What is the molarity of H2SO4 in a solution prepared by adding 15.0 mL of 6.0 Molarity H2S04 to enough water to make 100.0 mL of solution?

There are two easy ways to do this.

1. mL1 x M1 = mL2 x M2 and solve for the new molarity OR
2. 6.0 x (15.0/100.0) = ?

C1V1=C2V2

6*0.015=C2*0.1

..a bit of transposition
(0.015*6)/0.1=C2
C2= 0.9

To find the molarity of the solution, you need to use the formula:

Molarity (M) = moles of solute / volume of solution in liters

Let's break down the process step by step:

Step 1: Calculate the moles of H2SO4.
To do this, you need to know the volume and molarity of the solute. In this case, the volume of H2SO4 is given as 15.0 mL, and the molarity is 6.0 M.

Moles of H2SO4 = volume (in liters) × molarity
= 15.0 mL × (1 L / 1000 mL) × 6.0 M
= 0.09 moles

Step 2: Calculate the volume of the solution in liters.
The total volume of the solution is given as 100.0 mL.

Volume of solution = 100.0 mL × (1 L / 1000 mL)
= 0.1 L

Step 3: Calculate the molarity of the solution.
Now that you have the moles of H2SO4 (0.09 moles) and the volume of the solution (0.1 L), you can use the formula:

Molarity = moles of solute / volume of solution in liters

Molarity = 0.09 moles / 0.1 L
= 0.9 M

So, the molarity of the H2SO4 solution is 0.9 M.