A student performs a titration and records the following data: Initial buret volume: 13.76 mL Final buret volume: 28.65 mL Molarity of NaOH solution: 0.233 M Calculate the moles of NaOH used in this titration

A student performs a titration and records the following data: Initial buret volume: 13.76 mL Final buret volume: 28.65 mL Molarity of NaOH solution: 0.233 M Calculate the moles of NaOH used in this titration

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter13: Titrations In Analytical Chemistry

Section: Chapter Questions

Problem 13.2QAP

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The equation for a reaction by which a solution of sodium carbonate may be standardized is 2HC7H5O2+Na2CO32NaC7H5O2+H2O+CO2. A student determines that 5.038g of HC7H5O2 uses 51.89mL of sodium carbonate solution in the titration. Find the molarity of the sodium carbonate.
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
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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.
Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
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If 55 mg of lead(II) sulfate is placed in 250 mL of pure water, does all of it dissolve? If not, how much dissolves?
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?
Calculate the sodium ion concentration when 70.0 mL of 3.0 M sodium carbonate is added to 30.0 mL of 1.0 M sodium bicarbonate.
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