Question

A student determined the heat of neutralization of sulfuric acid mixed with sodium hydroxide solution using the procedure described in this experiment. 35.0 mL of 1.00 M H2SO4 were added to 70.5 mL of 1.00 M NaOH solution.

1)Calculate the mass of the reaction mixture. Assume that the density of the mixture is 1.03 g/mL.

_______g/mL

2)Calculate the number of moles of each reagent that are consumed when the solutions are mixed. Record your responses using decimal notation rather than scientific notation.

_______moles H2SO4

_______moles NaOH

3)If ΔT is 7.83oC, calculate the heat transferred from the reaction (i.e., q). Assume that the specific heat of the mixture is 3.89 J g-1 deg-1.

_______J

Answer 1

1) total volume of mixture = 35ml + 70.5 ml = 105.5ml

mass = density volume

= 1.03 105.5 = 108.665 gm

mass of the reaction mixture = 108.665 gm

2) 35 ml = 0.035 L

no. of mole = molarity volume of solution in liter

= 1.00 0.035 = 0.035 mole

0.035 mole of H₂SO₄

70.5 ml = 0.0705 L

no. of mole = molarity volume of solution in liter

= 1.00 0.0705 = 0.0705 mole

0.0705 mole of NaOH

3) q = mass specific heat ΔT

q = 108.665 3.89 7.83 = 3309.7946 J

heat transferred from the reaction = 3309.7946 J