Question

2.46g of sulphuric acid present in 500ml. calculate molarity​

Answer 1

0.05 M

Explanation:

moles of H₂SO₄ = mass of H₂SO₄/molar mass of H₂SO₄

                            = 2.46/98

                            = 0.025 moles

Molarity = number of moles of solute/Volume in L

              = 0.025/0.5

              = 0.05 M

Answer 2

Answer:

2.46g of sulphuric acid present in 500ml. Molarity = 0.05M

Explanation:

Molarity is defined as the amount of substance in a certain volume of the solution. Or it can be defined as the moles of a solute per liters of a solution. To calculate molarity we need to divide the moles of solute by the volume of solution in liters.

Here we have 2.46g sulfuric acid.

Molar mass of sulfuric acid = 98.08$g/mol$

Number of moles of sulfuric acid = $\frac{2.46}{98.08}$ = 0.025 moles

Here volume of the solution is given as = 500$ml$ = 0.5$l$

Therefore, molarity of sulfuric acid = $\frac{number of moles of solute}{volume of solution in liters}$ = $\frac{0.025}{0.5}$ =0.05M