Relationship between osmolarity and molarity of concentrated

How can molarity and osmolarity be calculated from m/v? | Socratic

relationship between osmolarity and molarity of concentrated

Molarity vs Osmolarity. Concentration is an important phenomenon, and it is used very commonly in chemistry. It is used to indicate quantitative. concentration wants to study the relationship between osmolality and osmolarity. as ratio of the solution molarity and its molality was introduced to convert. Answer: Osmolarity equals molarity times the van't Hoff i factor. The video below explains the difference between molarity and osmolarity.

So I'm going to draw little sodiums, and next to them, little chlorides. So this is sodium chloride. And again, I'm just drawing a few of them.

Difference Between Molarity and Osmolarity -

But just remember, because it's in a box I've got an entire mole of each of these things. So I've got here sodium chloride. And I'll try to keep the color code consistent. And I have two moles of it, so I've got an equal amount in either box. And now I've got three boxes of glucose. I'm going to draw glucose on this side.

So you can see, I'm going from one box of urea, two boxes of sodium, to now three boxes of glucose. I'm going to just draw glucose as little red balls here. So each little red ball represents a glucose.

And just to remind you what glucose looks like, we're going to draw it out as well. So glucose is a little molecule like this with an oxygen. And off of it, you get these little OH groups, so a little OH there option, oxygen and hyrdogen there. This one is like that. This one goes down.

How can molarity and osmolarity be calculated from m/v?

And you have another carbon coming off of it, with an OH as well. So that's your little glucose, and each little red dot represents one of those molecules. So we've got six moles of stuff here. And I'm going to make a little bit of space on this canvas. And we're going to say now, we're going to take our stuff and put it into a liter. So imagine I take a bucket or something here, and this is full of water, one liter of water exactly. So this is my little one liter. And you're going to take all this stuff, and let's say, dump it in here.

So all six moles of stuff go in there. And now, I ask you, tell me the molarity of this stuff. So we have three things. So let's start with urea.

relationship between osmolarity and molarity of concentrated

What is the molarity of urea? Well, you'd say, well, I have one mole of it. And I have one liter, so one mole per liter equals one molarity. And a big M represents molarity. So that's easy to do.

relationship between osmolarity and molarity of concentrated

And then you have, let's say, sodium chloride. So you have NaCl. And you have two moles of it. We put in two moles of it into one liter. So you say, you have two molarity of sodium chloride. And finally, you have glucose.

And you say, well, glucose-- and you're getting the pattern here. Three moles and becomes obviously same volume, and you have three molarity. So that's pretty straightforward, one, two, three. Now, imagine I actually take a little magnifying glass. I'm going to leave that up.

Take a little bit of that water, and let's say, I zoom in on it. This is where things get really interesting. Let's say I zoom in on this a little bit of water right there, just to get a better look at what's going on. So I zoom in on it, and I get something like this.

How is osmolarity related to molarity? | Socratic

Let's see if I can draw it out for you. Oh, my circle is not so neat, but you get the idea. So you zoom in on that little circle, and here's what you might see. I'm going to draw the sodium first. So you might get something like this.

Molarity vs. osmolarity

And let's draw another sodium over here. And just to label it, so you know what it is. And it's positively charged. And sodium you positively charged, and we have some chlorides.

And I'm not drawing them next to each other on purpose, because you'll see what happens. Even though sodium and chloride started out as partners. They started out next to each other. The moment they hit water an interesting thing happens. So the second they hit water, you've got H2O. And oxygen is slightly negatively charged.

And let's draw oxygen there. And it's attached to two hydrogens, two little hydrogens like that. And this is your slightly negatively charged oxygen and your slightly positively charged hydrogens. And so that negative oxygen and that positive nitrogen attract each other. So it's going to line up like that. In fact, you might even get another oxygen over here, line up with its two hydrogens and maybe even another one over here.

And you see what's happening is that, these oxygens and the hydrogens are lining up, so that the oxygens can be close to the nitrogen, or to the sodium, I said nitrogen by accident, sorry. And it happens over here too. Oxygen comes in close to the sodium, because it's got that little negatively-charged part to it-- call it a partial dipole-- and a little bit over here too. So some of that negativelyy-charged oxygen is being attracted to the very positive sodium.

And actually, the opposite is happening over here. Here, you have these slightly positively-charged hydrogen, two of them. It is used to indicate quantitative measurement of a substance. If you want to determine the amount of copper ions in a solution, it can be given as a concentration measurement. All most all the chemical calculations are using concentration measurements to draw conclusions about the mixture. To determine the concentration, we need to have a mixture of components.

There are few types of methods to measure the concentration. They are mass concentration, number concentration, molar concentration, and volume concentration. All are ratios where the numerator is representing the amount of the solute, and the denominator is representing the amount of solvent. In all these methods, the way of giving the solute differs. However, the denominator is always the volume of the solvent.

Molarity Molarity is also known as molar concentration. This is the ratio between the number of moles of a substance in one volume of a solvent.

relationship between osmolarity and molarity of concentrated

Conventionally, the solvent volume is given in cubic meters. However, for our convenience we often use liters or cubic decimeters.