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To a solution containing equimolar mixture of sodium acetate and acetic acid, some more amount of sodium acetate solution is added. The pH of mixture solution
- a)increases
- b)decreases
- c)remains unchanged
- d)unpredictable
Correct answer is option 'C'. Can you explain this answer?
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Most Upvoted Answer
To a solution containing equimolar mixture of sodium acetate and aceti...
Acetic acid and its conjugate base (acetate) form a buffer solution. A buffer solution resists changes in pH when small amounts of acid or base are added to it. The pH of a buffer solution is determined by the equilibrium constant (Ka) of the weak acid and the ratio of the weak acid and its conjugate base in the solution.
When an equimolar mixture of sodium acetate and acetic acid is prepared, the solution is at its buffering capacity. If more sodium acetate is added to this solution, the following changes occur:
1. The concentration of acetate ions (conjugate base) in the solution increases. This is because sodium acetate dissociates in water to form acetate ions and sodium ions.
NaC2H3O2 → Na+ + C2H3O2-
2. The concentration of acetic acid decreases. This is because some of the acetic acid molecules react with the additional acetate ions to form more sodium acetate.
C2H4O2 + OH- → C2H3O2- + H2O
C2H4O2 + C2H3O2- → 2C2H3O2- + H+
3. The ratio of the weak acid and its conjugate base in the solution shifts towards the conjugate base. This is because the concentration of the conjugate base increases while the concentration of the weak acid decreases.
4. The pH of the solution remains unchanged. This is because the equilibrium constant (Ka) of acetic acid is relatively small, and the ratio of the weak acid and its conjugate base in the solution is still within the buffering range. Therefore, the pH of the solution is still determined by the Ka of acetic acid and the ratio of the weak acid and its conjugate base in the solution.
Hence, the correct answer is option 'C' - the pH of the mixture solution remains unchanged.
When an equimolar mixture of sodium acetate and acetic acid is prepared, the solution is at its buffering capacity. If more sodium acetate is added to this solution, the following changes occur:
1. The concentration of acetate ions (conjugate base) in the solution increases. This is because sodium acetate dissociates in water to form acetate ions and sodium ions.
NaC2H3O2 → Na+ + C2H3O2-
2. The concentration of acetic acid decreases. This is because some of the acetic acid molecules react with the additional acetate ions to form more sodium acetate.
C2H4O2 + OH- → C2H3O2- + H2O
C2H4O2 + C2H3O2- → 2C2H3O2- + H+
3. The ratio of the weak acid and its conjugate base in the solution shifts towards the conjugate base. This is because the concentration of the conjugate base increases while the concentration of the weak acid decreases.
4. The pH of the solution remains unchanged. This is because the equilibrium constant (Ka) of acetic acid is relatively small, and the ratio of the weak acid and its conjugate base in the solution is still within the buffering range. Therefore, the pH of the solution is still determined by the Ka of acetic acid and the ratio of the weak acid and its conjugate base in the solution.
Hence, the correct answer is option 'C' - the pH of the mixture solution remains unchanged.
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To a solution containing equimolar mixture of sodium acetate and aceti...
On adding sodium acetate to the solution , there is no change in ph of solution because solution acts as a buffer solution which does not change its ph on adding or removing any compound. Buffer solutions has a constant value of ph which cannot be changed.
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To a solution containing equimolar mixture of sodium acetate and acetic acid, some more amount of sodium acetate solution is added. The pH of mixture solutiona)increasesb)decreasesc)remains unchangedd)unpredictableCorrect answer is option 'C'. Can you explain this answer?
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