Nitric acid.

You have nitric acid.

What are you serving today, nitric acid?

My weak acid.

And so weak acid.

Ammonium is a weak acid.

let's say I have some weak acid.

This one that has this weak base and its conjugate weak acid?

Preparation Oxalic acid is mainly manufactured by the oxidation of carbohydrates or glucose using nitric acid or air in the presence of vanadium pentoxide.

SAL Let's say I have some weak acid.

The ammonia from the Haber process is then converted into nitric acid (HNO3) in the Ostwald process.

So I could rewrite the same weak acid equilibrium as a weak base equilibrium.

We've dealt with the weak acid, so let's try an example with the weak base.

That could be the conjugate base of the weak acid.

Moles per liter divided by the concentration of our weak acid.

They can disassociate, or it's in equilibrium because it's a weak acid.

We know that this is a weak acid it doesn't disassociate completely.

So you're going to have more of our weak base turning into a weak acid and producing more OH.

The definition of a buffer is just a solution of a weak acid in equilibrium with its conjugate weak base.

BPh3 is a weak Lewis acid while B(C6F5)3 is a strong Lewis acid due to the electronegativity of the fluorine atoms.

But we know it's a weak acid, so this reaction goes in two directions.

But if you do it here if you apply the sodium hydroxide to this solution, the solution that contains a weak acid and it's conjugate base, the weak acid and its conjugate base, what happens?

So times the concentration of our weak acid divided by the concentration of our weak base is equal to our concentration of our hydrogen.

So it's a weak acid, where the A could be any other kind of molecular group.

Let's say I have a bucket of aqueous solution, and it contains some weak acid in it.

So it can be in equilibrium with since it's a weak acid, it's going to produce some hydrogen proton.

Nitric oxide synthases () (NOSs) are a family of enzymes catalyzing the production of nitric oxide (NO) from L arginine.

Now, this is just the pKa of our weak acid, which is just the negative log of its equilibrium constant.

Another common example is nitric oxide (NO).

We couldn't turn off the nitric oxide.

Sulfuric acid and then perchloric acid.

So this is nitric oxide or nitrogen monoxide.

So the negative log of all of that stuff, of your acidic equilibrium constant, times HA, our weak acid divided by our weak base, is equal to the negative log of our hydrogen concentration.

So we could say, plus the logarithm of our conjugate base concentration divided by the weak acid concentration is equal to the pH.

In the next video, I'm going to try to do the same thing, but I'm going to do it with a weak acid.

Acid

So 0.8 moles of nitric oxide or nitrogen monoxide.

Now, with that said, let's explore a little bit the math of a buffer, which is really just the math of a weak acid.

e Each of the devices contained about 100 kilograms of conventional explosives surrounding several layers of chemicals, including potassium cyanide, sodium cyanide, hydrogen peroxide, potassium ferricyanide, nitric acid, mixed acids, as well as various insecticides and pesticides.

So we're going to have 24 grams of nitric oxide.

So this can to be simplified to minus log of our Ka minus the log our weak acid concentration divided by its conjugate base concentration.

Formic Acid

Acetic Acid

Carbonic acid

Maleic Acid