Term
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Definition
| an acid is any substance (molecule or ion) that can transfer a proton (+H ion) to another substance, and a base is any substance that can accept a proton. |
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| Acids are proton _________ |
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| Bases are proton ________ |
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Definition
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| acid-base reactions are ________ |
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Definition
| proton-transfer reactions |
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Term
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Definition
| a substance that can transfer H+ |
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Definition
| a substance that can accept H+ |
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| conjugate acid-base pairs |
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Definition
| species whose formulas differ only by one proton |
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Definition
| Product of Bronsted-Lowery reaction. (the conjugate aid of H2O) |
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Term
| for a molecule or ion to accept a proton, it must _________________. All bronsted-lowery bases have this. |
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Definition
| it must have at least one unshared pair of electrons that it can use for bonding to the proton. |
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Definition
| one that is almost completely dissociated in water and is therefore a strong electrolyte |
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Definition
| substance that dissolves in water to produce solutions that conduct electricity |
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Definition
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Definition
| Hydrochloric Acid (strong) |
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Definition
| Hydrobromic acid (strong) |
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Definition
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| strong acids have very ______ conjugate bases |
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Definition
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Definition
| one that is only partially dissociated in water and is thus a weak electrolyte |
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Definition
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Definition
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Definition
| very weak acid that dont transfer protons which let the acid dissociation equilibrium lie 100% to the left. |
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Term
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Definition
| refers to the power of 10 (the exponent) used to express the molar H3O+ concentration. |
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