anonymous
  • anonymous
There are two solutions. Same compounds, and same number of moles. Only difference is, in one solution the compound is dissolved to make 1L of solution while in the other one, the compound is added to make 1 L of water. Is the molarity the same.
Chemistry
jamiebookeater
  • jamiebookeater
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anonymous
  • anonymous
what sol would you be talking about?
anonymous
  • anonymous
well i dont think it matters. Because they give the same concentration, although im not sure which one has a greater molarity
anonymous
  • anonymous
well... no i do not think the molarity is the same water has a very stable pH

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anonymous
  • anonymous
it is very neutral
anonymous
  • anonymous
is there anything to do with the process. One is being dissolved and the other is added.
JFraser
  • JFraser
Molarity is a specific term of concentration. The molarity is not the same, so the concentrations are not the same.
anonymous
  • anonymous
If the ammount of moles and the amount of litters are the same then they are the same concentration regardless how you get there. \[M=\frac{moles}{litters}\]
JFraser
  • JFraser
But the liters AREN'T the same. I do this demonstration all the time. If you start with 1L of water and dissolve a solute in it, the apparent volume of the solution increases. A second container with less water in it will fill up to the 1L mark. One of the solutions has 1L of WATER, the other has 1L of SOLUTION. The concentrations are different.
anonymous
  • anonymous
I agree with what you are saying for that situation. However, the question says the only difference was the way the solution was made, meaning that everthing else is the same. Therefore the amount of moles in solution is the same as the litters of soluate which would mean the molarity is the same.
JFraser
  • JFraser
"in one solution the compound is dissolved to make 1L of solution while in the other one, the compound is added to make 1 L of water." To me, that says the 2 solutions contain different volumes of solvent.

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