Titration of Acids and Basesfa Vola!!Part B. Determination of the molar concentration of an unknown acid.Volume of unknown acid used (mL)Final buret reading (mL NaOH)Initial buret reading (mL NaOH)Volume of NaOH used (mL)an unknownandMolarity of unknown acidTrial 110mL9.6 mL0.5mL9,1mLTrial 2Sample calculations for molarity of unknown acid solution:10mL18,9Trial 3Average molarity of unknown acid solution:10mL28.3mL9.6 ml 18,9ml9,3m² 9.4mLmol NaOHused?M N₂OH =M acid= .1Griln.1To multipledecimals

The question is based on the concepts of titrations. we need to calculate concentration of unknown…

Titration of Acids and Bases Mate of a Volatile Part B. Determination of the molar concentration of an unknown acid. Volume of unknown acid used (mL) the Final buret reading (mL NaOH) Initial buret reading (mL NaOH) Volume of NaOH used (mL) Molarity of unknown acid Trial 1 10mL on 9.6 mL 0.5ml 9.1mL Trial 2 Sample calculations for molarity of unknown acid solution: 10ml Average molarity of unknown acid solution: Trial 3 10mL 28.3mL 18.9 9.6 ml 18,9ml 9,3mL 9.4mL mol NaOH used? M NaOH = Macid= .1 Guil To multiple decimals

Titration of Acids and Bases Mate of a Volatile Part B. Determination of the molar concentration of an unknown acid. Volume of unknown acid used (mL) the Final buret reading (mL NaOH) Initial buret reading (mL NaOH) Volume of NaOH used (mL) Molarity of unknown acid Trial 1 10mL on 9.6 mL 0.5ml 9.1mL Trial 2 Sample calculations for molarity of unknown acid solution: 10ml Average molarity of unknown acid solution: Trial 3 10mL 28.3mL 18.9 9.6 ml 18,9ml 9,3mL 9.4mL mol NaOH used? M NaOH = Macid= .1 Guil To multiple decimals

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 70QAP: Three students titrate different samples of the same solution of HCI to obtain its molarity. Below...

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Another way to treat data from a pH titration is to graph the absolute value of the change in pH per change in milliliters added versus milliliters added (pH/mL versus mL added). Make this graph using your results from Exercise 61. What advantage might this method have over the traditional method for treating titration data?
Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
Follow the directions of Question 64. Consider two beakers: Beaker A has a weak acid(K a=1105). Beaker B has HCI. The volume and molarity of each acid in the beakers are the same. Both acids are to be titrated with a 0.1 M solution of NaOH. (a) Before titration starts (at zero time), the pH of the solution in Beaker A is the pH of the solution in Beaker B. (b) At half-neutralization (halfway to the equivalence point), the pH of the solution in Beaker A the pH of the solution in Beaker B. (c) When each solution has reached its equivalence point, the pH of the solution in Beaker A the pH of the solution in Beaker B. (d) At the equivalence point, the volume of NaOH used to titrate HCI in Beaker B the volume of NaOH used to titrate the weak acid in Beaker A.
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.
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.
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.
A student intends to titrate a solution of a weak monoprotic acid with a sodium hydroxide solution but reverses the two solutions and places the weak acid solution in the buret. After 23.75 mL of the weak acid solution has been added to 50.0 mL of the 0.100 M NaOH solution, the pH of the resulting solution is 10.50. Calculate the original concentration of the solution of weak acid.
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.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.