Consider the reaction below: (Question 16) CaBr2(aq) + 2 AgNO3(aq) ----> Compound A + Compound B (OR C a Br2(a q) + "2" A g N O3(a q) right arrow Compound A + Compound B) One of the the single ions that would be used to form compound A or compound B would be ____. Question 16 answer choice options: Br43- (OR Br4 3 minus) Br42- (OR Br4 2 minus) Br23- (OR Br2 3 minus) Br33- (OR Br3 3 minus) BrO23- (OR Br O2 3 minus) Br3- (OR Br 3 minus) Br32- (OR Br3 2 minus) Br3- (OR Br3 1 minus) BrO2- (OR Br O2 1 minus) Br2- (OR Br 2 minus) Br22- (OR Br2 2 minus) Br- (OR Br minus) Br4- (OR Br4 1 minus) Br44- (OR Br4 4 minus) Br2- (OR Br2 1 minus)

Q18

Which of these is an acid-base reaction? Fe2+ (aq) + 2 OH- (aq) ® Fe(OH)2 (s) Fe (s) + 2 Fe3+ (aq) ® 3 Fe2+ (aq)  NH3 (aq) + HNO3 (aq) ® NH4NO3 (aq) BaCl2 (aq) + K2SO4 (aq) ® BaSO4 (s) + 2KCl (aq) H2 (g) + Cl2 (g) ® 2 HCl (g)

Question 5 (1 point) Equimolar quantities of potassium fluoride and hydrofluoric acid are placed into solution. The equilibrium established is as follows: HF(aq) + H2O(l) F¯(aq) + H30+(aq) What happens to the above equilibrium if some acetic acid is added to the solution? Acetic acid ionizes so pH significantly increases. Acetic acid isn't in the equilbrium equation so it will have no effect on the pH of the solution. The acetic acid creates more hydronium ion so the equlibrium shifts left and pH is not changed significantly. The acetic acid creates more hydronium ion so the reaction shifts right and pH is not changed significantly.