Molarity and Dilution G23

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Rodrigo2J
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Molarity and Dilution G23

Postby Rodrigo2J » Sat Oct 05, 2019 6:21 pm

G23) A lab technician has made up 100.0 mL of a solution containing 0.50g NaCl and 0.30g KCl, as well as glucose and other sugars. What is the concentration of chloride ions in the solution?
I understand that I need to find a solution that is in L/mol (molarity) and to do that, I have to convert 0.50g NaCl and 0.30g KCl into moles of Cl-. I'm just wondering if we assume that only these two molecules are the ones we are using to calculate the molarity or if we have to use glucose for some kind of conversion factor to solve.

Katherine Wu 1H
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Re: Molarity and Dilution G23

Postby Katherine Wu 1H » Sat Oct 05, 2019 7:05 pm

just assume that NaCl and KCl are the only two you're using

Sofia Barker 2C
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Re: Molarity and Dilution G23

Postby Sofia Barker 2C » Wed Oct 09, 2019 12:44 am

The question is asking for the concentration of chloride ions in the solution. The solution is made up of NaCl, KCl, and sugar. Sugars do not contain any chloride ions, thus it is implied that the chloride ions within NaCl and KCl are the only ions to take into account when solving for concentration.

Chem_Mod
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Re: Molarity and Dilution G23

Postby Chem_Mod » Wed Oct 09, 2019 9:36 am

You may assume that the sugars do not contain chloride ions, they also do not give you amounts of the sugars so you cannot find moles of each either. One thing to note though is that molarity is mol/L, not L/mol.


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