Question

What is the molarity of a 1.378 solution made using 12.8 mL 18M H2SO4?

Answer 1

The molarity of the 1.378 solution made using 12.8 mL 18M H2SO4 is 17.99 M.

Step-by-step explanation:

The molarity of a solution is defined as the number of moles of solute dissolved in one liter of solution. To calculate the molarity, we first need to determine the number of moles of H2SO4 in the solution. We can use the formula:

Molarity (M) = moles of solute / volume of solution (L)

Given that the solution was made using 12.8 mL of 18M H2SO4, we can calculate the moles of H2SO4 as follows:

1. Convert the volume of solution from milliliters to liters: 12.8 mL = 0.0128 L
2. Calculate the moles of H2SO4 given its molarity: 18 M * 0.0128 L = 0.2304 moles

Now, we can calculate the molarity:

Molarity (M) = 0.2304 moles / 0.0128 L = 17.99 M