Question

1. Complete, balance, and write the net ionic equations for the following reactions: Also classify each reaction, giving its type.

Al (s) + Fe(NO₃)_2(aq) ®                                                            Type of reaction __________                             

            

Na₃PO_{4 (aq)} + Ba(NO₃)_{2 (aq)}   ®                                                    Type of reaction __________

H₂SO₃ (aq) + KOH_(aq)                ®                                                            Type of reaction __________

             NH₄Cl + NaOH              ®                                                             Type of reaction __________

2. a) What is the difference between standard solution and a primary standard?

b) What is the difference between equivalence point and end point in an acid- base titration?

When 185 mL of 0.431 M HCl at 20.48 ^oC is mixed with 215 mL of 0.431 M NaOH at 20.48 ^oC in a coffee cup calorimeter, the temperature of the mixture rises to 27.8 ^oC. What is the heat of reaction in KJ per mole of the acid? Assume the density and the specific heat of the solution are 1.02 g/ml and 4.017 J/g.^oC respectively. The heat capacity of the calorimeter is 10.0 J/^oC.

Answer 1

heat released from xxn = heat by solution & Heat gained by calorimeter daon = drott dar Here the heat lost will be negative sign where as heat gain are positive Now l = mc AT m= mass, c = specific heat DT = temperature - с ч-6ја за mass = density xvol = 1.02 g 1 me X (185+25) mL = 40 8 g DT = - = - - final initial temperature 27.8oc-20.48 7.32 °C go oso = = 408 X 4.017 X 7.32 1 1997 J 11.997 kJ Simmilary deal C.DT = heat copacity of Calorimeter 10.0's add AT= Change in temperature - 7.320 Temperature acol = ToX 7.30 = 0.0732kJ

dan I got that = 11.997 + 6 0.07 32 RJ = 12.07 ks Since it write is negative in sign we can den=-12.07 kJ Enthalphy - acid of = non -= non per mole of the heat released from the O moles of acid deen Conc X vor] – 12.07 fou1 mx 185oL 7 1ooo L=1000 F - 151.4kJ/mol