A compound containing Ti and Chlorine

[Lindy12]

This is the question am working on... A compound containing Ti and Chlorine is analyzed by converting all the Ti into 1.20g of TiO2 and all the chlorine into 6.45g of AgCl. What is the simplest formula...?

This is what I've done so far:
Moles of TiO2 = 1.20g/80g/mol = 0.015

Moles of AgCl 6.45g/143.4g/mol = 0.045

Am I on the right track? What do I do from here??

 

[The Bob]

Welcome to PF Lindy12!

The moles that you have calculated are the same as mine. However, I found the percentage mass of each element in each compound to find my answers. The point is (to my knowledge) it might not always work the way you have done it. You may need the percentage masses to be sure of what you have and what you are working with.

Knowing these moles you can find the empirical formula by dividing both by the smaller of the two to give you a ratio that will give you the formula.

The Bob (2004 ©)

 

[Lindy12]

Thanks The Bob :)
I'm really struggling with chemistry, as you can tell.

So, I went on to take 0.015 mol/0.015 mol = 1
and then 0.045 mol/0.015 mol = 3

So my final answer is TiCl3

What does the silver and oxygen have to do with the question?

 

[Borek]

Generally speaking - nothing.

However, the easiest way to check amount of chloride ions is to precipitate them as AgCl and to weight the precipitate. That's why you have AgCl in the question. Similarly with oxygen, although I must admit I don't know the procedure for Ti determination.

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[Lindy12]

Awesome! Thank you :)