# Determine an unknown concentration or volume using an acid–base titration. Calculate the volume of 2.63×10-2 M barium hydroxide required to neutralize 16.1 mL of a 0.110 M nitric acid solution. ? mL

Okay class, let's take a look at how to determine the volume needed to neutralize a solution. In this case, we have a 0.110 M nitric acid solution that requires 2.63×10-² M barium hydroxide to neutralize 16.1 mL of it. To calculate the volume, we will use the formula CaVa = CbVb, where Ca is the concentration of the acid, Cb is the concentration of the base, Va is the volume of the acid, and Vb is the volume of the base. So, substituting in the values from the problem, we get 0.0263 × Va = 16.1 × 0.110. Solving for Va, we get that Va is equal to 67.34mL. So, that's our answer - the volume of 2.63×10-² M barium hydroxide required to neutralize 16.1 mL of a 0.110 M nitric acid solution is 67.34mL. For more information on determining volumes, please see brainly.com/question/28241684.