Lesson 1.2A Vocabulary Words
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
on it to display the answer.
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| 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
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| 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
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| 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
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| hemoglobin | An iron-containing protein in red blood cells that reversibly binds oxygen
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| 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
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| hydrophilic | water-loving molecules that are polar in nature (such as salt (sodium chloride) in water).
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| hydrophobic | water-phobic molecules that are non-polar
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| lubricant | A fluid used to reduce friction by creating a thin layer between microscopic "hills and valleys" of a surface.
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| pH | relative strength of an acid
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| polarity | Any separation of charge into distinct positive and negative regions.
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| solvent | liquid component of a solution
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| 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.
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| 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 _____ _____.
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| sigma | negative charge
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| sigma + | positive charge
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| (NaCl) | sodium chloride (salt)
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| H2O | water - 2 hydrogen (H) molecules + 1 oxygen (O) molecule
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| HCl | Hydrochloric Acid
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| NaOH | sodium hydroxide - strong base
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| H2CO3 | carbonic acid - weak acid
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| HCO3 | bicarbonate ions - weak acid
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| 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.
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| 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
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| 3. What would be the pH of the water BEFORE adding an acid? | pH of 7
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| 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.
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| 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.
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To hide the entire table, click on the "Hide All" button.
You may also shuffle the rows of the table by clicking on the "Shuffle" button.
Or sort by any of the columns using the down arrow next to any column heading.
If you know all the data on any row, you can temporarily remove it by tapping the trash can to the right of the row.
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