nemical Equilibrium- Le Châtelier\'s post Lab Discussion Questions A. Saturated
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nemical Equilibrium- Le Châtelier's post Lab Discussion Questions A. Saturated Sodium Chloride Chem201L 1. What is the evidence for a shift in equilibrium? 2. W 3. In which direction did the equilibrium shift? 4. If concentrated NaOH hich ion caused the shift in equilibrium? shift back toward the right causing the precipitated NacI to were added to neutralize the HCl, would the solubility equilibrium dissolve? Explain. n why the results for the 6M HCI where different than the 12M HCI. B. Saturated Ammonium Chloride 1. What is the evidence for a shift in equilibrium? 2. Which ion caused the shift in equilibrium? 3. In which direction did the equilibrium shift? C. Iron(III) Chloride and Potassium Thiocyanate 1. What is the evidence for a shift in equilibrium when FeCl, is added to the stock 2, what is the evidence for a shift in equilibrium when KSCN is added to the stock solution? 3. a. What is the evidence for a shift in equilibrium when AgNO, is added to the st solution? (the formation of a precipitate is not the evidence, why?) b. The change in concentration of which ion in the equilibrium caused this equilibrium shift? c. Write the net ionic equation to illustrate how this concentration change occurred d. When the mixture part C4 was divided and further tested, what evidence showed that the mixture still contained Fe3c ions in solution? Copper(ll) Solutions with Ammonia 1, what was the evidence for the first shift in equilibrium when the NH3 was added to 2. a. Explain how adding more NH3/ag) cause the equilibria to shift again. 3. a. Explain how adding 3M H,SO, caused the equilibria to shift back again. D. the Cu solution? b. What observations were made in the Cu? system to indicate that the shift occurred b. What observations were made to indicate the reaction shifted to the left?Explanation / Answer
(1)Saturated sodium chloride solution :- Saturated solution means dissolution(breakdown of salt into ion) of salt is equal to pricipitation of salt (formation of salt or crystal from ions).
1) Evidence for the shift in eguilibrium:-
Na (aq) + Cl(aq) ------- NaCl (s) (precipitation)
NaCl (s)--------Na (aq) + Cl(aq) (dissolution)
Increase in Na+ and Cl- concentration will increase the precipitation of salt(forward direction) means formation of salt increases and increase in NaCl concentration in case of dissolution also increase dissolution of salt(backward direction) means formation of ions occure . Both these processes are in the dynamic equilibrium so rate of forward and backward reaction is equal.
2) Ion that cause the shift in equilibrium:- According to Le Chatelier's principle increase in reactant concentration will cause equilibrium to shift in the product side and vice versa.By considereing the equilibrium, increase in either Na+ and Cl- will lead to the formaion of salt and equilibrium will shift to the formation direction and increase in NaCl will shift the equilibrium to the backward direction.
3) In which direction the equilibrium will shift :- Equilibrium can shift to any direction by change in the concentration of ions or by adition of other compounds either in the reactants and product direction.
4)Adding NaOH increases the concentration of OH- ion in the solution and this OH- ion combine with the H+ to produce water. This increases the H2O concentration in the product side and will shifts the equilibrium to the backward direction.
5) Results of 6M HCl is diffterent from 12M HCl because of different concentration of ion released from the solution of different concentration. So solution at different concentration have different equilibrium constant means reaction of same compounds at different concentration will attain equilibrium at different concentration.
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