The standard enthalpy change of solution for ammonium nitrate, NH4NO3 , is +25.7 kJ mol–1. (a) Calculate the value for the standard entropy change in the surroundings, ∆Ssurroundings , when ammonium nitrate dissolves in water at 298 K.
Include a sign and units with your answer.

(b) Explain what can be deduced from your answer in (a) about the sign and the value of the standard entropy change in the system, ∆Ssystem , when NH4NO3 dissolves.

Calculate the molarity of 48.0 ml of 6.00 m h2so4 diluted to 0.250 l .

Calculate the mass of silver needed to react with chlorine to produce 126g if silver chloride?

Part b: study of equilibrium on solubility: mg(oh)2(s) ⇌ mg2+(aq) + 2 oh–(aq) cloudy clear (pink) 7. a. b. 8. a. b. 9. 10. 11. 12. when adding concentrated hydrochloric acid, how did the appearance of the equilibrium mixture change? the change in appearance indicated a shift in the point of equilibrium. in which direction did the equilibrium shift? (l) left (r) right explain your answer to question 7a. you should indicate which ion was added to or removed from the equilibrium mixture. when adding edta, how did the appearance of the equilibrium mixture change? the change in appearance indicated a shift in the point of equilibrium. in which direction did the equilibrium shift? (l) left (r) right explain your answer to question 8a. you should indicate which ion was added to or removed from the equilibrium mixture. upon heating in which direction is the equilibrium shifting? upon cooling in which direction is the equilibrium shifting? is the forward reaction a. endothermic explain your answers to questions 9, 10, and 11. (l) left (r) right (l) left (r) right b. exothermic