Concentrated sulfuric acid is 18.4 molar and has a density of 1.84 grams per milliliter. After dilution with water to 5.20 molar the solution has a density of 1.38 grams per milliliter. This concentration of H2SO4 is often used in lead storage batteries(like a car battery).
1.Calculate the volume of concentrated H2SO4 needed to make 1.00L of 5.20 molar solution.
Is this .283L
Kevin, I worked that somewhere between here and the top of the board but I don't remember if for you or another person. If you haven't found that one, please repost your question and the top of the board and I will find the old one and give you a link.
To calculate the volume of concentrated sulfuric acid needed to make a 1.00L of 5.20 molar solution, we can use the formula:
Molarity1 x Volume1 = Molarity2 x Volume2
Where:
Molarity1 = initial molarity of sulfuric acid (18.4 M)
Volume1 = volume of concentrated sulfuric acid to be calculated (in liters)
Molarity2 = final molarity of the diluted solution (5.20 M)
Volume2 = final volume of the diluted solution (1.00 L)
Plugging in the given values, we have:
18.4 M x Volume1 = 5.20 M x 1.00 L
Now, rearrange the equation to solve for Volume1:
Volume1 = (5.20 M x 1.00 L) / 18.4 M
Volume1 = 0.283 L
So, the volume of concentrated sulfuric acid needed to make a 1.00L of 5.20 molar solution is approximately 0.283 L.