Post lab 4

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Jan 9, 2024

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HSO4(aq) + H20(l)-> H3O+ (aq) + SO4^-2(aq) 1. When adding sodium sulfate solution, how did the color of the equilibrium mixture change? Initially it started out as a light pink but when adding sodium sulfate it turned into a light orange color. a. The color change indicated a shift in the point of equilibrium. In which direction did the equilibrium shift? (L) left (R) right (N) no change b. Explain your answer to question 1a. You should indicate which ion was added to or removed from the equilibrium mixture. When sodium sulfate was added to the product side, the reaction was product favored causing the reaction to shift right. 2. When adding sodium hydrogen sulfate crystals, how did the color of the equilibrium mixture change? When adding the sulfate crystals the mixture went from a light pink to a darker pink, almost rose. a. The color change indicated a shift in the point of equilibrium. In which direction did the equilibrium shift? (L) left (R) right (N) no change b. Explain your answer to question 2a. You should indicate which ion was added to or removed from the equilibrium mixture. When adding the crystal the mixture got darker and therefore it got more acidic causing there to be more products. 3. Upon heating in which direction is the equilibrium shifting? (L) left (R) right (N) no shift 4. Upon cooling in which direction is the equilibrium shifting? (L) left (R) right (N) no shift 5. Is the forward reaction A. endothermic B. exothermic C. insufficient info

6. Explain your answers to questions 3, 4, and 5. When adding a stressor such as heat the reaction tends to make products. The reaction becomes endothermic as it takes in heat causing it to be a left shift. The opposite reaction happens in the cold. The reaction slows down and releases energy which makes it an exothermic reaction. Therefore it is a right shift reaction. During a forward reaction it uses up the reactants and it releases energy which makes it an exothermic reaction. Equation MgOH2-> Mg2+(ag)+2OH-(aq) 7. When adding concentrated hydrochloric acid, how did the appearance of the equilibrium mixture change? When adding hydrochloric acid the color turned to a light pink color. a. The change in appearance indicated a shift in the point of equilibrium. In which direction did the equilibrium shift? (L) left (R) right (N) no shift b. Explain your answer to question 7a. You should indicate which ion was added to or removed from the equilibrium mixture. It was a left shift reaction because when adding concentrated hydrochloric acid to the products side it causes the products to be favored making it a left shift. 8. When adding EDTA, how did the appearance of the equilibrium mixture change? When the EDTA was added the mixture seems to get clearer than it was before. a. The change in appearance indicated a shift in the point of equilibrium. In which direction did the equilibrium shift? (L) left (R) right (N) no shift b. Explain your answer to question 8a. You should indicate which ion was added to or removed from the equilibrium mixture. When adding EDTA the precipitate went away in the mixture therefore taking away the products and making the reactants favored. 9. Upon heating in which direction is the equilibrium shifting? (L) left (R) right (N) no shift 10. Upon cooling in which direction is the equilibrium shifting?

(L) left (R) right (N) no shift 11. Is the forward reaction A. endothermic B. exothermic C. insufficient info 12. Explain your answers to questions 9, 10, and 11. When the stressor of heat is added products tend to be favored as the result making it a left shift reaction. Opposite to that as cold is added and energy is being released then reactants tend to be favored which makes it a right shift. Overall the forward reaction is exothermic since during the reaction the system loses energy to make the products. Equation 13. When adding silver nitrate solution, how did the color of the equilibrium mixture change? It changed from blue to pink a. The color change indicated a shift in the point of equilibrium, in which direction did the equilibrium shift? (L) left (R) right (N) no shift b. Explain your answer to question 13a. You should indicate which ion was added to or removed from the equilibrium mixture. Since silver nitrate (AgNo3) is an ionic compound (metal and nonmetal), it will dissociate into ions. Ag+ and No3- will be added to the equilibrium mixture. Cl- would be removed because of the added Ag+. 14. When adding hydrochloric acid, how did the color of the equilibrium mixture change? It changed from pink to blue a. If a color change indicated a shift in the point of equilibrium. In which direction is the equilibrium shifting? (L) left (R) right (N) no shift

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b. Explain your answer to question 14a. You should indicate which ion was added to or removed from the equilibrium mixture. From the HCl, H+ and Cl- ions will be added to the mixture. More products in the form of Cl- will be present in the mixture, so it would shift to the left to restore equilibrium. 15. When adding deionized water, how did the color of the equilibrium mixture change? Explain this observation. The mixture became lighter and more faint. This is because water is a liquid and does not have a concentration, so it will not affect the equilibrium equation in any way and won’t cause a shift resulting in a color change. 16. Upon heating in which direction is the equilibrium shifting? (L) left (R) right (N) no shift 17. Upon cooling in which direction is the equilibrium shifting? (L) left (R) right (N) no shift 18. Is the forward reaction A. endothermic B. exothermic C. insufficient info 19. Explain your answers to questions 16, 17, and 18. Since the forward reaction is exothermic, heat is released from the system. This means that heat is a product of the system, and when a product is added the equilibrium shifts left. When cooling the system, the system will move to the right to produce more heat to restore equilibrium. The forward reaction is exothermic because heat is released. Equation 20. Which reagent(s) did you use to enhance the formation of ? Why? We used iron(III) chloride and potassium thiocyanate because these would increase the concentration of the reactants and enhance the formation of the products due to Le Chetelier’s principle 21. Indicate which ion was added to or removed from the equilibrium mixture, based on the reagent(s) you chose in question 20. Fe3+ was added to the mixture from iron(III) chloride and SCN- was added from the potassium thiocyanate.

22. Which reagent(s) did you use to enhance the formation of Fe3+(aq)? Why? AgNO3 because it will react with SCN- and remove it from the equation. Since SCN- is a reactant the equation will shift left and enhance the formation of Fe3+ 23. Indicate which ion was added to or removed from the equilibrium mixture, based on the reagent(s) you chose in question 22. The Ag+ ion was added to the the equation which reacted with SCN- 24. Upon heating in which direction is the equilibrium shifting? (L) left (R) right (N) no shift 25. Upon cooling in which direction is the equilibrium shifting? (L) left (R) right (N) no shift 26. Is the forward reaction A. endothermic B. exothermic C. insufficient info 27. Explain your answers to questions 24, 25, and 26. When the temperature of liquid is lowered, the equilibrium will shift left because it is creating more liquid water. When the liquid is heated to a higher temperature, the reaction moves faster and shifts to the right. The forward reaction would then be exothermic because heat is released to the surrounding. Consider the following reaction and situations 1 through 10. In the spaces provided, clearly indicate the best response to each situation. A. increase C. no change E. shift right B. decrease D. shift left F. cannot be determined 1. What will be the effect upon the equilibrium if the pressure on the system is increased? D 2. What will be the effect upon the concentration of CO if the concentration of H2 is decreased? A 3. What will be the effect upon the equilibrium if the concentration of H 2 is decreased? E 4. What will be the effect upon the concentration of H2O if the concentration of H 2 is increased? A

5. What will be the effect upon the equilibrium if H2 is removed and more C is added? E 6. What will be the effect upon the concentration of H2 if the amount of C is increased? A 7. What will be the effect upon the equilibrium if the temperature and the concentration of H2 increases? F 8. What will be the effect upon the concentration of CO if the temperature is increased? A 9. What will be the effect upon the equilibrium if the concentration of H2O is decreased and CO is increased? D 10. What will be the effect upon the equilibrium if a catalyst is added? C

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