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BIO 12-MOD1/1.2A
Lesson 1.2A Vocabulary Words
| Term | Definition |
|---|---|
| acids | (pH too low, such as in a fish tank- yellowy-green when tested) (too much H+) compounds that form hydrogen ions when dissolved in water |
| bases | (alkalinity - pH too high, such as in a fish tank- very blue when tested) molecules that either release hydroxide ions (OH-) or take up hydrogen ions (H+); bases have a pH greater than 7 |
| buffer | a compound or combination of compounds (often a weak acid or base and a related salt) that keeps the pH of a solution within its normal limits |
| hemoglobin | An iron-containing protein in red blood cells that reversibly binds oxygen |
| hydrogen bonding | weak bond that arises between a slightly positive hydrogen atom of one molecule and a slightly negative atom of another molecule or between parts of the same molecule |
| hydrophilic | water-loving molecules that are polar in nature (such as salt (sodium chloride) in water). |
| hydrophobic | water-phobic molecules that are non-polar |
| lubricant | A fluid used to reduce friction by creating a thin layer between microscopic "hills and valleys" of a surface. |
| pH | relative strength of an acid |
| polarity | Any separation of charge into distinct positive and negative regions. |
| solvent | liquid component of a solution |
| temperature regulator | Water acts as this by using its numerous hydrogen bonds to resist temperature changes, also evaporation of sweat helps cool the human body. |
| covalent bond | is a chemical bond that involves the sharing of electron pairs between atoms. The stable balance of attractive and repulsive forces between atoms when they share electrons is known as _____ _____. |
| sigma | negative charge |
| sigma + | positive charge |
| (NaCl) | sodium chloride (salt) |
| H2O | water - 2 hydrogen (H) molecules + 1 oxygen (O) molecule |
| HCl | Hydrochloric Acid |
| NaOH | sodium hydroxide - strong base |
| H2CO3 | carbonic acid - weak acid |
| HCO3 | bicarbonate ions - weak acid |
| 1. What happens to the concentration of hydrogen ions (H+) in a beaker of pure water when an acid is added to it? | The concentration of H+ increases as acid is added to pure water. |
| 2. Give an example of a name and chemical formula of an acid. | Answers will vary but the acid must have a hydrogen atom at the front of the formula. An example would be hydrochloric acid HCl |
| 3. What would be the pH of the water BEFORE adding an acid? | pH of 7 |
| 4. What happens to the pH of the solution as you add an acid to it? | The pH of the solution will continue to decrease as you add acid to it. Acids have a pH of less than 7. The lower the number, the stronger the acid. |
| 5. If you begin with pure water that has a pH of 7 and add an acid until the solution had a pH of 4, how many more times acidic is the new solution compared to the pure water? | 1000 times. Each number on the pH scale represents an increase the acidity by 10X. Dropping the pH from 7 to 4 moves three numbers on the pH scale: 10 X 10 X 10 = 1000 times more acidic. |
Created by:
WOOLGIRL
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