What volume in ml of 0200 m naoh do we need to titrate 3600...

Transcript

00:01 Hi there.

00:02 We are conducting a titration, and we want to determine the volume of our base that we would need to reach the equivalence point.

00:11 Well, the equivalence point occurs when we have a stoichiometric equal amount of each of the reactants.

00:19 So we need a balanced equation.

00:22 So we are reacting the acid, hbr, with the base, an a -o -h.

00:30 These are both aqua -os solutions.

00:32 We are going to get aquas, n -a -v -r, and liquid h -2o.

00:41 I'm not putting the subscripts in right now because they are not important for what we need, which is a balanced equation.

00:49 Okay, so looking at this equation, it is balanced as written.

00:53 So that tells us that we have a one -to -one ratio between the acid and the base.

01:01 Okay, so let's go ahead and do some strikiometry to calculate how much of that base we need.

01:07 So we have 36 milliliters of the hbr.

01:16 That is what we are trying to titrate.

01:20 And we have its molarity.

01:23 So i am going to change this to liters.

01:26 In 1 ,000 milliliters, there is one liter.

01:33 Or 1 ,000 militers equals one liter, i guess i should say.

01:37 And next then, so now we're in liters.

01:40 So now i can use the molarity of hbr.

01:42 We are told because our molarity is moles per liter.

01:47 So there are 1 .40 moles of hbr per every liter of solution.

01:56 Because that is the definition of molarity.

01:58 It is moles per liter.

02:00 And the molarity is 0 .140...

What volume (in mL) of 0.200 M NaOH do we need to titrate 36.00 mL of 0.140 M HBr to the equivalence point? Express your answer to three significant figures.