how would you prepare 1.00 L of a .50M solution of H2SO4 from concentrated (18M) sulfric acid?
Note: concentrated sulphuric acid is very corrosive and must be handled with care, taking all protective measures as required.
The quantity of concentrated sulphuric acid (18N) required to make 1 l. of 0.5N diluted acid is 1000 ml. *0.5/18=27.78 ml.
Fill a 1 litre volumetric flask to between 600 and 700 ml. with distilled water. Gradually add the measured quantity of concentrated sulphuric acid while swirling to ensure a good mixture, and the dissipation of heat generated. Continue swirling for a minute after all acid has been added.
Let liquid stand until content is cooled to room temperature.
Add distilled water to about 1/2" below mark and homogenize contents with stopper closed. Top up to mark with distilled water and homogenize again.
The solution is now ready for use. (approximately 0.5N).
All concentrations above should have been expressed in M (and not N).
Oh, it's time to get funky with some chemistry! To prepare 1.00 L of a 0.50 M solution of H2SO4, you'll need to be a real sulfuric acid superstar. Now, buckle up and let's break it down!
First, we need to figure out the volume of concentrated sulfuric acid you'll need to dilute. We can use the handy equation:
(M1)(V1) = (M2)(V2)
Where M1 is the concentration of the concentrated sulfuric acid (18 M), V1 is the volume of the concentrated acid we want to find, M2 is the desired concentration (0.50 M), and V2 is the final volume (1.00 L).
Plug in the numbers, and we get:
(18 M)(V1) = (0.50 M)(1.00 L)
Now, let's solve for V1:
V1 = (0.50 M)(1.00 L) / (18 M)
V1 ≈ 0.028 L
So, you'll need approximately 0.028 liters (or 28 milliliters) of concentrated sulfuric acid. Now, make sure you handle it with care and safety!
Next, you want to add this volume of concentrated sulfuric acid to a container (like a beaker or flask) with some distilled water. With gentle stirring, slowly add the concentrated acid to the water. Remember, NEVER add water to concentrated acid—it can get explosively excited!
Once you've added the concentrated acid, continue stirring until you've reached the desired final volume, which is 1.00 L.
Congratulations, my chemically inclined friend! You've successfully prepared your 0.50 M solution of H2SO4, all while keeping your lab intact. Enjoy your solution, but remember: don't drink it!
To prepare a 1.00 L of a 0.50 M solution of H2SO4 from concentrated (18M) sulfuric acid, you can use the concept of dilution. Here's how you can calculate the amounts needed:
1. Determine the amount of concentrated sulfuric acid needed:
Since the concentrated sulfuric acid is given as 18 M, we can use the equation M1V1 = M2V2 to calculate the volume of concentrated sulfuric acid required.
M1 is the initial concentration (18 M), V1 is the initial volume (unknown), M2 is the final concentration (0.50 M), and V2 is the final volume (1.00 L).
Rearranging the equation, we get:
V1 = (M2 * V2) / M1
Plugging in the values, we have:
V1 = (0.50 M * 1.00 L) / 18 M
V1 ≈ 0.0278 L or 27.8 mL
Therefore, you will need approximately 27.8 mL of the concentrated sulfuric acid.
2. Add distilled water to reach the final volume:
After measuring out the required amount of concentrated sulfuric acid, you can transfer it to a container and slowly add distilled water while stirring. Continue adding water until the final volume of the solution reaches 1.00 L.
It's essential to add the water slowly and cautiously as concentrated sulfuric acid is highly corrosive and can cause severe burns. Always wear appropriate protective equipment when dealing with concentrated acids.
By following these steps, you should be able to prepare a 1.00 L of a 0.50 M solution of H2SO4 from concentrated (18M) sulfuric acid.