Answer to Question #172696 in General Chemistry for Ashley

Question

1. Compare the concentration of OH-​ ​ and H​3O​ +​ ​ in a neutral solution.

2. In terms of ion concentrations, how are basic solutions different from acidic solutions?

3. Compare the concentration of OH─​ ​ and H​3O​ +​ ​ in an acidic solution.

4. What happens to the H​3O​ +​ ​ concentration as pH decreases?

5. What is the pH of a solution that has a hydronium ion concentration 100 times greater than a solution with a pH of 4?

(1) 5 (2) 3 (3) 2 (4) 6

6. Identify a possible pH of an acidic solution.

7. Identify a possible pH of a basic solution.

Answer 1

1.When there is a reaction in an aqueous solution, the water molecules have the ability to attract and temporarily hold a donated proton (H+). This creates the hydronium ion (H3O+). In an acidic aqueous solution, the concentration of hydronium ions will be higher than the concentration of hydroxide (OH-) ions.

2.An acidic solution has a high concentration of hydrogen ions (H +start superscript, plus, end superscript), greater than that of pure water. A basic solution has a low H +start superscript, plus, end superscript concentration, less than that of pure water.

3.The higher the concentration of OH- in a solution, the more basic the solution is. Pure water undergoes a reversible reaction in which both H+ and OH- are generated.

4.As H+ ions dissociate from the acid and bond with water, they form hydronium ions, thus increasing the hydronium concentration of the solution.

5.$pH of below 3 to 1$

6.Any pH below 7

7.All pH above 7