Inorganic chemistry help please! Please only answer if you can answer it entirel
ID: 505697 • Letter: I
Question
Inorganic chemistry help please! Please only answer if you can answer it entirely.
If a saturated solution prepared by dissolving silver (I) carbonate in water has [Ag^+1] = 2.56 x 10^-4 M, what is the value of the Ksp for silver (I) carbonate. Use LeChatelier's principle to explain the following changes in the solubility of silver (I) carbonate in water: Why does the solubility decrease upon addition of silver(I) nitrate Why does the solubility increase upon addition of nitric acid Why does the solubility decrease upon addition of sodium carbonate Why does the solubility increase upon addition of ammoniaExplanation / Answer
3. Silver carbonate dissociates as Ag2CO3(solid) = 2Ag+(solution) + (CO3)2-(solution)
So here concentration of Ag+ is 2S if (CO3)2- is assumed as S. Now solubilty product which is designed normally as Ksp for such type of solution is [Ag+]2[CO32-] = [2S]2[S] = 4S3
In your question 2S = 2.56 X 10-4
From that calculating we get 4S3 = 4 X (1.28X 10-4)3 = 8.39X 10-12
4. Le Chatelier Principle is thatwhen a system in equilibrium is disturbed the system will adjust itself in such a way that the effect of the change will be nullified. Now have a look at the above equilibrium from Q3. Here the right side has Ag+ and CO32- ions.
Now in Q4 the first and third condition suggests silver nitrate and sodium carbonate is being added. First one has Ag+ and second one has CO32- ions. So in these two cases the concentration of right side ions increases. To nullify these change the solubility of silver carbonate has to decrease on each case so that concentration of those ions dont become excess.
Now the 2nd and 4th case. Here the nitric acid reacts with the silver carbonate and the products of them becomes soluble in the water or gets out of reaction medium(the CO2).
Ag2CO3 + 2HNO3 = 2AgNO3(highly soluble) + H2O + CO2
So obviously the solubility of silver carbonate increases.
In 4th case the ammonia reacts with the cation of the right side equilibrium to form Ag(NH3)+ complexes because of which the concentration of silver ion decreases and to nullify the effect more silver carbonate has to convert to its ions i.e the right side reaction which means increase in solubilty of silver carbonate.