when the pH of both solutions is Note the dynamic equilibrium in the opening plo
ID: 985189 • Letter: W
Question
when the pH of both solutions is Note the dynamic equilibrium in the opening ploto. Which solution changes color increased? Explain. 5. Experimental Procedure, Part ci.Will to increase o the addition of Nac H o to aCH.cooH solution cause the P decrease? Explain. See equation 16.14. 6. A state e 2Ag ong) +co, (ag), exists in solution. a. What shift, if any, occurs in the equilibrium if more Ag.coys)is added to the system? What shift, if any, occurs in the equilibrium if AgNo,daq) is added to the system? c. After water is added to the system and equilibrium is reestablished: what change in the number of moles of Ag (aq) occurs in the system? Explain. (ii) what change in the concentration of Ag (ag) occurs in the system? Explain "d. What shift ooo in equilibrium if HCI(aq) is added to the system? Explain.Explanation / Answer
6.(a) The given reaction in equilibrium is
Ag2CO3(s) <=====> 2Ag+(aq) + CO32-(aq)
Ksp for this reaction is Ksp = [Ag+(aq)]2x[CO32-(aq)]
The value of Ksp is independent of solid reactants or products like Ag2CO3(s). Hence when we add Ag2CO3(s), there would be no change in the equilibrium of the reaction.
(b) When we add AgNO3 to the above reaction, the concentration of Ag+(aq), [Ag+(aq)] will increase. Hence to make the value of Ksp constant more and more Ag+(aq) will react with CO32-(aq) to form Ag2CO3(s). Hence the equilibrium will shift towards left i.e reactant side.
(c) When water is added the concentration of Ag+(aq) and CO32-(aq) decreases. Hence to make the value of Ksp constant, more and more Ag+(aq) and CO32-(aq) are formed and the concentration of Ag+(aq) and CO32-(aq) increases.
(i) Since more Ag+(aq) are formed, number of moles of Ag+(aq) increases.
(ii) There would be no change in the concentration as more Ag+(aq) are formed to make the value of Ksp constant.
(d) When HCl is added it will react with Ag+(aq) to form AgCl(s). Hence the value of [Ag+(aq)] decreases decreasing the value of Ksp. Now to make the value of Ksp constant more and more Ag2CO3 dissociate to form Ag+(aq). Hence the equilibrium shifts towards right i.e towards product side.
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