How to solve this Solution Chemistry problem?

Question

A 48.83-mL sample of an ammonia solution is analyzed by titration with HCl. The reaction is given below.

NH_3(aq) + H^+(aq) --> NH_4^+(aq)

It took 38.00 mL of 0.0976 M HCl to titrate (react completely with) the ammonia. What is the concentration of the original ammonia solution?

Answer 1

The reaction in question is

NH₃(aq) + H^+(aq) --> NH₄^+(aq)

moles of H⁺ used = 38.00 ml x 1 L/1000 ml x 0.0976 mol/L = 0.003709 mol H⁺

moles NH3 = 0.003709 mol H⁺ x 1 mol NH3/mol HCL = 0.003709

concentration NH3 = 0.003709 mol/0.04883L = 0.07595 M

Check my math as I’m using an antique system