Sulphuric acid is generally available in market as 18.0 M solution. How would you prepare 250 mL of 0.50 M aqueous `H_(2)SO_(4)` ?

Explanation

To prepare 250 mL of a 0.50 M aqueous solution of sulfuric acid (H₂SO₄) from an 18.0 M stock solution, we can use the dilution equation, which is represented as:

\[ M_1 V_1 = M_2 V_2 \]

Where:
- \( M_1 \) = initial molarity (18.0 M)
- \( V_1 \) = volume of the stock solution we need to find
- \( M_2 \) = final molarity (0.50 M)
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