how to prepare 1 L of 2.5M nitric acid from 69% of concentrated nitric acid?
Do you know the density.
1000 x density(g/mL) x 0.69 x (1/63) = ?M = approx 14M but you need that more accurate than that.
Then mL1 x M1 = mL2 x M2
1000 x 2.5M = mL2 x approx 14
Solve for mL2, add that amount to a 1L volumetric flask, make to the mark, stopper, share thoroughly.
To prepare 1 L of 2.5M nitric acid from 69% concentrated nitric acid, you'll need to calculate the volume of concentrated nitric acid required and then dilute it to the desired concentration. Here's how you can do it:
Step 1: Determine the amount of nitric acid needed.
The molarity (M) of a solution is defined as the number of moles of solute divided by the volume of the solution in liters. So, to calculate the volume of the concentrated nitric acid needed, use the formula:
M1 x V1 = M2 x V2
Where:
M1 = initial molarity of the concentrated nitric acid (69% concentration)
V1 = volume of concentrated nitric acid needed (unknown)
M2 = desired molarity of the final solution (2.5M)
V2 = final volume of the solution (1 L)
Substituting the values into the formula:
(0.69 M) x V1 = (2.5 M) x (1 L)
Simplifying the equation:
0.69 V1 = 2.5
Dividing both sides by 0.69:
V1 ≈ 3.62 L
So, you will need approximately 3.62 liters of concentrated nitric acid for this dilution.
Step 2: Dilute the concentrated nitric acid with water.
To prepare the desired 1 L of 2.5M nitric acid, take 3.62 L of the 69% concentrated nitric acid and dilute it with distilled water until the final volume reaches 1 L.
It's important to remember to always add concentrated acid to water slowly to avoid splashing or spattering. So, fill a 1L container with about 800 mL of water and while stirring, slowly add the calculated volume (3.62 L) of concentrated nitric acid. Then, continue stirring while adding water until the final volume reaches 1 L.
Finally, you will have prepared 1 L of 2.5M nitric acid from 69% concentrated nitric acid.