A 5.00 ml sample of vinegar was titrated with 0.08751 M NAOH. The sample requires 22.31 mL of NaOH to reach the endpoint. Calculate the molarity of the acetic acid (CH,COOH) solution in the vinegar sample. The density of the vinegar solution has been determined to be 1.0052 g/ml.

A 5.00 ml sample of vinegar was titrated with 0.08751 M NAOH. The sample requires 22.31 mL of NaOH to reach the endpoint. Calculate the molarity of the acetic acid (CH,COOH) solution in the vinegar sample. The density of the vinegar solution has been determined to be 1.0052 g/ml.

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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Question

please help me out

Use the titration data to calculate the molarity of acetic acid in the vinegar.
Try a sample calculation Refer to Section 4 for sample calculations:
A 5.00 ml sanmple of vinegar was titrated with 0.08751 MNaOH. The sample requires 22.31 mL of
NAOH to reach the endpoint. Calculate the molarity of the acetic acid (CH;COOH) solution in the
vinegar sample. The density of the vinegar solution has been determined to be 1.0052 g/ml.
If the vinegar is being manufactured, and is supposed to have a molar concentration between 0.45 and
0.60, can this batch be sold?

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An acid is titrated with NaOH. The following beakers are illustrations of the contents of the beaker at various times during the titration. These are presented out of order. Note: Counter-ions and water molecules have been omitted from the illustrations for clarity. (a) (b) (c) (d) (e) a. Is the acid a weak or strong acid? How can you tell? b. Arrange the beakers in order of what the contents would look like as the titration progresses. c. For which beaker would pH = pKa? Explain your answer. d. Which beaker represents the equivalence point of the titration? Explain your answer. e. For which beaker would the Ka value for the acid not be necessary to determine the pH? Explain your answer.
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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?
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 2.500-g sample of a mixture of sodium carbonate and sodium chloride is dissolved in 25.00 mL of 0.798 M HCl. Some acid remains after the treatment of the sample. a Write the net ionic equation for the complete reaction of sodium carbonate with hydrochloric acid b If 28.7 mL of 0.108 M NaOH were required to titrate the excess hydrochloric acid, how many moles of sodium carbonate were present in the original sample? c What is the percent composition of the original sample?
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