What will be the final temperature attained if all the heat released in neutralization of 1L of 0.2 M NH4OH with 2L of 0.1M HCl increases the temperature of the final solution having density 0.95 gm/ml and specific heat capacity = 13J/gºC, if original temperature was 27ºC? Assume weak base to be completely unionized.
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NH4OH + HCl → NH4Cl + H2O
Number of mole of NH4OH = 1L × 0.2M
nNH4OH = 0.2 mole
Number of mole of HCl = 2L × 0.1 M
nHCl = 0.2 mole
Total volume of final solution = 2L + L = 3L
Mass = 0.95 × 3L × 1000 = 2850gm
total heat released = 2850 × 13J × ΔT = 37.05kJ
ΔT = 37.05 ΔT = 51.46kJ
T2 − T1 = 1.4
T2 − 300 = 1.4
T2 = 301.4k