How would you prepare 100 ml of 0.4 m mgso4 from a stock solution of 2 m mgso4? my attempt at answering this: using the formula (vi)(mi)=(vf)(mf) (vi)(2m)=(100)(0.4)=200-100(final volume)=100 ml i am assuming you would add 100 ml of water to the 2 m mgso4 200 ml to get the 0.4 m mgso4 100 ml

To prepare 0.4M, 100 ml of solution, 20 ml of the 2 M stock has to be taken, and the volume has been makeup to 100 ml with the solvent.

To prepare the diluted solution from the stock solution, the amount of stock solution required will be calculated as:

M1V1 = M2V2

Where M1 and V1 are the molarity and the volume of stock

M2 and V2 are the molarity and volume of solution to be prepared.

100 ml 0.4 M = Volume of stock 2 M

Volume of stock = 20 ml

Thus to prepare 0.4M 100 ml of solution, 20 ml of the 2 M stock has to be taken, and the volume has been makeup to 100 ml with the solvent.

For more information about molarity, refer to the link:

link

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.