When 50.0 cm^3 of 2.0 m hcl was added to 50.0 cm^3 of 2.0 m naoh solution in a simple calorimeter, there was a rise in temperature of 13.0°c . (assume that the specific heat capacity and density of the solution are 4.2j g^-1 k^-1 and 1.0 g cm^-3 respectively.) (a) calculate the enthalpy change of neutralization for one mole of water formed (solved : -1201.2 kj mol^-1) (b) what would be the temperature rise if 100.0 cm^3 of 2.0 m hcl were added to 100.0 cm^3 of 2.0 m naoh solution? explain your answer with the aid of calculations

Amixture initially contains a, b, and c in the following concentrations: [a] = 0.300 m , [b] = 1.05 m , and [c] = 0.550 m . the following reaction occurs and equilibrium is established: a+2b⇌c at equilibrium, [a] = 0.140 m and [c] = 0.710 m . calculate the value of the equilibrium constant, kc.

Answer asap need to be answered 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.

What is the reduction potential of a hydrogen electrode that is still at standard pressure, but has ph = 5.65 , relative to the she?