So in this case, my solution already has hydrochloric acid in it.

So to balance it let me put 2 let me put a 2 in front of the hydrochloric acid, the aqueous solution of hydrochloric acid.

But what happens if you at hydrochloric acid to this solution right here?

Let's say it's hydrochloric acid. HCl.

But hydrochloric acid is one of them.

It tells us the concentration or the moles of hydrochloric acid per liter of our entire solution.

When I take that first measurement, my solution of hydrogen chloride, or hydrochloric acid, has a pH 0.

And we need to figure out the mass of this calcium carbonate that we need to react completely with the hydrochloric acid solution.

If I were to take some hydrochloric acid that's actually what it's called, but you could say hydrogen chloride in an aqueous solution.

This hydrochloric acid is donating a proton to this water molecule, right?

Well, this hydrochloric acid is let me look at this reaction right here.

So now this equation is balanced after we threw that 2 coefficient on the hydrochloric acid.

What we want to do in this video is figure out the mass of calcium carbonate we need to react completely with 25 milliliters of 0.75 molar hydrochloric acid solution.

And just to remind ourselves what we're talking about we have this hydrochloric acid, and it is dissolved in water.

So this hydrochloric acid is donating a proton to this water molecule to make a hydronium molecule, and it gave it away.

Well, all of these hydrogen protons that disassociate from the hydrochloric acid are all going to react with these OHs you have here.

Finally, you can try immersing the seeds in a sulfuric acid solution.

And the way you can kind of think of it is you had hydrochloric acid before, when this guy gave away this atom or this proton right there.

If you were to add a strong acid to the solution, what would happen?

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?

A solution whose pH is 7.3 will contain equal concentrations of hypochlorous acid and hypochlorite ion reducing the pH will shift the balance toward the acid.

So if we have hydrogen flouride, or if it's in an aqueous solution it's hydrofluoric acid.

Now, what I'm going to do is I'm going to titrate this aqueous solution of acid.

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

This reaction involves the preparation of aldehydes (R CHO) from nitriles (R CN) using tin(II) chloride (SnCl2), hydrochloric acid (HCl) and quenching the resulting iminium salt ( R CH NH2 Cl ) with water (H2O).

Sulfuric acid and then perchloric acid.

Vinegar is an example of a solution where the molecules of acetic acid are blended with molecules of water.

Acid

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

Formic Acid

Acetic Acid

Carbonic acid

Maleic Acid

Squaric acid

Ascorbic acid

Acid Jazz

Acid Punk

Perflourooctanoic acid.

Nitric acid.

Lactic acid.

Stearic acid can be converted to oleic acid in the liver.

lives inside the equivalent of battery acid, and excretes sulfuric acid.

Show Acid Behavior

Acetyle salicylic acid

l Lactic acid