Question

Equal volumes, 50.0 mL, of 0.54897 M solution of HCl and 0.9573 M NaOH solutions having an initial temperature of 18.5 °C react in a coffee-cup calorimeter. The resultant solution records a temperature of 22.9 °C. Since the solutions are mostly water, the solutions are assumed to have a density of 1.0 g/mL and a specific heat of 4.184 J/g °C. The heat capacity of the calorimeter is 1.0 x 101 J/°C.

Answer 1

Given:

V₁ = 50mL = V₂

T₀ = 18.5°C

Tf = 22.9°C

Density = 1.0g/mL

c_solution = 4.184J/g°C

c_calorimeter = 1.0 x 10¹J/°C

To find:

Heat released by the solution.

Solution:

Heat released by the solution

H = M_solution × c_solution × ΔT + c_calorimeter + ΔT

H = [(50 + 50) × 1.0] × 4.184 × (22.9 - 18.5) + 1.0 × 10¹ × (22.9 - 18.5)

H = 100 × 4.184 × 4.4 + 1.0 × 10¹ × 4.4

H = 1840.96 + 44

H = 1884.96J

H ≈ 1885J

Therefore, heat released by the solution is 1885J.