How would you prepare 50.0 mL of 2.0 M H2SO4 starting with concentrated sulfuric acid (18M)?
c1v1 = c2v2
c = concn
v = volume
50 x 2.0 = x*18
solve for x
Take x mL of 18 M H2SO4, transfer quantitatively to a 50 mL volumetric flask and add water (deionized or distilled of course) to the mark on the volumetric flask. Stopper and mix thoroughly.
To prepare 50.0 mL of 2.0 M H2SO4 starting with concentrated sulfuric acid (18 M), you will need to dilute the concentrated sulfuric acid with water.
Here's a step-by-step procedure to prepare the solution:
1. Determine the amount of concentrated sulfuric acid needed:
- The desired concentration is 2.0 M.
- The desired volume is 50.0 mL.
- Use the formula: C1V1 = C2V2, where C1 and V1 are the initial concentration and volume, and C2 and V2 are the final concentration and volume.
- Plug in the values into the formula: (18 M)(V1) = (2.0 M)(50.0 mL).
- Solve for V1: V1 = (2.0 M)(50.0 mL) / 18 M. Calculate the value of V1, which should be 11.11 mL.
2. Measure 11.11 mL of concentrated sulfuric acid using a graduated cylinder or a volumetric pipette.
3. Pour the measured concentrated sulfuric acid into a clean and dry container.
4. Add distilled water to the container to make the total volume up to 50.0 mL. Be cautious while adding water and mix gently to avoid splashing or excessive heat generation.
5. Mix the solution well by stirring it gently to ensure the sulfuric acid is thoroughly mixed with the water.
6. The resulting solution is now 50.0 mL of 2.0 M H2SO4.
Remember to always exercise caution when working with concentrated sulfuric acid, as it is a corrosive substance. Wear appropriate personal protective equipment, such as gloves and safety glasses, and work in a well-ventilated area.
To prepare 50.0 mL of a 2.0 M solution of H2SO4 starting with concentrated sulfuric acid (18 M), you can use the concept of dilution. Dilution involves adding a certain amount of concentrated solution to a solvent to achieve the desired concentration.
Here's the step-by-step process to prepare the solution:
1. Determine the volume of concentrated H2SO4 needed:
To calculate the volume of concentrated sulfuric acid needed, you can use the equation:
M1V1 = M2V2
Where M1 is the initial concentration, V1 is the initial volume, M2 is the final concentration, and V2 is the final volume.
In this case, the initial concentration (M1) is 18 M, the final concentration (M2) is 2.0 M, and the final volume (V2) is 50.0 mL. Rearranging the equation to solve for V1 gives you:
V1 = (M2 * V2) / M1
Plugging in the values, you get:
V1 = (2.0 M * 50.0 mL) / 18 M = 5.56 mL
Therefore, you will need 5.56 mL of concentrated sulfuric acid.
2. Measure the concentrated sulfuric acid:
Use a pipette or a measuring cylinder to accurately measure 5.56 mL of the concentrated sulfuric acid.
3. Transfer the measured acid to a container:
Carefully transfer the measured amount of concentrated sulfuric acid to a container that can hold more than 50.0 mL.
4. Add the solvent (water) to the container:
Slowly add distilled water to the container while stirring until the total volume reaches 50.0 mL. Ensure that the solution is well-mixed.
5. Verify the final concentration:
To verify the final concentration, you can use a pH meter or acid-base titration. If using a pH meter, the pH should be around 0.3. If using titration, perform a neutralization reaction with a known concentration of a base (e.g., NaOH) and calculate the concentration of H2SO4 based on the volume of base consumed.
Remember to handle concentrated sulfuric acid with extreme caution. It is highly corrosive, and appropriate protective measures and equipment should be used.