Prepare 600mL of a 100mM solution of glucose in 0.9% NaCl. Also need to prepare the 0.9% NaCl solution.

And the 0.9% is w/w, w/v, ??

it doesn't say but I'm assuming its w/v

Is this an isotonic something or other?

I'm not sure the only help my professor gave for this question is as follows...

Make a liter of 0.9%NaCl in water. The result for grams of NaCl to add to the water I want in one sig fig. Then use 600 mL of the 0.9% NaCl you prepared as the solvent to make a 100mM Glucose solution. Amount of glucose required is expressed in 3 sig figs. This is how this solution would likely be prepared in most labs.

Yes, a 0.9% NaCl w/v is an isotonic solution.

Your prof wants 1L so wouldn't 0.9 g NaCl/100 mL solution be correct or 9 g/L of soln? That gets your 1 L of 0.9% w/v NaCl.
Look up the molar mass glucose, you want how many moles glucose? That will be---
you want 100 mM which is 0.1M and moles = M x L = 0.1M x 0.6L = xx moles glucose.
moles = grams/molar mass so solve for grams glucose. From your prof's explanation, youy drop about 10.8 g in 600 mL of th solvent and dissolve all of the glucose. This will NOT prepare EXACTLY 100 mM although it will be close. I don't know how much flexibility you have. As an analytical chemist, if someone told me to do this, I would weigh the glucose, drop in a container, and MAKE TO A FINAL VOLUME of 600 mL (although I know 600 mL volumetric flasks are difficult(if not impossible) to come by). If I couldn't find one I would make up a L of solution or 500 mL of solution for which volumetric flasks are available. Anyway, you get the idea. I suspect, although I don't know, that the volume will change so little by adding about 11 g glucose that the osmotic pressure will be essentially isotonic with the solutions to be analyzed.

Dr. Bob seriously you have saved me and I am very thankful that there are people like you out there who wish to help others!!!!!

To prepare 600mL of a 100mM solution of glucose in 0.9% NaCl, you will need to follow a step-by-step process.

First, let's calculate the amount of glucose and 0.9% NaCl needed for the solution.

Step 1: Determine the amount of glucose:
To prepare a 100mM solution of glucose, we need to know the molar mass of glucose. The molar mass of glucose (C6H12O6) is approximately 180.16 g/mol.

To calculate the weight of glucose needed, use the formula:
Weight of glucose (g) = Volume of solution (L) × Concentration (mol/L) × Molar mass (g/mol)

In this case, the volume is given as 600 mL, but it is better to convert it to liters:
Volume of solution (L) = 600 mL × 1 L/1000 mL = 0.6 L

Next, we need to calculate the concentration in mol/L:
Concentration (mol/L) = 100 mM × 1 mol/1000 mM = 0.1 mol/L

Now, we can calculate the weight of glucose needed:
Weight of glucose (g) = 0.6 L × 0.1 mol/L × 180.16 g/mol

Step 2: Prepare the 0.9% NaCl solution:
To prepare the 0.9% NaCl solution, we need to determine the weight of NaCl required.

The weight of NaCl in a 0.9% solution is given by the equation:
Weight of NaCl (g) = Volume of solution (mL) × Concentration (%w/v) × 1 g/100 mL

Since the volume for both the glucose solution and the 0.9% NaCl solution is the same (600 mL), we can use the same value for the volume.

Now, use the equation to calculate the weight of NaCl:
Weight of NaCl (g) = 600 mL × 0.9 g/100 mL

Finally, we are ready to prepare the solutions.

Step 3: Preparation of the solutions:
a) Glucose Solution:
To prepare the glucose solution, dissolve the calculated weight of glucose in distilled water to make a total volume of 600 mL. Mix it thoroughly until the glucose is completely dissolved. Avoid using normal saline (0.9% NaCl solution) to dissolve the glucose, as it might result in an inaccurate concentration due to interaction between glucose and NaCl.

b) 0.9% NaCl Solution:
To prepare the 0.9% NaCl solution, dissolve the calculated weight of NaCl in distilled water to make a total volume of 600 mL. Mix it until the NaCl is completely dissolved.

Ensure that both solutions are properly labeled and stored in appropriate containers for future use.

Note: It is always important to practice proper laboratory techniques and consult safety protocols when working with chemicals and solutions.