This is confusing.
I am supposed to explain how to prepare a solution using the proper lab equipment (both from dry solid and a stock solution)
Help would greatly be appreciated...
It's confusing to me, too, since you provided few, if any, details. In general, you prepare a 1 M solution by placing 1 mole of the solid in a 1 liter volumetric flask, dissolve in a small amount of water, then make to the final mark of the flask with water.
Yeah I know...sorry, but that's all the information I was given
Thank you for your answer.
But what exactly do you mean by "then make to the final mark of the flask with water." ?
Preparing a solution in a lab can seem confusing at first, but with the right guidance, it becomes easier. Here's a step-by-step explanation of how to prepare a solution using dry solid and a stock solution:
1. Determine the amount and concentration of the solution you need to prepare. This information is usually provided in the experiment or experiment protocol.
2. Start with a dry solid: If you need to prepare a solution from a dry solid, you need to weigh the appropriate amount of the solid. Use a balance to measure the required mass accurately. Make sure to use a container (such as a weighing boat or paper) to prevent contamination.
3. Dissolve the solid: Add the weighed solid into a clean and dry container, such as a beaker or a flask. Then, add a small amount of solvent (usually water) to start the dissolution process. Stir the mixture using a stirring rod until the solid is completely dissolved. If necessary, you can gently heat the solution to speed up the dissolution process.
4. Make up the volume: Once the solid is fully dissolved, add more solvent (water in most cases) to make up the total desired volume of the solution. Use a graduated cylinder or a volumetric flask to accurately measure the final volume. Make sure to measure at eye level to avoid parallax errors.
5. Mix thoroughly: Use a stirring rod or a magnetic stirrer to mix the solution thoroughly. This ensures that the components are evenly distributed.
6. Adjust the concentration: If the initial concentration of the solution is different from the desired concentration, you might need to dilute or concentrate the solution. Dilution involves adding more solvent to decrease the concentration, while concentration involves evaporating or adding more solute to increase the concentration. Use the appropriate calculations to determine the necessary adjustments.
7. Label and store: Label the container with the name, concentration, and any other relevant information about the solution. Store the solution in a properly labeled and sealed container, preferably away from direct sunlight or heat sources.
Using a stock solution (previously prepared concentrated solution):
1. Determine the amount and concentration of the solution required, as mentioned before.
2. Calculate the volume of the stock solution needed. Use the following formula for dilution calculations: C1V1 = C2V2, where C1 is the concentration of the stock solution, V1 is the volume of the stock solution needed, C2 is the desired concentration, and V2 is the final volume of the solution.
3. Measure and transfer the calculated volume of the stock solution into a clean and dry container.
4. Make up the volume by adding the appropriate amount of solvent (usually water). Measure the final volume accurately using a graduated cylinder or a volumetric flask.
5. Mix thoroughly to ensure complete mixing of the stock solution and the solvent.
6. Conduct any necessary concentration adjustments, if required, using the methods explained earlier.
7. Label and store the solution as before.
Remember to always wear appropriate personal protective equipment (PPE), such as gloves and safety goggles, and consult your lab supervisor or instructor for any specific guidelines or safety precautions.