16. Exactly 25.00 ml of 0.0685 M HClO4 solution is placed in a flask and titrated with standardized 0.050M NaOH.
A. Determine the endpoint of the titration
B. Determine the pH of the solution after the following amounts of NaOH are added to the acid solution:
a.) Initially, 0.00 ml NaOH. b.) 5.00 ml c.) 15.00 ml
d.) 25.00 ml e.) 34.00 ml f.) At the endpoint of the titration
g.) 34.35 ml h.) 45.00 ml i.) 50.00 ml
17. Exactly 25.00 ml of a 0.0685 M pentanoic acid solution,(C4H8O2), is placed in a flask and titrated with standardized 0.050 M NaOH. (the pKa of this acid is 4.84).
A. Determine the endpoint of the titration
B. Determine the pH of the solution after the following amounts of NaOH are added to the acid solution:
a.) Initially, 0.00 ml NaOH. b.) 5.00 ml c.) 15.00 ml
d.) 25.00 ml e.) 34.00 ml f.) At the endpoint of the titration
g.) 34.35 ml h.) 45.00 ml i.) 50.00 ml
18. Make a labeled rough sketch of pH vs. ml of NaOH for the titrations performed in questions #16 and #17
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16. Exactly 25.00 ml of 0.0685 M HClO4 solution is placed in a flask and titrated...
Exactly 25.00 ml of a 0.0685 M pentanoic acid solution,(C4H8O2), is placed in a flask and titrated with standardized 0.050 M NaOH. (the pKa of this acid is 4.84). A. Determine the endpoint of the titration B. Determine the pH of the solution after the following amounts of NaOH are added to the acid solution: a.) Initially, 0.00 ml NaOH. b.) 5.00 ml c.) 15.00 ml d.) 25.00 ml e.) 34.00 ml...
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A solid weak acid is weighed, dissolved in water and diluted to exactly 50.00 ml. 25.00 ml of the solution is taken out and is titrated to a neutral endpoint with 0.10 M NaOH. The titrated portion is then mixed with the remaining untitrated portion and the pH of the mixture is measured. Mass of acid weighed out (grams) 0.762 Volume of NaOH required to reach endpoint: (ml) 18.0 pH of the mixture (half neutralized solution) 3.15 Calculate the following...
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