[Karatekboy]

A student wants to prepare 100.0 mL of a 0.100 M NaCl solution and has available the following:1. A bottle of reagent grade NaCl, 2. 2.00 L of 0.0500 M NaCl, and 3. 2.00 L of 1.00 M NaCl. (A) Can the student readily prepare the desired solution from each sample of NaCl by itself and with water? Justify your response. (B) In words outline how the student could prepare the desired solution based on your responses to a.
*Any help with answering this problem or I would go about solving this problem is much obliged.

[Hunter2]

What is your opinion first. Of course its possible with 2 of the given samples. Which ones?

[AWK]

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[Arkcon]

You have some work to do, but I'd like to say, "Boy, what an obtuse question, your teacher has given you."

Can you make the solution, yes or no.
Prove it.
Write out the procedure in words.

A dumb question, and the same explanation twice.  Well, this is what you have to work with.

[Karatekboy]

I'm just having trouble with the reagent grade NaCl because I don't know what the molar its of it is. I would assume 1.00 M because it is pure NaCl but it says that there is already 1.00 M solution that I can use.

[AWK]

NaCl reagent grade is solid? Usually contains >99% NaCl.

[Arkcon]

There is no "molar" for a dry solid, if I take the sense in which you mean it.  It has no "molarity" because its not a solution of any concentration, which is how molarity I defined.  It does have a molar mass, which you can look up or compute to make a solution I a certain molarity.

[Karatekboy]

That makes more sense. I was under the assumption that it was a liquid since it said a bottle of it but now I understand, thank you.