Which of the following is true about the properties of aqueous solutions?

A. A pH change from 5.0 to 6.0 reflects an increase in the hydroxide ion concentration ([OH-]) of 20%

B. A pH change from 8.0 to 6.0 reflects a decrease in the proton concentration ([H+]) by a factor of 100

C. Charged molecules are generally insoluble in water

D. Hydrogen bonds form readily in aqueous solutions

E. The pH can be calculated by adding 7 to the value of the pOH

Answer: d. Hydrogen bonds forma readily in aqueous solutions.

Explanation: pH is a logarithmic scale which means that a change of 1 unit on it equlas a change of 1 order of magnitude (1, 10, 100 etc) in the concentration of [H+] or [OH-] depending on if we are talking of pH or pOH. So a its not correct. And b is not correct either because when pH decrease, H + concentration increase.

On the other hand, water is a dipolar molecule so it has negative and positive charge and dissolves easily charged molecules. This difference in charge occurs because oxygen atoms have free electrons arround that make them negative and hydrogen atoms give electrons so they remain positive. Taking into account that opposite charges attract each other, the positive hydrogen of one molecule stay closer to oxygen of other because of charge affinity. Thats haw hydrogen bonds are formed and water facilitated them.