The heat of neutralization, ΔHneut, can be defined as the amount of heat released (or absorbed), q, per mole of acid (or base) neutralized. ΔHneut for nitric acid is –52 kJ/mol HNO3. At 27.3°C, 50.00 mL of 0.743M HNO3 is neutralized by 1.00 M Sr(OH)2 in a coffee-cup calorimeter.
(a) How many mL of Sr(OH)2 were used in the neutralization?
(b) What is the final temperature of the resulting solution? (Use the assumptions in Question 11.)
Reference Question 11:
When 35.0 mL of 1.43 M NaOH at 22.0°C are neutralized by 35.0 mL of HCl also at 22.0°C in a coffee-cup calorimeter, the temperature of the final solution rises to 31.29°C. Assume that the specific heat of all solutions is 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 neutralization of one mole of NaOH.
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