This experiment involves assessing the alkalinity of a water sample by titrating it with a standard acid solution. Alkalinity is a measure of water's capacity to neutralize acids, which is crucial for maintaining pH stability in various applications.
Ensure that the titration is done slowly near the endpoint to avoid overshooting, which could lead to inaccurate results.
This experiment determines the hardness of a water sample using EDTA as a complexing agent. Hardness is caused by calcium and magnesium ions, which can affect water quality and industrial applications.
Ensure the pH is correctly adjusted as the EDTA titration is pH-sensitive.
This experiment focuses on determining the percentage composition of sodium hydroxide (NaOH) in a mixture with sodium chloride by titration against a standard acid.
Use a pH indicator like phenolphthalein to identify the endpoint accurately.
This experiment determines the amounts of oxalic acid and sulfuric acid in a solution by titration with standard solutions of sodium hydroxide and potassium permanganate.
Handle potassium permanganate with care as it is a strong oxidizing agent.
This experiment measures the copper content in a copper ore solution by iodometric titration, where iodine reacts with copper ions to determine its concentration.
Ensure all solutions are freshly prepared for accurate results.
This experiment measures the concentration of chloride ions in a water sample through precipitation with silver nitrate, forming a visible precipitate of silver chloride.
1. Add potassium chromate indicator to the water sample.
2. Titrate with silver nitrate until a persistent reddish-brown precipitate appears, indicating the endpoint.
- Ensure accurate addition of potassium chromate for consistent results.
- The endpoint is sensitive to pH, so maintain a neutral pH for reliable results.
This experiment calculates the concentration of magnesium sulfate in solution through titration with EDTA, a common complexing agent that binds to metal ions.
1. Add an appropriate buffer to maintain pH.
2. Use Eriochrome Black T as an indicator.
3. Titrate with EDTA until the color changes, indicating all magnesium ions have reacted.
- Ensure pH is stable for accurate EDTA binding.
- The endpoint color change can be subtle; observe carefully.
This experiment measures the surface tension of a liquid by counting the number of drops required to release a specific volume, which correlates to the liquid's cohesive forces.
1. Use a burette to release drops of the liquid.
2. Count the drops necessary to reach a specific volume.
3. Calculate surface tension based on the drop count and volume.
- Temperature affects surface tension, so perform the experiment at room temperature.
- Maintain consistent drop sizes for accurate results.
Viscosity, or the resistance of a liquid to flow, is determined by allowing a liquid to flow through a capillary tube and measuring the time taken.
1. Measure the density of the liquid.
2. Fill a viscometer with the liquid.
3. Record the flow time between two marks.
4. Use density and time to calculate viscosity.
- Ensure the viscometer is clean for accurate readings.
- Avoid air bubbles in the liquid column.
This experiment determines the cell constant for a conductivity cell and uses it to measure conductometric titration between strong acid and base.
1. Calibrate the cell using a standard KCl solution.
2. Titrate the acid and base, recording conductivity changes.
3. Determine cell constant and equivalence point.
- Accurate calibration is essential for reliable results.
- Clean electrodes between uses to maintain conductivity accuracy.