A 500 mL sample of solution of H2SO4 was titrated with 60 mL of 1.5 M KOH. What was the molarity of the H2SO4 sample?

2KOH + H2SO4 ==> 2H2O + K2SO4

mols KOH = M x L = ?
mols H2SO4 = 1/2 that number.
M H2SO4 = mols H2SO4/L H2SO4.

To determine the molarity of the H2SO4 sample, you can use the concept of stoichiometry in a titration. Here's how you can calculate it step by step:

Step 1: Write the balanced chemical equation for the reaction between H2SO4 and KOH:
H2SO4 + 2KOH → K2SO4 + 2H2O

Step 2: Determine the moles of KOH used in the titration.
To do this, you can use the following formula:
moles = concentration (M) x volume (L)

Given that the volume of KOH used is 60 mL and its concentration is 1.5 M, you can calculate the moles of KOH using the following equation:
moles of KOH = 1.5 M x 0.060 L = 0.09 moles

Step 3: Use stoichiometry to determine the moles of H2SO4.
From the balanced chemical equation, you can see that the stoichiometric ratio between H2SO4 and KOH is 1:2. Therefore, the moles of H2SO4 is twice the moles of KOH used.
moles of H2SO4 = 2 x moles of KOH = 2 x 0.09 moles = 0.18 moles

Step 4: Calculate the molarity of the H2SO4 solution.
The molarity of a solution is defined as moles of solute divided by the volume of the solution in liters.
Molarity of H2SO4 = moles of H2SO4 / volume of solution (in L)

Given that the volume of the solution is 500 mL (or 0.500 L), you can substitute the values into the formula to calculate the molarity:
Molarity of H2SO4 = 0.18 moles / 0.500 L = 0.36 M

Therefore, the molarity of the H2SO4 sample is 0.36 M.