pH is a measure of the acidity or basicity of an aqueous solution. It's defined as the negative logarithm of the hydrogen ion concentration ($[H^+]$). In simpler terms, pH tells us how many hydrogen ions are floating around in a liquid – the more there are, the more acidic it is, and the lower the pH value. Remember that pH values range from 0 to 14, with 7 being neutral. Solutions with pH less than 7 are acidic, and those with pH greater than 7 are basic (or alkaline). Mastering pH calculations is crucial for success in AP Chemistry!
Let's boost your pH skills with some practice!
Match the terms with their definitions:
| Term | Definition |
|---|---|
| 1. pH | A. A substance that accepts protons. |
| 2. Acid | B. The negative logarithm of the hydrogen ion concentration. |
| 3. Base | C. A substance that donates protons. |
| 4. Titration | D. A solution that resists changes in pH. |
| 5. Buffer | E. A process used to determine the concentration of a solution. |
(Match the numbers 1-5 to the letters A-E)
Complete the following paragraph with the correct words:
A strong acid completely ______ in water, producing a high concentration of ______ ions. A strong base completely dissociates to produce ______ ions. Weak acids and bases only partially ionize, meaning they reach an ______ where both the ionized and unionized forms are present.
(Possible words: equilibrium, hydroxide, hydrogen, dissociates)
Explain why understanding pH is important in biological systems. Give at least two specific examples.
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