Barium

Barium

Only barium and radium remain.

Barium oxide 2 Iron oxide 1

Let's say sodium hydroxide.

Radium still refuses to separated from barium.

Barium and radium can not be separated.

Alright, then, radium wouldn't be separated from barium.

And then plus a hydroxide ion.

Sodium hydroxide in an aqueous solution.

Remember, hydroxide is a strong base.

So it increases the hydroxide concentration.

You produce hydroxide and some sodium cations.

Or are you creating hydroxide or not?

The barium meal is a modern derivative of this research.

Your alkali earth metals are bonded with hydroxide.

I drank a barium solution, and stood behind a fluoroscope screen.

This was the problem to separate barium and radium somehow or other.

If you put them in water, the hydroxide pops off.

Well the little hydroxide ion is going to pop off.

And though they did not find a way to separate radium and barium in a single process they did discover a method of removing barium little by little in infinite decimal amounts.

All that was now left was to separate these two survivors barium and radium.

So if I take some lithium hydroxide in an aqueous solution.

As I slowly add hydroxide, it's going to increase the pH.

And a base is something that increases your hydroxide concentration in water.

It can be prepared by heating mixture of benzil, alcohol and potassium hydroxide.

So this guy, he had this nice little relationship with this hydroxide ion.

Arrhenius's definition, the base is something that creates hydroxide ions, or anions in water.

The hydroxide ion got disassociated, and it becomes a little bit fungible right here.

So I must have added 1 mole of hydroxide to get to this point.

The sample requires 34.47 milliliters of 0.485 molar sodium hydroxide to reach the equivalence point.

Working on the theory that once the whole of the barium is removed nothing could be left but radium.

So if you think about what's happening, if I just threw this sodium hydroxide in water.

And so on this axis, I'm going to slowly add more and more of this hydroxide.

So we have a double bond to one oxygen, and then another bond to a hydroxide.

Because sure, when you put the sodium hydroxide there, it just ate up all of the hydrogens.

This lithium hydroxide, when it goes into water There's a couple of ways to think of it.

And it's a weak base because it likes to accept hydrogen from water, leaving the water with just a hydroxide.

With the use of barium carbonate as starting material the first commercially used process became available in the 1860s developed by Margueritte and Sourdeval.

And then one of those water molecules that it plucked that hydrogen off of is now going to be a hydroxide molecule.

I guess on the other side, you could add more hydroxide and then you would have more OH concentration, and maybe a

The protective group can be removed by heating the compound in a solution of potassium hydroxide in propan 2 ol (a retro Favorskii reaction).

Now, everything I've done so far this is the Arrhenius definition where an acid increases your hydrogen concentration, a base increases your hydroxide concentration.

H2O, disassociating in itself, really, into a hydrogen ion in an aqueous solution plus a hydroxide anion in an aqueous solution or a negative ion.

So if I just did NaOH in an aqueous solution so that's just throwing it in water that disassociates completely into the sodium cation and hydroxide anion.