Question

In: Chemistry

Assume you are carrying out the titration of 50 mL of a 0.025 M solution of...

Assume you are carrying out the titration of 50 mL of a 0.025 M solution of acetic acid with 0.1023 MNaOH. Acetic acid has aKaof 1.8×10−5.

(a) Calculate the pH of the solution at V= 0, V= 0.3Veq, V=Veq, and V= 1.2Veq. (Veq is the equivalence point volume)

(b) If a phenolphthalein indicator was used in this titration, where would the apparent endpoint occur? Assume the apparent endpoint would occur at the end of the color range of the indicator (pH’s of 8.0-9.6).

Solutions

Expert Solution



Related Solutions

For the titration of 25 ml of a 0.025 M weak acid solution (pKa = 4.615)...
For the titration of 25 ml of a 0.025 M weak acid solution (pKa = 4.615) with 0.050 M NaOH. What will be the pH and pOH at the Equivlance point?
Consider the titration of 30.0 mL of 0.030 M NH3 with 0.025 M HCl. Calculate the...
Consider the titration of 30.0 mL of 0.030 M NH3 with 0.025 M HCl. Calculate the pH after the following volumes of titrant have been added. (a) 35.0 mL (b) 36.0 mL (c) 37.0 mL
In an acid-base titration experiment, 50 mL of a 0.05 M solution of acetic acid (Ka...
In an acid-base titration experiment, 50 mL of a 0.05 M solution of acetic acid (Ka = 1.75 x 10-5 ) was titrated with a 0.05M solution of NaOH at 25 oC. The system will acquire this pH after addition of 40 mL of the titrant: Answer: 5.36 How do you solve this?
You mix together 25.0 mL of a 0.025 M aqueous solution of copper(II) sulfate and 50.0...
You mix together 25.0 mL of a 0.025 M aqueous solution of copper(II) sulfate and 50.0 mL of 0.01 M sodium phosphate and isolate 68.3 mg of a precipitate. 1.Write the balanced equation for this reaction. Label all states. 2.What is the identity of the precipitate? 3.What is the theoretical yield of the reaction? 4.What is the percent yield of the reaction? You mix together aqueous solutions of 100.0 mL of 0.05 M sodium nitrate and 10.0 mL of potassium...
You carry out the titration of 35.00 mL of 0.1750 M pyridine using a 0.275 M...
You carry out the titration of 35.00 mL of 0.1750 M pyridine using a 0.275 M HCl solution. Pyridine has a pKb = 8.77 What is the pH at: 0 ml HCl added 5.0 ml HCl added half equivalence point for HCl half equivalence point for pyridine 17.0 ml HCl added 21.0 ml HCl added equivalence point 26.0 ml HCl added
Titration of a 15.0 mL solution of KOH requires 17.0 mL of 0.0250 M H2SO4 solution....
Titration of a 15.0 mL solution of KOH requires 17.0 mL of 0.0250 M H2SO4 solution. What is the molarity of the KOH solution? M=?
For the titration of 50.00 mL of a 0.1000 M solution of compound H2SO4 with a...
For the titration of 50.00 mL of a 0.1000 M solution of compound H2SO4 with a 0.2000 M solution of compound NaOH in the following table. For each titration, calculate the pH after the addition of 0.00, 20.00, 25.00, 37.50, 50.00, and 60.00 mL of com- pound NaOH. Please explain all the steps.
For the titration of 50.00 mL of a 0.1000 M solution of compound ethylenediamine with a...
For the titration of 50.00 mL of a 0.1000 M solution of compound ethylenediamine with a 0.2000 M solution of compound HCl in the following table. For each titration, calculate the pH after the addition of 0.00, 20.00, 25.00, 37.50, 50.00, and 60.00 mL of com- pound HCl. Please explain all the steps.
At 25 C, you conduct a titration of 15.00 mL of a 0.0400 M AgNO3 solution...
At 25 C, you conduct a titration of 15.00 mL of a 0.0400 M AgNO3 solution with a 0.0200 M NaI solution within the following cell: Saturated Calomel Electrode || Titration Solution | Ag (s) For the cell as written, what is the voltage after the addition of the following volume of NaI solution? The reduction potential for the saturated calomel electrode is E = 0.241 V. The standard reduction potential for the reaction Ag+ + e- --> Ag(s) is...
50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of 2.0 M methylamine hydrochloride (CH3NH3Cl)...
50. mL 2.0 M methylamine (CH3NH2) solution and 50. mL of 2.0 M methylamine hydrochloride (CH3NH3Cl) solution. The Kb for methylamine is 4.4 x 10-4. What is the pH of the resulting solution after adding 100 mL of 1.0 M KOH to the original buffer solution? 11.12                           b) 10.64                       c) 12.32                       d) 0.48                         e) 5.32
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT