Imagine a solution of two liquids that are so similar that their interactions together are the same as in the individual liquids. will this solution deviate positively from, deviate negatively from, or ideally follow raoult's law?

ideally follow Raoult's law

Explanation:
Raoult's law states that: "the partial vapor pressure of each component of an ideal mixture of liquids is equal to the vapor pressure of the pure component multiplied by its mole fraction in the mixture"

It is given that:
1- the two solutions are similar
2- their interactions together are the same as in the individual liquids

This means that the solution formed will be an ideal solution. This means that the vapor pressure formed will be exactly equal to that predicted by Raoult's law.

Hope this helps :)

m=9

step-by-step explanation:

7m+8=71 subtract   8 from 71 which is 63 than divide it by 7m   equal 9.

                             

Ur e n d is not real