DESCRIBE HOW YOU WOULD PREPARE A 0.1M OF H2S04 IN 500cm^3 flask
To prepare a 0.1M solution of H2SO4 in a 500cm^3 flask, you would need to follow the steps mentioned below:
1. Determine the amount of H2SO4 needed: To calculate the amount of solute (H2SO4) required, you need to know the molar concentration (Molarity) and the volume of the solution you want to prepare. In this case, the desired molar concentration is 0.1M, and the volume is 500cm^3.
Molarity (M) = moles of solute / volume of solution (in liters)
Rearranging the equation, moles of solute = Molarity * volume of solution (in liters)
Moles of H2SO4 = 0.1 mol/L * 0.5 L (since 500cm^3 = 0.5L)
2. Calculate the mass of H2SO4: To convert the moles of H2SO4 to grams, you need to know the molar mass of H2SO4, which is approximately 98 g/mol.
Mass of H2SO4 (in grams) = moles of H2SO4 * molar mass
Mass of H2SO4 = 0.1 mol * 98 g/mol
3. Weigh out the correct amount of H2SO4: Using a balance, measure the calculated mass of H2SO4 accurately. It is crucial to handle chemicals with caution and use appropriate safety measures.
4. Dissolve H2SO4 in distilled water: Carefully transfer the weighed amount of H2SO4 into a clean 500cm^3 flask. Add a small volume of distilled water to dissolve the H2SO4, ensuring that most of it is dissolved. Swirl the flask gently to aid the dissolution process.
5. Rinse and fill the flask to the desired volume: Rinse a small amount of distilled water into the flask containing the dissolved H2SO4 to ensure all solute is transferred. Then, fill the flask to the 500cm^3 mark using distilled water, ensuring accuracy by aligning the bottom of the meniscus with the mark.
6. Mix thoroughly: Close the flask with a stopper and mix the solution by gently inverting the flask several times to ensure uniform concentration.
Now, you have successfully prepared a 0.1M solution of H2SO4 in a 500cm^3 flask. Remember to label the flask appropriately and handle all chemicals with care.