00:02
Hello there.
00:03
I see that there are multiple parts to this question.
00:08
So we'll go over each of them.
00:09
So the first part, how you go about trying to solve further concentration of hydrochloric acid.
00:18
Sorry.
00:20
How you go about this is, okay, work with me, work with, okay.
00:26
How you go about this is that we would have to times the volume, malarity, and moles of the second part to get the first part and the reason why is because how the how this equation is set up and you notice that i balanced it so i balanced it where i put the two in a certain spot that's where the mole will come into the important that's where the moles are going to be used for this question and have its importance and my pen is acting up so so i just did a calculation where we're setting it up, where we're solving for the concentration, where it's like for the volume concentration and moles of our sodium carbonate.
01:25
And we're dividing the volume and the moles of hydrochloric acid.
01:33
And doing that, this is how our data is set up.
01:41
I kind of left them alert, middle leaders being the same, but i just set up and just, i set them up where i conferred them to leaders just to end up with this outcome.
01:59
I think it could end up with the outcome without conferring it, but i just did it just to be safe.
02:06
Okay, so for the second part, where am i? okay, so they brought up where they want to know what.
02:14
Is the ph of the resulting solution will be when you have water that is added to 20 milliliters of solution of ph 4 in the volume made up of 100 milliliters and how you go about this with this setup where we had to get the ph and we had to conferred that to like one times so we had to convert that to 10 milliliters i mean and then we got i mean malaria and then we got the concentration times volume is a unique type of setup but doing so that we times the concentration by 20 millimeters and then we're leaving that c2 blank because we're solving for the 100 milliliters because that's the total outcome and then and doing that calculation, you will end up with 0 .2 times 10 to negative 4.
03:28
So the next one, where...
03:37
And so by doing so, this is where we solve the ph now, where we do the negative log of 8 of 0 .2 times 10 to negative 4, where we end up with 4 .7.
03:53
So that's how you go about it for that one.
03:56
Then the next one, they want us to find the, they want us to find the hydronium ion for a natural, for a natural, a clear solution with the ph of 7.
04:13
So how we go about this.
04:16
Again, the ph is equal to negative log of hydronium.
04:22
And then to fix this, you can remove the negative sign over to the 7.
04:27
And then set up where it's 10 by the power of negative 7, which is where you get 1 times 10 to the negative 7.
04:38
And then for the next one, they want to find the hydroxide or natural aqueath of the ph of 7.
04:49
So how we go about that is that it minus the 14 by 7, which we get 7, and then same process, end up getting the same set up, i mean the same answer.
05:04
So then the next one, they want to know if the p k -a of negative log times k -a value of an acid is greater than zero, is it a strong or weak acid? so for this one, how they brought it up, they brought it up when i saw they said when the pk value that if the acid is greater than zero, i mean, the base, if the base is greater than zero, no, if the base is greater than zero, then the, then, then that means, it was like something where it was like vice versa.
06:00
I know i'm getting my stain wrong.
06:03
I mean, they were saying, it's saying that the strong.
06:07
The acid the weaker the conjugate base so the weaker the acid the stronger the conjugate pace so sorry based off of that so based off of dad it basically says that it's basically weak so then the next one they want us to calculate the ph of hydrobromic acid solution preparing by adding 5 .6 times 10 to negative 2 moles of hydrobromic acid and enough water for a final volume of 750 milliliters so how we go about this oh that was the part i was supposed to show you so when we go about this we so i just confer this to make it into a smaller mole and then um conferred the mill liters to liters and then set up into like a malarity type of i don't know why i put the g i set up in a malarity type of setup make into a concentration and to do so i'm able to set up this ph where i got 1 .12 so then i want to calculate the ph of hcn aqueous solution with 0 .0 .0 .0 .0 to malaria and a k of 4 .9 times 10 to negative 10 and then how to set that up.
08:11
I end up doing like the ice setup where basically plot it out like i understand how ice is a bit tricky so this is our initial concentration and i forgot what e was i'm sorry let me try what 8 was okay so this is initial change in equilibrium so that's what i was trying to say so this is how we set it up so we write down what we know when it came down to what the malaria d is and the 0 that i put down negative add the plus and then put the x there where our setup is the 2x2 xxs time each other divided by 0 .2 minus x and doing so we have our setup where it will where we have 4 .9 times 10 to a negative 10 times our x square over our 0 .2 minus x and this is how you get the outcome of 10 to the negative 6 and then we're going to do our ph law and doing so we get 6.
09:28
The next one is to calculate the ph of the solution.
09:32
Oops, sorry, i'm hitting my mind.
09:34
Of a 7 .5 times 10 to negative 6 solution of bromon, bromam hydroxide.
09:47
So how we go about this is basically do a negative log setup where we end up getting, let me go over this because i think i did something wrong here.
10:03
Okay, so you do this where you get 5 .12 and then at that you just minus this right, 14, and this is what your ph would look like...