[Histonet] Question

[Goins, Tresa]

The final concentration of 1.25 ml 10N NaOH into 1000 ml water is the same as:
12.5 ml 1N NaOH into 987.5 ml water.

-----Original Message-----
From: Geoff [mailto:mcauliff at rwjms.rutgers.edu] 
Sent: Friday, May 01, 2015 9:16 AM
To: histonet at lists.utsouthwestern.edu
Subject: Re: [Histonet] Question

Huh?
Take a solution more dilute than you want it and dilute it more?

Geoff

On 5/1/2015 10:41 AM, Goins, Tresa wrote:
> All that matters here is the final concentration of the reagent - it doesn't matter what stock you start with if you calculate the dilution.
> Adding 1.25 ml to 1000 ml is diluted by a factor of .00125 so 10N x .00125 = .0125 N final concentration.
> If using a 1 N stock solution, just add 10X the volume or 12.5 ml 1 N stock to 987.5 ml water.
>
> Hope this helps,
>
> Tresa
>
> -----Original Message-----
> From: histonet-bounces at lists.utsouthwestern.edu [mailto:histonet-bounces at lists.utsouthwestern.edu] On Behalf Of Bernice Frederick
> Sent: Thursday, April 30, 2015 1:35 PM
> To: Histonet at lists.utsouthwestern.edu
> Subject: [Histonet] Question
>
> All,
> I have a procedure here that call for and I quote "1.25 ml NaOH 10N in 1L of water." I know how to get 1 N, but how do I get 10. Having rarely hd the opportunity to make many Normal solutions ,my brain is not computing. Is it an error?
> Bernice
>
> Bernice Frederick HTL (ASCP)
> Senior Research Tech
> Pathology Core Facility
> Robert. H. Lurie Cancer Center
> Northwestern University
> 710 N Fairbanks Court
> Olson 8-421
> Chicago,IL 60611
> 312-503-3723
> b-frederick at northwestern.edu<mailto:b-frederick at northwestern.edu>
>
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Geoff McAuliffe, Ph.D.
Neuroscience and Cell Biology
Robert Wood Johnson Medical School
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