A 0.0875 M solution of aqueous ammonia was titrated with a solution of sulphuric acid. If 25.00 mL of the ammonia solution required 30.66 mL of the acid to reach the end-point, calculate the molarity of the acid.

NH3(aq) + H2SO4(aq) �¨ (NH4)2SO4(aq)

Write the equation.

H2SO4 + 2NH3 ==> (NH4)2SO4

Calculate mols NH3. mols = L x M.
Convert mols NH3 to mols H2SO4 using the coefficients in the balanced equation.
Convert mols H2SO4 to L using mols = L x M. You have mols and L which leaves just the M as an unknown. Post your work if you get stuck.

To determine the molarity of the acid, we can use the molarity equation:

Molarity = (moles of solute) / (volume of solution in liters)

In this case, the moles of solute refer to the moles of acid used in the titration. The volume of solution refers to the volume of the ammonia solution.

First, let's calculate the moles of ammonia used in the titration by using the given concentration and volume:

Moles of ammonia = concentration x volume = 0.0875 M x 0.02500 L

Now, since the balanced equation between ammonia and sulfuric acid is 1:1, the number of moles of ammonia used is equal to the number of moles of sulfuric acid used.

Therefore, the moles of sulfuric acid used in the titration is also 0.0875 M x 0.02500 L.

Next, we need to convert the volume of acid used to liters:

Volume of acid used = 30.66 mL = 30.66 / 1000 L

Now, we can substitute the values into the molarity equation to solve for the molarity of the acid:

Molarity of acid = (moles of acid) / (volume of acid used)

Molarity of acid = (0.0875 M x 0.02500 L) / (30.66 / 1000 L)

Calculate the value to find the molarity of the acid.