Oceanography Acids and bases Worksheet Questions

Exploring Acids and Bases

In class, you learned that pH is inversely related to the concentration of H⁺ ions by the following equation: pH = -log[H⁺].  Lower pH values have higher [H⁺] while high pH values have lower [H⁺].  Acids have a lot of H⁺ ions and donate them to other molecules.  Bases accept H⁺ ions.  We will explore this relationship further using an online simulation of acid-base solutions.

1. Please go to the following website: http://goo.gl/V0YcK

2. This should take you to an acid-base solutions simulation. Click download.

3. First, we will study the solutions under the "Introduction" tab.  To measure the pH, simply click on the gray box labeled "pH" and drag it into the solution.

4. Finally, you create your own acids and bases using the "Custom Solution" tab.

Water

The concentration of H₃O⁺ ions is _________ than OH^- ions.  Therefore the pH of the solution is ____.

Strong Acid

The concentration of H₃O⁺ ions is _________ than A^- ions.  Therefore the pH of the solution is ____.

Weak Acid

The concentration of H₃O⁺ ions is _________ than A^- ions.  Therefore the pH of the solution is ____.

Strong Base

The concentration of M⁺ ions is _________ than OH^- ions.  Therefore the pH of the solution is ____.

Weak Base

The concentration of M⁺ ions is _________ than OH^- ions.  Therefore the pH of the solution is ____.

Custom Solutions

1. For a weak acid, what is the pH of a 0.01 mol/L solution?

2. What concentration of H₃O⁺ ions would you need for the solution's pH to be 6.50? (First use the sliding scales to manipulate the concentration and strength of the acid to the desired pH. Then use equilibrium view to find the [H₃O⁺].)

3. How would you decrease the pH of this solution to 5.00? 

4. For a weak base, what is the pH of a 1.000 mol/L solution?

5. What happens to the solution's pH when you decrease the concentration of OH^- ions?