Term
| Arrhenius concept of Acid and bases |
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Definition
| Acids are substances that, when desolved in water increase the concentration of H+ ions. Likewise bases are subsances that, when desolved in water, increase the concentration of OH- ions. |
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Term
| Bronsted Lowery concept of Acid and Base |
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Definition
| An acid is a substance (molecule or ion) that can donate a proton to another substance. Likewise a base is a substance that can accept a proton. |
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Term
| Lewis concept of acid and bases |
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Definition
| A lewis acid is a electron pair acceptor and a lewis base is a electron pair doner. |
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Term
| Lewis concept of acid and bases |
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Definition
| A lewis acid is a electron pair acceptor and a lewis base is a electron pair doner. |
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Term
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Definition
| Is simply a proton with no surrounding valence electrons. |
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Term
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Definition
| A substance that can act as either an acid or a base in a reaction. It acts as a base with something more acidic than itself and as a acid with something more basic than itself. It all depends on the pH level. |
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Term
| Does the Bronsted Lowery definitions apply to non aqueous solutions? |
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Definition
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Term
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Definition
| a molecule or ion must have a nonbonded pair or electrons that it can use to bind the H+ ion |
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Term
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Definition
| a molecule or ion must have a hydrogen atom it can lose as an H+ ion. |
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Term
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Definition
| Dissociates completely in H2O, hence there is a single arrow --> not equilibrium <-> |
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Term
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Definition
| These completely transfer their protons to water leaving no undissociated molecules in the solution. Their conjugate bases have a negligible tendency to be protonated (to abstract protons) in aqueous solution |
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Term
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Definition
| These only partially dissociate in aqueous hence they exist in a solution as a mixture of acid ions and constituent ions. The conjugate bases of weak acids show a slight ability to remove protons from water. |
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Term
| The conjugate acids of weak bases |
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Definition
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Term
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Definition
| Are those that contain hydrgen but do not demonstrate any acidic behavior in water. Hence their conjugate acids are strong bases. |
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Term
| In every acid/ base reation the position of the equilibrium favors |
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Definition
| the transfer of the proton to the stronger base |
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Term
| Ion product constant for water |
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Definition
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Term
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Definition
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Term
Acid [H+] >
Base [OH+] >
Hence the pH decreases as |
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Definition
Acid [H+] > 1.0x10^-7
Base [H+] < 1.0x10^-7
as the [H+] increases |
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Term
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Definition
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Term
| According to pH and Acid is |
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Definition
[H+](M) [OH-](M) pH value
>1.0x10^-7 <1.0x10^-7 <7.00 |
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Term
| According to pH an Acid is |
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Definition
| [H+](M)>1.0x10^-7 [OH-](M)<1.0x10^-7 pH value <7.00 |
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Term
| According to pH a Neutral is |
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Definition
| [H+](M)=1.0x10^-7 [OH-](M)=1.0x10^-7 pH value =7.00 |
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Term
| According to pH a Base is |
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Definition
| [H+](M)<1.0x10^-7 [OH-](M)>1.0x10^-7 pH value >7.00 |
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