You need to prepare 250. ml of a 0.150 m aqueous solution of sucrose, c12h22o11(aq), which is used frequently in biological experiments.

The complete question is in the picture below

Explanation:

a) Type of glassware to use

It's always better to use the volumetric ball, because it's very important to be accurate . You can use another glassware to make the measures of water to be more accurate but, to stock this solution, it's always better the volumetric ball.

b) Correct amount of solute to use:

In this case, the sucrose, is a solid compound, therefore, the best way to measure this is using a balance and weight the required mass basing on the concentration of the solution. So, it's best to measure out the grams of solute in a balance.

The amount needed is the following:

M = n/V

n = M*V

n = 0.150 * 0.250 = 0.0375 moles

to get the mass:

m = n*MM

The molar mass of sucrose is 342.3 g/mol so:

m = 0.0375 * 342.3

m = 12.84 g

c) How the solute and solvent be mixed

Finally for this part, now that you have weight the mass of sucrose needed, all you have to do is put the solute on the volumetric ball, and add some water. This way, the sucrose will mix with the water and become a solution. Then, you should complete the volume to 250 mL to get the solution at 0.150 M.

your answer would be “dry”