A titration was performed using a 25.00 mL sample of 0.15 M weak acid and 0.092 M strong base.What was the pH 5.00 mL after the equivalence point was reached?REPORT YOUR ANSWER TO 2 DECIMAL PLACES. DO NOT INCLUDE UNITS.× 12.40

Step 1: To determine the pH after the equivalence, point in a titration of a weak acid with a strong…

Answered: A titration was performed using a 25.00…

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.102E

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Three students titrate different samples of the same solution of HCI to obtain its molarity. Below are their data. Student A: 20.00mLHCl+20.00mLH2O 0.100 M NaOH used to titrate to the equivalence point Student B: 20.00mLHCl+40.00mLH2O 0.100 M NaOH used to titrate to the equivalence point Student C: 20.00mLHCl+20.00mLH2O 0.100 M Ba(OH)2 used to titrate to the equivalence point. All the students calculated the molarities correctly. Which (if any) of the following statements are true? (a) The molarity calculated by A is half that calculated by B. (b) The molarity calculated by A is equal to that calculated by C. (c) The molarity calculated by B is twice that calculated by C. (d) The molarity calculated by A is twice that calculated by B. (e) The molarity calculated by A is equal to that calculated by B.
Consider the nanoscale-level representations for Question 110 of the titration of the aqueous weak acid HX with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: After a very small volume of titrant has been added to the initial HX solution? When enough titrant has been added to take the solution just past the equivalence point? Halfway to the equivalence point? At the equivalence point? Nanoscale representations for Question 110.
A solution of sodium cyanide, NaCN, has a pH of 12.10. How many grams of NaCN are in 425 mL of a solution with the same pH?
Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong acid HA with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: (a) After a very small volume of titrant has been added to the initial HA solution? (b) Halfway to the equivalence point? (c) When enough titrant has been added to take the solution just past the equivalence point? (d) At the equivalence point? Nanoscale representations for Question 111.
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
A student is given 0.930 g of an unknown acid, which can be either oxalic acid, H2C2O4, or citric acid, H3C6H5O7. To determine which acid she has, she titrates the unknown acid with 0.615 M NaOH. The equivalence point is reached when 33.6 mL are added. What is the unknown acid?
You are given the following acidbase titration data, where each point on the graph represents the pH after adding a given volume of titrant (the substance being added during the titration). a What substance is being titrated, a strong acid, strong base, weak acid, or weak base? b What is the pH at the equivalence point of the tiration? c What indicator might you use to perform this titration? Explain.
A student titrated 28.32 ml of a 0.118 M HCl solution with a NaOH solution of unknown concentration. After adding 36.35 ml of NaOH solution, the student realized that she had neglected to add the phenolphthalein indicator solution before starting the titration. When he/she added the phenolphthalein solution, the titration mixture turned bright pink. The student added 4.47 ml of HCl solution to cause the titration mixture to just become colorless. What is the molarity of the NaOH solution? (Put your answer in 3 significant figures)
A 0.2897-g sample of an unknown monoprotic acid is dissolved in water and titrated with standardized barium hydroxide. The equivalence point in the titration is reached after the addition of 28.65 mL of 6.189×10-2 M barium hydroxide to the sample of the unknown acid. Calculate the molar mass of the acid.
You are trying to determine the percentage of acetic acid in vinegar by titrating a sample of the vinegar with a standardized NaOH solution. Why is bromcresol green not a good choice for an indicator for this titration? If you do use bromcresol green as an indicator, will your result for the percentage of acetic acid in vinegar be too high or too low? What would be a better choice for an indicator for this titration? Why is your choice better?
The titration of 100.mL of 0.100 M NH3 (in the flask) with 0.200 M HCL (in the burette) was carried out. Calculate the pH solutions at the following volumes of HCL added
5 A chemistry graduate student is given 450. mL of a 0.10M ammonia (NH3) solution. Ammonia is a weak base with K, = 1.8 × 10. What mass of NH4Cl should the student dissolve in the NH3 solution to turn it into a buffer with pH = 9.11? You may assume that the volume of the solution doesn't change when the NH4Cl is dissolved in it. Be sure your answer has a unit symbol, and round it to 2 significant digits. ☐ ☐ x10

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A titration was performed using a 25.00 mL sample of 0.15 M weak acid and 0.092 M strong base. What was the pH 5.00 mL after the equivalence point was reached? REPORT YOUR ANSWER TO 2 DECIMAL PLACES. DO NOT INCLUDE UNITS. × 12.40