Question

When 35.0 mL of 1.43 M NaOH at 22.0 degres Celsius is neutralized by 35.0 mL of HCL also at 22.0 degrees Celsius in a coffee-cup calorimeter, the temperature of the final solution rises to 31.29 degrees Celsius. Assume that the specific heat of all solutions i 4.18 J/ g* C, that the density of all solutions is 1.00 g/mL, and that volumes are additive.

A) calculate q for the reaction.
B) calculate q for the neautralization of one mole of NaOH.

i understand the calorimeter equation, but with that molarity in the equation, i got thrown off. help please.

Answer 1

A.
q = mass water x specific heat water x delta T = heat evolved by the neutralization of HCl with NaOH.

B. The above is q for how many moles? moles = L x M = 0.035L x 1.43 M = xx
Then q/xxmoles = joules/mole

Answer 2

Thank you!