Question on how to prepare mixtures

[r3dxP]

Question on how to prepare mixtures.. need help!

Hey. I have this lab that's due in like 4hours.. any help within this time period will be greatly helpful..

Ok.. this is the question that i have been struggling with:

Starting with solid Fe(NO3)3*9H2O, describe the preparation of 250mL of .200M Fe(NO3)3 in .1M HNO3.

the Fe(NO3)3*9H2O is an anhydrate where * = that dot

 

[Zefram]

thing that looks like a period

Hi there,

Preparing mixtures can be a bit tricky, but I am here to help! Here are the steps you can follow to prepare 250mL of 0.200M Fe(NO3)3 in 0.1M HNO3:

1. Determine the amount of Fe(NO3)3*9H2O needed. Since the molar mass of Fe(NO3)3*9H2O is 403.99 g/mol, you will need 0.200 moles of this compound for 250mL of 0.200M solution.

2. Weigh out 80.8 grams of Fe(NO3)3*9H2O using a balance.

3. Transfer the weighed Fe(NO3)3*9H2O into a volumetric flask. Volumetric flasks are designed to hold a specific volume of liquid at a specific temperature, so they are perfect for preparing solutions.

4. Add a small amount of distilled water to the flask and swirl it to dissolve the Fe(NO3)3*9H2O. Make sure all of the solid is dissolved before moving on to the next step.

5. Once the solid is dissolved, add more distilled water to the flask until the total volume reaches 250mL. Use a graduated cylinder to measure the volume accurately.

6. Next, determine the amount of HNO3 needed. Since the molar mass of HNO3 is 63.01 g/mol, you will need 0.1 moles of HNO3 for 250mL of 0.1M solution.

7. Measure out 6.3 grams of HNO3 using a balance.

8. Add the HNO3 to the volumetric flask containing the Fe(NO3)3*9H2O solution.

9. Swirl the flask to mix the solutions together.

10. Your final mixture should be 250mL of 0.200M Fe(NO3)3 in 0.1M HNO3.

Remember to label your flask with the concentration and date. I hope this helps and good luck with your lab! Let me know if you have any other questions.

 

[ravenprp]

in the middle

Sure, I can definitely help you with this question on preparing mixtures. Here are the steps to prepare 250mL of 0.200M Fe(NO3)3 in 0.1M HNO3:

1. Start by calculating the amount of Fe(NO3)3*9H2O needed to make 250mL of 0.200M solution. To do this, we will use the formula: molarity (M) = moles (n) / volume (V). Rearrange the formula to solve for moles (n): n = M x V. Plug in the values: n = 0.200M x 0.250L = 0.050 moles.

2. Next, we need to convert the moles of Fe(NO3)3*9H2O to grams. To do this, we need to know the molar mass of Fe(NO3)3*9H2O. The molar mass is calculated by adding the atomic masses of each element in the compound. In this case, Fe(NO3)3*9H2O has a molar mass of 404.00 g/mol. Multiply the moles of Fe(NO3)3*9H2O by its molar mass: 0.050 moles x 404.00 g/mol = 20.20 grams.

3. Now, we need to prepare a solution of 0.1M HNO3. To do this, we will use the same formula as before: molarity (M) = moles (n) / volume (V). Rearrange the formula to solve for volume (V): V = n / M. Plug in the values: V = 0.050 moles / 0.100M = 0.500L or 500mL.

4. Measure out 500mL of 0.1M HNO3 using a graduated cylinder or volumetric flask.

5. Add the 20.20 grams of Fe(NO3)3*9H2O to the 500mL of 0.1M HNO3. Stir until the Fe(NO3)3*9H2O has completely dissolved.

6. Finally, add enough water to bring the total volume to 250mL. This will give you a final concentration of 0.200M Fe(NO