Please don\'t do 4!! 2. Consider the following equilibrium: 2+, BaSO4(s) In whic
ID: 493685 • Letter: P
Question
Please don't do 4!! 2. Consider the following equilibrium: 2+, BaSO4(s) In which direction will the equilibrium shift if a. H2SO4 is added? Why? b. Baci2 is added? Why? c. NaCl is added? Why? d. Heat is added? Why? 3. Consider the following equilibrium for nitrous acid, HNO2,a weak acid: HNO2(aq) H2O() H3O (aq) NO2 (aq) In which direction will the equilibrium shift if a. NaOH is added? b. 2 is a c. HCl is added? d. The acid solution is made more dilute? 4. Complete and balance the following equations and then write balanced net ionic equations. a. AgNO3(aq) HCl(aq) b. NH3(aq) HCl(aq) c. Na2CO3 (aq) HNO3(aq) 5. On the basis of LeChatelier's Principle, explain why Ag2Co3 dissolves when HNO3 is added.Explanation / Answer
2a. When H2SO4 is added to BaSO4 salt it has no effect on the equilibrium since delta H (enthalpy) of reaction is more than zero and is unfavorable.It requires high amount of heat to separate Barium and sulfate ions.
2b & c. When BaCl2 and NaCl are added to suspension of BaSO4 in water they have no effect on the equilibrium as BaSO4 is a neutral salt and doesn't dissolve in water while other two salts readily dissolve in water.
2d. Whe heat is applied it drives the equilibrium to right side as its delta H >0 and an endothermic reaction.
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3a. When NaOH, a strong base, added to weak acid we get a basic salt such as NaNO2.and drives the equilibrium to right side until all the nitrite ions on the right side are consumed.
3b. When NaNO2, is added it has no effect on the equilibrium of reaction as it simply dissolves in water.
3c. When HCl, a strong acid, is added to the reaction mixture, it drives the equilibrium to right side as it protonates free water.
3d. When the solution diluted further it drives equilibrium to left side as there will be more free water and less of protonated water (H3O+).
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5. Le Chatelier's principle is also known as Equilibrium Law in chemical reactions according to which when chemical system at equilibrium is subjected to change in concentration, temperature, volume, or pressure, then the system readjusts itself to (partially) counteract the effect of the applied change and a new equilibrium is established.
Silver carbonate is poorly soluble in water i.e poorly ionizes into Ag+ and CO32- ions. However when HNO3, a weak acid, is added to an aqueous solution of Ag2CO3 it drives the equilibrium to right side as silver nitrate is formed which is readily soluble in water. The carbonate anion reacts with acidic protons and forms carbonic acid H2CO3 which readily decomoses into CO2 and H2O. So the equilibrium is driven to right side until all the carbonate anion is consumed.
Ag2CO3 + 2HNO3 ....................> 2 AgNO3 + CO2 + H2O
2H+ + CO32-................................> H2CO3 ........................> CO2 + H2O