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 9.145E

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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)
Determine the volume (mL) of 0.154 M NaOH required to titrate to the equivalence point 21.0 mL of a 0.242 M solution of a monoprotic weak acid that is 33.0% ionized. Enter your answer to 1 decimal place.
Circie the volumes of the titrated NaOH(aq) which you want to use for your calculations. How and why did you choose these volumes of NaOH(aq)?
D. Acid-Base Titrations A 0.1558 g of primary-standard-grade benzoic acid, C6H$COOH, was used to standardize a solution of Mg(OH)2. Calculate the normality of this solution if it needed 19.15 mL of this base to reach the end point of the titration. A solution of an unknown monoprotic acid was found in a laboratory. When titrated, 25.00 mL of this unknown solution needed 28.44 mL of the same base to reach the endpoint. The remaining solution of unknown monoprotic acid amounting 15.00 mL was left in an Erlenmeyer flask uncovered to recover the acid crystals. After 5 days, the mass of the unknown monoprotic acid left on the flask weighed 0.0967 g. Determine the equivalent weight of this unknown acid. FW: C6HSCOOH: 122.12 Mg(OH)2 = 58.32
A student performs a titration, titrating 25.00 mL of a weak monoprotic acid, HA, with a 1.59 M solution of NaOH. They collect data, plot a titration curve and determine that the equivalence point occurred after the addition of 21.93 mL of sodium hydroxide. What was the total volume ( in mL) of the solution at the equivalence point?(give your answer to two decimal places)

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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