# The Naked Scientists Forum

### Author Topic: Dilution ?  (Read 3051 times)

#### kristenann2000

• First timers
• Posts: 3
##### Dilution ?
« on: 04/09/2005 21:23:29 »
In general I understand how to do dilutions using the MV=MV formula.  However, I'm for some reason puzzled over certain issue I have encountered.  I've never really used dilution ratios, but it is my understanding that 1:10 solution would be 1/10 of its initial concentration.  It is saying to mix 1 part solute with 9 parts solvent.

So anyways, a fellow chemist told me that she prepared 1:1 HCl using 10 ml HCl and 10 ml water.  So how is this a 1:1 solution?  In a 1:1 solution wouldn't their ideally not be a dilution occuring since the initial and final concentration would be the same?  It seems like using 10 ml of HCl and 10 ml of water would create a 1:2 dilution because this would decrease the concentration of HCl in 1/2 (using MV=MV, you would have V=10 and V=20).

#### Steve Vai

• Jr. Member
• Posts: 30
##### Re: Dilution ?
« Reply #1 on: 04/09/2005 22:13:00 »
ratios

i think you are wrong on the first count, in a dilution ratio of 1:10m it would be 1/11 of the original concentration, there are 11 parts, 1 part solute and 10 parts solvent

a 1:1 ratio isnt 1/1, its 1/2 as there are two parts in total

i think.

"Turkeys killed my family" - Chip, 02/09/2005, 12:49

#### David Sparkman

• Sr. Member
• Posts: 234
##### Re: Dilution ?
« Reply #2 on: 05/09/2005 04:59:59 »
Add to the fact that most HCL is not 100% HCL out of the bottle, but has some water in it to try to hold down fuming.

David

#### The Naked Scientists Forum

##### Re: Dilution ?
« Reply #2 on: 05/09/2005 04:59:59 »