Precipitation of Lead Salts -Chem IA

You can explore the enthalpy of precipitation of Lead salts for the chemistry internal assessment. This can be a good IA based on hands-on experiment. In this IA you need to explore the precipitation of different lead salts like lead sulphate, lead halides, lead hydroxide . You can measure the enthalpy change during the precipitation of each lead salts and explore them.
Investigating The Enthalpy Change During The Precipitation of Lead Salts – DP Chem IA
Investigating the enthalpy change associated with precipitation of lead salts is a fascinating topic for an IB DP Chemistry IA. In this article, you’ll learn everything from the preparation and research aspects to accurately calculate enthalpy changes during precipitation of lead salts. Step-by-step guidance included!

Research the Purpose of the IA and Gather Necessary Materials.
Before beginning the IA, it’s important to carefully research the purpose of investigation and gather all necessary materials for the experiment. To measure enthalpy change during precipitation of lead salts, you will need a LabTech Thermal Analysis System (LTST), compound thermometer, 25ml and 50ml measuring cylinders, a beaker, lead (II) sulphate solution and calcium chloride solution, filter paper/ funnel/ glass rod, Bunsen burner, hot plate or electric plate. Additionally, you’ll need your reference materials; including safety data sheets for both chemicals being used.

Prepare Solutions and a note book detailing the procedure and observations made throughout the experiment.
To begin, prepare solutions of lead (II) sulphate and calcium chloride in the desired molarities. Dilute to approximately 25 mL volume for each solution and label both. Next, create a note book detailing the procedure and observations made throughout the experiment. This should include detailed descriptions about the set up ofeach trial (volume of each solution, equipment used, temperatures worn by each part etc).Also note down any control experiments run such as adding different concentrations at different amounts. Additionally, record any values obtained while measuring enthalpy change during precipitation; noting time intervals, range and new readings.

Obtain accurate measurements of mass and temperature at important steps during the experiment.
To measure enthalpy change, the mass and temperatures of the lead (II) sulphate solution and calcium chloride solution must be conducted at different stages. Take accurate measurements for each trial. Calculate mass by measuring out a desired amount of each substance used in the experiment and tare the container before measuring out what is neeeded. Additionally, obtain accurate temperature measurements through thermometers set up immediately next to where each substance enters the calorimeter cup. Be sure to take multiple readings at specific intervals to gain an accurate average of tempeature throughout the experiment.

Calculate enthalpy changes between reactants and products, taking into account any phase transitions that occurred in the reaction.
To calculate the enthalpy change during precipitation of lead salts, you must measure the difference in energy between reactants and products, taking into account any phase transitions that occurred in the reaction. Use mass and temperature measurements to calculate q, or the energy exchanged between the system and its surroundings. Then use Enthalpy Change Formula (H=q/m) to determine ΔH. Compare your calculated value with expected enthalpy values from theoretical sources to evaluate accuracy of experiment results.

Reach conclusions based on results obtained during the investigation, including possible explanations for discrepancies if there are any, as well as applications to real-world scenarios of precipitation reactions.
After analyzing the results from your investigation, you should be able to reach conclusions about the enthalpy change during the precipitation of lead salts. Compare your calculated value of ΔH to theoretical sources, and consider possible explanations for any discrepancies between values. Discuss possible applications of these findings in a real-world scenario — for example, how this knowledge could be used to improve production processes or environmental conditions.

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