The concentration of sulfuric acid needed to react with the given amount of ammonia solution is 0.5368 mol/L. This concentration is calculated based on the stoichiometry of the reaction and the volume of the sulfuric acid solution.
To determine the concentration of sulfuric acid needed to react with the given amount of ammonia solution, we can use the stoichiometry of the reaction and the volume of the sulfuric acid solution.
The balanced equation for the reaction between sulfuric acid (H2SO4) and ammonia (NH3) is:
H2SO4 + 2NH3 -> (NH4)2SO4
From the balanced equation, we can see that 1 mole of sulfuric acid reacts with 2 moles of ammonia. Therefore, the molar ratio between sulfuric acid and ammonia is 1:2.
First, we need to calculate the number of moles of ammonia present in the given 24.4 mL of 2.20 mol/L ammonia solution:
Moles of ammonia = volume (L) x concentration (mol/L)
Moles of ammonia = 24.4 mL x (1 L/1000 mL) x 2.20 mol/L = 0.05368 mol
Since the molar ratio between sulfuric acid and ammonia is 1:2, we can conclude that 0.05368 mol of ammonia would react with 0.02684 mol of sulfuric acid.
Next, we can calculate the concentration of the sulfuric acid solution using the volume of the solution (50.0 mL) and the number of moles of sulfuric acid (0.02684 mol):
Concentration of sulfuric acid = moles/volume (L)
Concentration of sulfuric acid = 0.02684 mol / (50.0 mL x (1 L/1000 mL)) = 0.5368 mol/L
Therefore, the concentration of sulfuric acid needed to react with 24.4 mL of a 2.20 mol/L ammonia solution using 50.0 mL of sulfuric acid is 0.5368 mol/L.