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

But hydrochloric acid is one of them.

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.

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

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

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

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.

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 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.

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.

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.

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.

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).