When 50.0 mL of 0.400 mol L-2 Ca(NO3)2 is added to 50.0 mL of 0.800 mol L NaF.
CaF2 precipitates, as shown in the net ionic equation below. The initial temperature of both
solutions is 24.0 °C. Assuming that the reaction goes to completion, and that the resulting solution
has a mass of 100.00 g and a specific heat of 4.18 J gilºc 1, calculate the final temperature of the
solution.
Ca2+(aq) + 2F (ag) - Cafz(s) 4, H = -11.5 kJ

Answer asap need by wednesday morning explain how a buffer works, using an ethanoic acid/sodium ethanoate system including how the system resists changes in ph upon addition of a small amount of base and upon addition of a small amount of acid respectively. include the following calculations in your i. calculate the ph of a solution made by mixing 25cm3 0.1m ch3cooh and 40cm3 0.1m ch3coo-na+. [ka = 1.74 x 10-5 m] ii. calculate the ph following the addition of a 10cm3 portion of 0.08 m naoh to 500cm3 of this buffer solution. iii. calculate the ph following the addition of a 10cm3 portion of 0.08 m hcl to 200cm3 of the original buffer solution.