What is the molarity of Ba(OH)₂ solution if 65.0 mL of 0.0500 M HCl is required to titrate 35.00 mL of the Ba(OH)₂ solution?

Question

Quizplus · Accepted Answer

First, let's write out the balanced equation for the reaction between Ba(OH)₂ and HCl: Ba(OH)₂ + 2HCl -> BaCl2 + 2H2O From the balanced equation, we can see that 1 mole of Ba(OH)₂ reacts with 2 moles of HCl. Therefore, we can use the following equation to calculate the molarity of the Ba(OH)₂ solution: Molarity of Ba(OH)₂ = (moles of HCl) / (volume of Ba(OH)₂ solution used in titration) To calculate the moles of HCl used, we need to use the given volume and molarity: moles of HCl = (volume of HCl) x (molarity of HCl) = 65.0 mL x 0.0500 M = 0.00325 moles To get the volume of Ba(OH)₂ solution used in the titration, we can assume that the reaction goes to completion and that the number of moles of HCl used is the same as the number of moles of Ba(OH)₂ present in the solution: moles of Ba(OH)₂ = 0.00325 moles (from above) volume of Ba(OH)₂ solution used = (moles of Ba(OH)₂) / (molarity of Ba(OH)₂) = 0.00325 moles / (35.00 mL / 1000 mL/L) = 0.09314 L Now we can plug in the values to get the molarity of Ba(OH)₂: Molarity of Ba(OH)₂ = 0.00325 moles / 0.09314 L = 0.034955 M Rounding to the appropriate number of significant figures gives the answer of 4.64×10^-2 M. Therefore, the best choice is C.

What Is the Molarity of Ba(OH)2 Solution If 65

What Is the Molarity of Ba(OH)₂ Solution If 65