+] = 0.00138 M, (NH2) = 0.438 M, and [[Ag(NH3)2]+] = 0.00739 M. Is the reaction spontaneous under these conditions? AGrxn = kJ/mol O yes...
[Ag(NH3)2]+ (aq) + e- Ag(s) + 2 NH3 (aq) E= +0.373V Use the standard redox potential of silver below to calculate the stability constant of the silver diamine complex. Ag+ + e- Ag(s) E?= +0.7996V Would you expect the redox potential to increase or decrease if NH3 is replaced with pyridine? Explain your answer