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Chemistry Forums for Students => Undergraduate General Chemistry Forum => Topic started by: tkelley on April 25, 2006, 09:12:56 AM

Title: What is the molarity of an acetic acid solution prepared by diluting 200.0 ml of
Post by: tkelley on April 25, 2006, 09:12:56 AM
Sorry about this but having problems with this type of problem... 

What is the molarity of an acetic acid solution prepared by diluting 200.0 ml of .500M HC2H3O2  to a tolal of 1.00L 

I just need help with the general set up if possible.   
thanks tom
Title: Re: One more question...
Post by: Albert on April 25, 2006, 09:17:07 AM
Multiplying a volume by a molar concentration (M) you'll get the moles of that substance.

Then, moles/volume = concentration.
Title: Re: One more question...
Post by: Borek on April 25, 2006, 10:45:42 AM
Most general approach:

http://www.chembuddy.com/?left=concentration&right=dilution-mixing
Title: Re: What is the molarity of an acetic acid solution prepared by diluting 200.0 ml of
Post by: tennis freak on May 17, 2006, 06:31:24 PM
my suggestion would be the equation mv=mv where the initial molarity times the initial volume equals the final molarity times the final volume.  just solve for m by dividing the original mv by the second v and you have your answer.
Title: Re: What is the molarity of an acetic acid solution prepared by diluting 200.0 ml of
Post by: syko sykes on May 17, 2006, 08:58:53 PM
Quote from: tennis freak on May 17, 2006, 06:31:24 PM
my suggestion would be the equation mv=mv where the initial molarity times the initial volume equals the final molarity times the final volume.  just solve for m by dividing the original mv by the second v and you have your answer.
and don't forget conversions, i.e. .2L not 200mL

should end up with .1M for answer
Title: Re: What is the molarity of an acetic acid solution prepared by diluting 200.0 ml of
Post by: tennis freak on May 17, 2006, 09:55:53 PM
Quote from: syko sykes on May 17, 2006, 08:58:53 PM
Quote from: tennis freak on May 17, 2006, 06:31:24 PM
my suggestion would be the equation mv=mv where the initial molarity times the initial volume equals the final molarity times the final volume.  just solve for m by dividing the original mv by the second v and you have your answer.
and don't forget conversions, i.e. .2L not 200mL

should end up with .1M for answer

right nice catch dude ;D