Trifluoroacetic acid has the chemical formula CF3CO2H. It is a colorless liquid that has a density of 1.489 g/mL. (d) How many milliliters of a 0.500 M solution of NaOH would it take to neutralize 10.5 mL of trifluoroacetic acid?

Video transcript

Hey everyone, we're asked to calculate the volume of 0.4-0 moller potassium hydroxide solution needed to neutralize 6.30 ml of per cleric acid and were given the density of per cleric acid 1st. Let's go ahead and write out our reaction. So we know that we have per clark acid and it reacts with potassium hydroxide. So we're going to produce potassium perk Laurie plus water 1st. We want to determine the mole of potassium hydroxide needed to neutralize our perk Lorik acid. So starting off with 6.30 ml of Perk Lorik acid, We're going to take the density a per cleric acid which is 1. g per one millim. Taking the molar mass of per caloric acid. We know that it's 100.458g of per cleric acid Per one Mole of Perk Lorik Acid. And as we can see from our reaction, We know that one mole A per clerk acid is equivalent to one mole of potassium hydroxide. So when we calculate this out, we end up with a total of 0.1047 mol of potassium hydroxide. Now that we have our mole of potassium hydroxide, we can take this value and calculate our volume of potassium hydroxide. Starting off with 0.1047 mole of potassium hydroxide. We can take our malaria T, which is 0.420 mol of potassium hydroxide per one leader a potassium hydroxide And this will get us a total of 0. leaders which we can also say as ml. And this is our final answer. So I hope this made sense and let us know if you have any questions.