The enthalpy change when a strong acid is neutralized by strong base is - 56.1 kj/mol. if 135 ml of 0.450 m hi at 23.15°c is mixed with 145 ml of 0.500 m naoh, also at 23.15°c, what is the maximum temperature reached by the resulting solution? (assume that there is no heat loss to the container, that the specific heat of the final solution is 4.18 j/g·°c, and that the density of the final solution is that of water.)

Question

Chemistry

Aaliyah Martin

7 August, 03:52

The enthalpy change when a strong acid is neutralized by strong base is - 56.1 kj/mol. if 135 ml of 0.450 m hi at 23.15°c is mixed with 145 ml of 0.500 m naoh, also at 23.15°c, what is the maximum temperature reached by the resulting solution? (assume that there is no heat loss to the container, that the specific heat of the final solution is 4.18 j/g·°c, and that the density of the final solution is that of water.)

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Answers (1)

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Judith Lucero · Answer 1

First, we have to get the moles of HI = molarity * volume L

= 0.45 m * 0.135 L

= 0.06075 moles

then the moles of NaOH = molarity * volume L

= 0.5 m * 0.145 L

= 0.0725 moles

when we have the reaction equation is:

HI + NaOH → H2O + NaI

and HI is the limiting reactant

when Q = molar enthalpy change * moles HI

= 56100 j / mol * 0.06075 mol

= 3408 j

when Q = M * Cp * ΔT

M is the mass & Cp is the specific heat & ΔT is difference in temperature

we need to get the mass (m), when the total volume = 135 ml + 145 ml

=280 ml

∴ Mass (m) = volume * density

= 280 * 1 = 280 g

so by substitution:

3408 = 280 g * 4.18 * ΔT

∴ΔT = 2.9 °C

∴ (Tf - Ti) = 2.9 °C

when Ti = 23.15°C

∴Tf = 23.15 + 2.9

= 26.05 °C