# Enthalpy Of Solution Lab Report Assessed on: * Data Collection and Processing (DCP) * Conclusion and Evaluation (CE)

Essay by TheKamelRiderHigh School, 11th gradeB+, March 2009

Usman Omid Chemistry IB 1A

Enthalpy Of Solution

Introduction

Aim

The aim of this investigation was to determine the enthalpy of the solution created when dissolving Sodium Hydroxide (NaOH) in water (H2O).

Theory

When a solid ionic compound is dissolved in water a change of enthalpy is involved. The enthalpy of a solution, ÃÂHsol is the enthalpy change when one mole of the substance is dissolved in water to form aqueous solution. Ã¯Â¿Â½

Chemical

Sodium Hydroxide (NaOH)

Procedure

The recommended amount of compound ito use is around 0.1 moles.

Add the solid salt and stir the mixture thoroughly and continuously.

Calculate ÃÂHsol. Ignore the heat capacity of the caleriometer.

Results

Raw Data

Tab.1. The different data required for the calculations.

 Trial Mass of NaOH / g (ÃÂ± 0.001 g) Volume of H2O / ml (ÃÂ± 1 ml) Initial Temperature / ÃÂ°C (ÃÂ± 1 ÃÂ°C) Final Temperature / ÃÂ°C (ÃÂ± 1 ÃÂ°C) 1 3.954 50 19 39 2 4.027 70 19 33 3 3.991 80 19 31 4 3.988 100 19 28

One qualitative data that might have affected the results is that the Sodium Hydroxide (NaOH) seemed to start a slow melting process as soon as it left its container.

This was a qualified guess based on that it started to sparkle and looked like it was melting.

Another one that probably did affect the results was the fact that the containers in which we mixed the water (H2O) and Sodium Hydroxide (NaOH) in had holes. And this increases the energy lost to the surroundings in the form of heat, which affects the temperature. Ã¯Â¿Â½

Processed Data

Calculations

Theory states:

ÃÂH= -Q/n

Q = m * c * ÃÂT Ã¯Â¿Â½

Where in this case m =...