The concentration of an H2C2O4 solution is determined by titrating it with a 0.1968 M solution of permanganate. The balanced net ionic equation for the reaction is shown below. 2 MnO4-(aq) + 5 H2C2O4(aq)+6 H3O+(aq)2 Mn2+(aq) + 10 CO2(g)+14 H2O(l) In one experiment, 24.98 mL of the 0.1968 M MnO4- the solution is required to react completely with 20.00 mL of the H2C2O4 solution. Calculate the concentration of the H2C2O4 solution.

Y=‐1x + 7 if y has a value of ‐24 what is the value of x?

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

Compare and contrast the bohr model and the electron cloud models of the atom.