22.3 mL of the standard barium hydroxide solution was combined with 20.0 ml of t

Question

22.3 mL of the standard barium hydroxide solution was combined with 20.0 ml of the nitric acid in Question 19 part (b) in a constant pressure calorimeter. The initial temperature of the solutions was 22.0 degree C. Use the enthalpy of reaction calculated in Question 19 part (c) to determine the final temperature of the solution, assuming the volumes are additive, the density of the final solution is 1.00 g/cm^3, and the specific heat of the solution is 4.18 J/g- degree C. (Use Delta H_rxn = -100.0 kJ/mol Ba(OH)_2 if you do not have an answer in Question 19 part (c))

Explanation / Answer

Volume of mixture = 20+22.3= 42.3ml

Assumed molarity of Ba(OH)2= 1

moles of Ba(OH)2 in 22,3ml =22.3/1000 moles=0.0223

density of solution = 1 g/cc, mass of solution= 42.3*1= 42.3 gm

enthalpy change= 100*1000 *0.0223 J= 42.3*4.184*(T-22)

T-22= 12.6, T= 34.6 deg.c

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