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| What is the most important solvent on earth? |
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| It is extremely abundant on earth and is has an exceptional ability to dissovle a wide variety of solutes |
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| Why is water the most important solvent on earth? |
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| have no effect on the pH of a solution. |
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Definition
| A cation(Na+, K+) from a strong base or an anion(Cl-, NO3-) from a strong acid will... |
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| A cation from a weak base or an anion from a weak acid will have.... |
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| The cation(NH4+, Al3+) from a WEAK base will produce an......solution |
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| The anion (CH3COO-, CN-, ClO-) from a WEAK acid will produce a .....solution. |
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Definition
| an ion that is produced by more than one solute in a solution |
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Definition
| the equilibrium is shifted by the presence of the common ion. the addition of a common to a solution of a weak electrolyte causes the extent of dissociation of the weak electrolyte to decrease |
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| .....has no resistance to changes in pH. Even if a small amount of acid or base is added to....the pH changes signifacntly |
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Definition
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Definition
| No resistance to change in pH(water has no buffering capacity) |
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Definition
| A solution which does resist a change in pH. |
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Term
| In a buffer, what two species are required? |
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Definition
| either a weak acid and its conjugate base or a weak base and its conjugate acid. |
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| The acid species neutralized...., and the basic species neutralizes...... Because an acid-conjugate base system or a base-conjugate acid system is used, the two species do not neutralized each other. |
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Definition
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| In acidic solution, a ....congjuate base system is used. |
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Definition
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| In basic solution, a .....conjugate acid system is used. |
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Definition
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Term
| Buffers allow small amounts of acid or base to be added to solutions without resulting in... |
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Definition
| significant pH changes. (blood is a buffered solution) |
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Term
| pH depends on two things which are |
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Definition
| 1)Ka and 2) the ratio between the acid and the conjugate base. |
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Term
| Buffers resist changes in pH most effectively when the ratio b/w the acid and the conjugate base is approximately... |
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Definition
| 1!. Or in other words, they resist changes in pH most effectively when the concentrations of the acid and the conjugate base are approximately equal, thus pH=pKa |
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Term
| Buffers are usually selected so that they have a pKz close to the desired... |
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Definition
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Definition
| the amound of acid or base that can be added to a buffer solution before it changes appreciably. |
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Term
| The maximum capacity to resist pH changes exists when the concentrations of weak acid(or base) and its salt are kept large and approximately.... |
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Definition
| equal to one another. The maxium buffering capacity occurs when pH=pKa |
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Term
| Whenever the ratio of salt to acid(or base) is less than about 0.10 or greater than about 10, the buffer loses its capacity. Thus, the buffer is effective for only about... |
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Definition
| 1 pH unit on either side of the value pH=pKa |
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Term
| Rearrangement of the Kz and Kb equations useful in calculations involving.... |
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Definition
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| For a weak acid-conjugate base buffer solution: [H3O+]= |
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Definition
| [acid]/[conjugate base] x Ka |
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Term
| For a weak base-conjuage acid buffer solution: [OH-]= |
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Definition
| [base]/[conjuage acid] x Kb |
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Term
| By taking the negative logarithm of both sides of the acid equation and making the appropriate subsitions, we get... |
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Definition
pH=pKz + log{[conjugate base]/ [acid]}
or Henderson-Hasselbalch equation |
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Term
| A similar equation can be written for basic buffers which is... |
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Definition
| pOH=pKb +log{[conjugate acid/[base]} |
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Term
| The solution pH depends primarily on... |
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Definition
| the acid or base present (pKa or pKb) |
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Term
| When concentrations of acid and conjugate base are equal in solution then pH= |
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Definition
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| If there is more conjugate base then acid, then pH is |
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Definition
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| If there is less conjugate base than acid, the ph is |
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Definition
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