1. Suppose you did not line up the buret tip with the eye of the drop counter an
ID: 529189 • Letter: 1
Question
1. Suppose you did not line up the buret tip with the eye of the drop counter and missed several drops of the base. What effect will this have on the value of the pKa? Explain.2. Suppose you accidentally used pH 4 buffer instead of pH 7 buffer when calibrating the pH electrode. What effect will this have on the value of the pKa? Explain.
3. Sketch the Titration curves for each of the following systems. Calculate the value and indicate the location on the sketch; the equivalence point, initial pH of the solution, and at least one other significant point on the Titration curve. a) 10.00 mL of 0.00500 N HNO3 titrated with 0.100 N NaOH b) 10.00 mL of 0.0500 N benzoic acid titratwd with 0.100 N NaOH 1. Suppose you did not line up the buret tip with the eye of the drop counter and missed several drops of the base. What effect will this have on the value of the pKa? Explain.
2. Suppose you accidentally used pH 4 buffer instead of pH 7 buffer when calibrating the pH electrode. What effect will this have on the value of the pKa? Explain.
3. Sketch the Titration curves for each of the following systems. Calculate the value and indicate the location on the sketch; the equivalence point, initial pH of the solution, and at least one other significant point on the Titration curve. a) 10.00 mL of 0.00500 N HNO3 titrated with 0.100 N NaOH b) 10.00 mL of 0.0500 N benzoic acid titratwd with 0.100 N NaOH
2. Suppose you accidentally used pH 4 buffer instead of pH 7 buffer when calibrating the pH electrode. What effect will this have on the value of the pKa? Explain.
3. Sketch the Titration curves for each of the following systems. Calculate the value and indicate the location on the sketch; the equivalence point, initial pH of the solution, and at least one other significant point on the Titration curve. a) 10.00 mL of 0.00500 N HNO3 titrated with 0.100 N NaOH b) 10.00 mL of 0.0500 N benzoic acid titratwd with 0.100 N NaOH
Explanation / Answer
Ans 1.
pKa is the strength of any acid which is defined as the negative logarithm of acid dissociation constant of the acid.
Smaller the pKa value , stronger is the acid .
If you did not line up the eye of buret tip with the eye of the drop counter and missed several drops of base , you will get a false burett reading of the base , which will be higher than what it should be and hence the calculated value of pKa for the acid will be lower.
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