Perchloric acid behaves as an acid, even when it is dissolved in sulfuric acid.

1. (a) Write a balanced equation showing how perchloric and can transfer a proton to sulfuric acid
2. (b) Draw a Lewis electron dot structure for sulfuric acid How can sulfuric acid function as a base?

Interpretation:

The balanced equation has to be written for the reaction between perchloric acid and sulfuric acid;

Concept Introduction:

Balanced reaction is a chemical reaction in which number of atoms for each element in the reaction and the total charge are same on both reactant side and the product side.

Steps in balancing the information

• Step 1: Write the unbalanced equation
• Step 2: Find the coefficient to balance the equation.
• The coefficient should be reduced to the smallest whole number

Sulfuric acid is a weaker acid than perchloric acid. This is because of the fact that the resonating structure of the conjugate base of perchloric acid is more stable than the resonating structure of the conjugate base of the sulfuric acid. The free lone pairs of oxygen atom of the sulfuric acid can bind to hydrogen ion (H+).

Sulfuric acid is a weaker acid than perchloric acid. It is because of the fact that conjugate base of perchloric acid (perchlorate anion) is more stable than the conjugate base of sulfuric acid (hydrogen sulfate anion). Sulfuric acid has only two double bonds with oxygen while there are three chlorine oxygen double bonds. therefore resonance delocalization of negative charge on oxygen is better in the perchlorate anion. Thus proton is transferred from perchloric acid which is stronger acid to sulfuric acid which is a weaker acid.

Structure of perchlorate anion and hydrogen sulfate anion are given below:

Interpretation:

Lewis electron dot structure has to be drawn for the sulfuric acid and function of sulfuric acid has to be explained.

Concept Introduction:

Sulfuric acid is a weaker acid than perchloric acid. This is because of the fact that the resonating structure of the conjugate base of perchloric acid is more stable than the resonating structure of the conjugate base of the sulfuric acid. The free lone pairs of oxygen atom of the sulfuric acid can bind to hydrogen ion (H+).