Titration of Acids and BasesPart B. Determination of the molar concentration of an unknown acid.Molarity of N₂OH = .09M☆Volume of unknown acid used (mL)Final buret reading (mL NaOH)Initial buret reading (mL NaOH)Volume of NaOH used (mL)Molarity of unknown acidTrial 110mbMoles9.6 mL0.5mL9.1mL(OH)Sample calculations for molarity of unknown acid solution:Trial 210mL18,9Average molarity of unknown acid solution:Trial 310mL28.3mL9.6 ml 18.9ml9,3mL 9.4mLmol NaOHused?M N₂OH =M acid = .1GrilTo multipledecimals

To find out the molarity of the unknown acid solution, we need to use the dilution law. Using that,…

Titration of Acids and Bases Part B. Determination of the molar concentration of an unknown acid. Mollarity of NaOH = .09M Volume of unknown acid used (mL) Final buret reading (mL NaOH) Initial buret reading (mL NaOH) Volume of NaOH used (mL) Molarity of unknown acid Trial 1 10mb 9.6 mL 0.5mL 9.1mL Trial 2 Sample calculations for molarity of unknown acid solution: 10ml 18,9 9.6 ml 9,3mL Average molarity of unknown acid solution: Trial 3 Detal 10mL 28.3mL 18.9ml 9.4mL 002 mol us MA Maci G To mun decin

Titration of Acids and Bases Part B. Determination of the molar concentration of an unknown acid. Mollarity of NaOH = .09M Volume of unknown acid used (mL) Final buret reading (mL NaOH) Initial buret reading (mL NaOH) Volume of NaOH used (mL) Molarity of unknown acid Trial 1 10mb 9.6 mL 0.5mL 9.1mL Trial 2 Sample calculations for molarity of unknown acid solution: 10ml 18,9 9.6 ml 9,3mL Average molarity of unknown acid solution: Trial 3 Detal 10mL 28.3mL 18.9ml 9.4mL 002 mol us MA Maci G To mun decin

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter9: Acids, Bases, And Salts

Section: Chapter Questions

Problem 9.103E

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Similar questions

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.
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.
Consider the following two acids: In two separate experiments the pH was measured during the titration of 5.00 mmol of each acid with 0.200 M NaOH. Each experiment showed only one stoichiometric point when the data were plotted. In one experiment the stoichiometric point was at 25.00 mL added NaOH, and in the other experiment the stoichiometric point was at 50.00 mL NaOH. Explain these results. (See Exercise 113.)
Using Figure 17.11, suggest an indicator to use in each of the following titrations: (a) The weak base pyridine is titrated with HCl. (b) Formic acid is titrated with NaOH. (c) Ethylenediamine, a weak diprotic base, is titrated with HCl. Figure 17.11 Common acid-base indicators. The color changes occur over a range of pH values. Notice that o few indicators hove color changes over two different pH ranges.
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.
Consider the titration of 100.0 mL of 0.200 M acetic acid (Ka = 1.8 105) by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL b. 50.0 mL c. 100.0 mL d. 150.0 mL e. 200.0 mL f. 250.0 mL
A 0.2481 M solution of KOH is used to titrate 30.00 mL of 0.269 M hydrobromic acid. Assume that volumes are additive. (a) Write a balanced net ionic equation for the reaction that takes place during the titration. (b) What are the species present at the equivalence point? (c) What volume of KOH is required to reach the equivalence point? (d) What is the pH of the solution 1. before any KOH is added? 2. halfway to the equivalence point? 3. at the equivalence point?