May 29, 2024, 04:54:46 AM
Forum Rules: Read This Before Posting


Topic: Dilution problem  (Read 3300 times)

0 Members and 1 Guest are viewing this topic.

Offline ziczac

  • Very New Member
  • *
  • Posts: 1
  • Mole Snacks: +0/-0
Dilution problem
« on: May 05, 2009, 10:24:36 PM »
I know this question is basic, but I am not sure my anwswer is right or not.

I was given a 37% w/w HCl which I have to dilute it to a 50 ml of 2 Mol/L HCl.

The way i am doing it is:

Mass of HCl present in the target solution, 50 ml of 2 Mol/L = ( 2 x 36.5) / (1000 / 50) = 3.65 g

As every 100g of the Concentrated acid contains 37g of HCl,

The amount need for dilution = (3.65 / 37) x 100 = 9.86g

i.e. Weight 9.86g of the conc. HCl and add water to 50 ml to get the target solution.


Is the above calculation correct or not?



Offline plankk

  • Full Member
  • ****
  • Posts: 150
  • Mole Snacks: +20/-4
  • Gender: Female
Re: Dilution problem
« Reply #1 on: May 06, 2009, 12:02:54 AM »
Correct.

Offline Borek

  • Mr. pH
  • Administrator
  • Deity Member
  • *
  • Posts: 27689
  • Mole Snacks: +1803/-410
  • Gender: Male
  • I am known to be occasionally wrong.
    • Chembuddy
Re: Dilution problem
« Reply #2 on: May 06, 2009, 03:17:44 AM »
I know this question is basic

Quote
I was given a 37% w/w HCl

This makes the question acidic, not basic.

I would go one step further - take density tables and check what volume of concentrated HCl you need.
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info

Sponsored Links