Continuation of the chemistry Titration Experiment 2026

Added: 2026-05-20

[00:00:00]All right. So, now to proceed here Now, that leads us to the next question, BII.

[00:00:06]Now, the other time we got the concentration of the pure A, the acid, to be 0.1 mole per dm3.

[00:00:17]All right. Now, notice this to be the pure acid.

[00:00:20]And here we're told that the acid is in an impure form. That means that the 5.1 g dissolved or measured for this acid must have contained mass of impurities together. Now, here we've been able to analyze Okay, we've been able to convert the mole per dm3 concentration of the acid to grams per dm3. So, that means that by virtue of the pure acid that was reacted or that reacted with the base, we have it to be 9.8 g, you know, dissolved in 1,000.

[00:00:53]The actual pure acid was 9.8 g to be measured and dissolved in 1,000 of this solution. That's what it means. That's for the pure. And the impure here, we're told that 5.1 g was dissolved in 500. If 5.1 g was dissolved in 500 as I often explain, simplified concentration, it means that how many of this mass equivalently will be in 1,000 because concentration is always per dm3. So, if what if there are 5.1 g in 500, it means there would be altogether 10.2 g in 1,000. So, permit me from there, okay?

[00:01:33]Then we have I've been able to convert the uh the mass the concentration of the acid also in mass in grams per dm3.

[00:01:48]in grams per dm3. All right. So, here we have the uh So, from the pure from the pure form of the acid, we have it to be there are 9.8 g of the pure H2SO4 to be in 1,000.

[00:02:09]Okay? To be in 1,000. Okay, now let me not go this way.

[00:02:12]Now, if there are pure 9.8 g of the acid in 1,000, and the pure here were turned 5.1 g in 500, then equivalently means that 10.2 g in 1,000.

[00:02:25]Okay? 10.2 g in 1,000. That's what it means. Now, compare this. Look at the pure acid. Look at that of the impure form. So, that tells us that part of this impurity, the actual pure form there, okay, the actual pure form of the acid is 9.8, while the difference in between these two tells us the mass of the impurity. So, we can say that the mass of the impurity, mass of impurity, okay, becomes the difference, 10.2 g minus 9.8 g. Okay? That tells us that we have Let me quickly 10.2 minus 9.8.

[00:03:10]So, we have that to be 0.4.

[00:03:14]All right, 0.4 g becomes that of the impurity.

[00:03:19]Okay? All right. So, we are not asked to find the mass of the impurity, but rather we have to find the percentage purity, percentage purity. Okay? I think that's the last question. Percentage purity.

[00:03:33]All right. So, now the percentage purity here, that's B I I I, percentage purity tells us that the mass of pure over mass of impure * 100. Notice percentage, this. So, mass of the pure we had it to be 9.8. Okay, mass of the impure all together, all right, gives us 10.2 * 100. So, we have this.

[00:04:09]Let's go very quickly. 9.8 / 10.2.

[00:04:14]Okay.

[00:04:16]Now, we have this to be 0.96 * 100, okay? We have it to be 96%. So, it means that the percentage purity of the acid is 98% 96% rather, according to our calculation, all right? So, that comes to the end of the the WAEC chemistry practical 2026 titration experiment. So, I wish you all the best in your exams tomorrow. Thank you and God bless you. We await your testimony.

[00:04:46]All right.