None UESTION 225.00 mL of a nitric acid solution of unknown concentration is pipetted into a 125-mL Erlenmeyer flask and 2 dropsof phenolphthalein are added. A 0.307 M sodium hydroxide solution (the titrant) is used to titrate the nitric acidsolution (the analyte). If 25.56 mL of the titrant is dispensed from a buret in causing a color change of thephenolphthalein, what is the molar concentration of the nitric acid solution?

Given: Volume of HNO3 = 25.00 mL ( 4 significant figures)Concentration (molarity)…

Answered: UESTION 2 25.00 mL of a nitric acid…

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.28QAP

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Similar questions

Describe how the amount of sodium hydroxide in a mixture can be determined by titration with hydrochloric acid of known molarity.
Explain how to choose the appropriate acid-base indicator for the titration of a weak base with a strong acid.
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?
A bottle of concentrated hydroiodic acid is 57% HI by weight and has a density of 1.70 g/mL. A solution of this strong and corrosive acid is made by adding exactly 10.0 mL to some water and diluting to 250.0 mL. If the information on the label is correct, what volume of 0.988 M NaOH is needed to neutralize the HI solution? Suggest an indicator for the titration.
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.
A monoprotic organic acid that has a molar mass of 176.1 g/mol is synthesized. Unfortunately, the acid produced is not completely pure. In addition, it is not soluble in water. A chemist weighs a 1.8451-g sample of the impure acid and adds it to 100.0 mL of 0.1050 M NaOH. The acid is soluble in the NaOH solution and reacts to consume most of the NaOH. The amount of excess NaOH is determined by titration: It takes 3.28 mL of 0.0970 M HCl to neutralize the excess NaOH. What is the purity of the original acid, in percent?
.00 mL of a nitric acid solution of unknown concentration is pipetted into a 125-mL Erlenmeyer ask and 2 drops of phenolphthalein are added. A 0.150M sodium hydroxide solution (the titrant) is bocd to titrate the nitric acid solution (the analyte), If 12.75 mL of the titrant is dispensed from a et in causing a color change of the phenolphthalein, what is the molar concentration of the nitric Sin acid solution
A 20.0 mL portion of a 0.300 M solution of hydrochloric acid is to be titrated with a standarized 0.350 M solution of KOH. What is the expected volume of the KOH solution needed to reach the phenolphthalein end point?
Part (c) and (d) only
What weight of sample should be taken for analysis sos that the volume of 0.1074N NaOH used for titration equals the percentage of potassium acid phthalate (KHC8H4O4) in the sample (Answer 2,193 g)
A vinegar sample of 28 mL was diluted with distilled water to a 250-mL volume. 25 mL portion ofthis solution was directly titrated with standard 0.01 mol/L NaH solution. The consumption was foundas 27.1 mL. Find the concentration (mol/L) of acetic acid in vinegar sample.
2. Using the procedure described in this module, a student determined the percent KHP in an impure sample of KHP. A 3.150-g sample of impure KHP required 41.50 mL of 0.1352M NaOH solution for titration. (a) Calculate the number of moles of NaOH required for the titration. (b) Calculate the number of moles of KHP present in the impure sample of KHP. (c) Calculate the number of grams of KHP present in the impure sample. (d) Calculate the percent of KHP in the impure sample, using Equation 8. Equation 8: percent KHP in the impure sample, % = ( mass of KHP in the sample,g/ mass of sample analyzed, g) (100%)

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