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Metal ions that have a very large Kf with EDTA can be complexed at lower pH values than those that have smaller Kf:TrueFalse...

Question

Metal ions that have a very large Kf with EDTA can be complexed at lower pH values than those that have smaller Kf:TrueFalse

Metal ions that have a very large Kf with EDTA can be complexed at lower pH values than those that have smaller Kf: True False



Answers

What is meant by pH? True or false: A strong acid solution always has a lower pH than a weak acid solution. Explain.

So the ph scale just provides scientists and chemists with a very compact method to represent the solution acidity. So because the proton iron source in an aqueous solution is typically quite small, we use the P scale in the form of the ph scale that provides a convenient way to represent the solution acidity. So the ph is defined as follows equal to negative log of the protein source. So the ph decreases as the H plus concentration increases and vice versa. So this means that for strong acids the concentration of the H plus iron is more than the weak acid. Therefore the pH value for strong acids is lower than a weak acid, because pH is inversely proportional to the H plus concentration. Yeah.

So are females on alcohols. Both have age groups. So let's just go ahead and drop off. Fino. Well, this is simply a benzene private. We have an alcohol functional group touched. And now we can go ahead and draw any alcohol. For example, this is 1234 pentagonal. Well, we have five carbons, so I should concede. Yes, Both of them have a alcohol group present. So this is correct. So moving on females are weak assets. This is also factually true. And then lastly, just to finish up with addressing females and it's physical characteristic is also lassic acidic than our acetic acid.

Okay, So for this problem, we are tasked with a true or false. So the situation were put in is that we have sodium chloride, you may know is table salt. So this question actually has some real world implications. Well, it is dissolved in water, so we're throwing some salt, Sarah throwing some salt in a glass of water like this. And as you can guess, this will disassociate when it gets in the water, so it will dissolve in the water. So let's draw molecular representation of this, so we will see. So this is after Let's just keep this in mind. This is After that, I'm going to be depicting Now we see sodium will be separate from the chloride, okay, and we'll draw more so things aren't complete, but we need to finish the premise here. So we're told that the water molecules closest to the ions will tend to preferentially on face so that the oxygen part of water will face the sodium ions and face away from the chloride ions. So why might this be the case? Well, let's let's redraw this. Actually, this could be easier to demonstrate. So why this? Why might this be the case? So we know that this is an ionic bond, right? Sodium chloride. Meaning that Here we see this is the cat ion This positive and chloride is the n i n being negative and they would form together making this neutral, uh, molecule being sodium chloride. So when they disassociate, they go back to their iron form. Being sodium is positive and chloride is negative. So what do you know about water? What do we know about water? Let's draw it very quickly. So we know that it is Htoo, meaning it is comprised of two oxygen's to hydrogen, one oxygen. And there's a certain kind of bond that occurs in water. And this is going to depict the bond we're going to see it has a polar covalin bond. I'll abbreviate with PC meeting unequal sharing of electrons. Now, what this means is that I drew oxygen here in green and then I drew the hydrogen is here in blue. Now, electron is a very hydrogen. Sorry. Oxygen is a vory electro negative, Adam. Meaning is going to take a large share of the negative charge. So if you're to draw a dipole going to see that there's gonna be a partial negative at the oxygen parcel. Partial positives by the hydrogen is because oxygen tends to carry the bulk of the electrons in the chemical bond. So what do we know? We know opposites attract right and things that are the same. Charge Appel repel each other. You ever played around with magnets? This has been very clear to you, I assume so. We're seeing the same concept applied here, so we know that sodium is positive. The oxygen is largely negative, so these two are going to be attracted to one another, whereas is going to be repelled away from the chloride because it is heavily negative. It's completely negative for the chloride, and it is partially mostly negative for the oxygen. So that is why it is facing away from the chloride, but towards the sodium.

So we have a true false statement. We're looking at two solutions with same, uh, reverse osmotic pressure. They would also have the same osmotic pressure. Uh, and would that be so for a solution of sodium chloride at a lower mill arat e than a solution of, uh, calcium chloride. And so, uh, of course, the osmotic pressure depends on the polarity times, the ideal gas concert times, uh, temperature, But that m that polarity equals, uh, the mill aridity of the total her dissolved ions. So for one bowler solutions and one Moeller of each, that is one Moeller sodium chloride gives I'm sorry. Gives one Moeller sodium alien and one Moeller chloride ion and one Moeller Calcium chloride gives us one more calcium ion and to Moller chloride ion. Because each mole of the compound produces Tim als, of course. And I on when it's dissolved. And so, if we had two solutions at the same concentration, the that is that one Moeller, the, uh, calcium chloride would be exerting 1.5 times the polarity of dissolved ions. And that's what you would be plugging in. And so, for the same concentration of solution, you'd get a lot more osmotic pressure from the calcium chloride, so it takes less of the calcium chloride, less concentration of the calcium chloride. And so this is backwards. This is false. The, uh, the polarity of the sodium chloride in order that the concentration of the ions be the same would have to be 1.5 times the concentration of the calcium chloride, not less they and the concentration of calcium chloride.


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