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Topic: 10 %solution of BaCl2*2H2O  (Read 2438 times)

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Offline zanio

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10 %solution of BaCl2*2H2O
« on: March 31, 2018, 01:14:59 AM »
Hi my frends,

I have a question:

How to prepare  1L 10%solution of  BaCl2*2H2O?

Thank you!

Offline sjb

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Re: 10 %solution of BaCl2*2H2O
« Reply #1 on: March 31, 2018, 03:45:18 AM »
What are your thoughts? 10% by what, w/w, v/v, w/v..?

Offline zanio

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Re: 10 %solution of BaCl2*2H2O
« Reply #2 on: March 31, 2018, 06:51:43 AM »

    W/V

Offline Borek

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Re: 10 %solution of BaCl2*2H2O
« Reply #3 on: March 31, 2018, 10:39:40 AM »
You have to show your attempts at solving the problem to receive help, it is a forum policy.
ChemBuddy chemical calculators - stoichiometry, pH, concentration, buffer preparation, titrations.info, pH-meter.info

Offline zanio

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Re: 10 %solution of BaCl2*2H2O
« Reply #4 on: March 31, 2018, 11:22:59 AM »
 It is known that 10 grams of the substance and 90 milliliters of water are required to obtain a 10% solution. or in the case of 1 liter 100 grams of substance and 900 ml. water.
But the problem is that BaCl2 contains 2 molecules of water. they can not calculate and get the desired concentration.

I recently work in a chemical lab and I need a BaCl2 solution to determine the concentration of Na2CO3 in the samples.

Tank you!


Offline Borek

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Re: 10 %solution of BaCl2*2H2O
« Reply #5 on: March 31, 2018, 03:06:17 PM »
If it is to precipitate the carbonate you don't need a really high accuracy, ignore water of crystallization and just calculate how much dihydrate contains enough of just BaCl2.
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Offline zanio

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Re: 10 %solution of BaCl2*2H2O
« Reply #6 on: April 01, 2018, 01:42:07 AM »
Thank you!

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