How can a chemist accurately prepare a solution of precise molarity?

Answer 1

This is necessary because we need solutions with an exact molar concentration. Serious experiments in chemistry and application of analytical chemistry methods are possible only having data about masses, volumes, concentrations of compounds.

Answer 2

A chemist's preparation of a precise molar solution is based upon the following criteria. First, the substance being solvated must be of known purity and precise mass. Accordingly the chemist's mass instrumentation must be correctly calibrated and zeroed. Second, the volume of water needs to be precisely measured to ensure the molar yield is reached. Third, the solution must be thoroughly (and possibly actively) mixed to ensure equal molar concentration throughout the solution.

Answer 3

In addition to the molar concentration, you need to know the volume of solution desired and the molar mass (gram/mole) of the substance. Then, molar concentration = mole/liter and with the known volume, you calculate as follows:
mole/liter x liter x gram/mole = grams. Measure out the calculated grams and dissolve in enough solvent to make the final volume.

Answer 4

with salt: 5.8 grams + 100 ml of distilled water

with sugar: 34 grams + 100 ml of distilled water

Answer 5

Dissolve one mole of the substance in 1 litre demineralized water at 20 oC.