How much 35.6 M H2SO4 is needed to make a 1 L solution that is .007 ppm? Not sure how to convert from M to ppm-is there a formula?
.007 ppm. That is a very slight concentration, so you can safely assume one liter of solution has a mass of 1000grams.
So, to get .007 ppm in a million grams of solution, you need .007 grams of sulfuric acid, so in a liter (1000 grams) you need : 7E-6grams of acid.
7E-6grams=35.6*molmassAcid*Volumeneeded
volumeneeded=7E-6/(35.6*98)=2E-9liters=
= 2E-6ml
As shockingly small as this seems, remember that Acid Rain is about .01ppm.
Check my calculations.
To convert from molarity (M) to parts per million (ppm), you need to know the molar mass of the compound. In this case, the molar mass of H2SO4 is:
Molar mass of H2SO4 = (2 * atomic mass of H) + (1 * atomic mass of S) + (4 * atomic mass of O)
= (2 * 1.008) + (1 * 32.06) + (4 * 16.00)
= 98.09 g/mol
Now, let's calculate the amount of 35.6 M H2SO4 required to make a 1 L solution with a concentration of 0.007 ppm:
Step 1: Convert 0.007 ppm to grams per liter (g/L).
0.007 ppm = 0.007 g/10^6 L
Step 2: Convert grams to moles.
0.007 g × (1 mol/98.09 g) ≈ 7.14 × 10^-5 mol
Step 3: Calculate the volume of the 35.6 M H2SO4 needed using the molarity formula.
Volume (L) = moles (mol) / Molarity (M)
Volume (L) = 7.14 × 10^-5 mol / 35.6 M
≈ 2.01 × 10^-6 L
≈ 2 μL (microliters)
Therefore, you would need approximately 2 μL of 35.6 M H2SO4 to make a 1 L solution with a concentration of 0.007 ppm.