How many mL of 13.00 M hydrochloric acid must be diluted with water to prepare 1.20 L....?

How many mL of 13.00 M hydrochloric acid must be diluted with water to prepare 1.20 L of a 0.440 M HCL solution?

Answer:
x(13.00 M) = 1.20L (.440 M)=40.6mL 13.00 M HCl
I am not going to ans. your question but I can say this, if it isn't suffiencently diluted you could end up with permanent scars. My daughter has one on her neck because her lab partner made a boo boo. She came home and told us she finally did some 'acid'
Diluted solution contains:

0.440 [mol/L] * 1.20 [L] = 0.528 mol HCl

However, the number of moles of HCl does not change, so the original solution has the same 0.528 mol HCl

0.528 [mol] / 13.00 [mol/L] = 0.040615 L = 40.62 mL
Well I think that's like this: 0.44(mol/lit)*1.2(lit)=0.528 ,moles
So you need that amount of moles which is 0.528(mole)/13(mole/lit)=.0406... or 40.6 mL.

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