O Chemical ReactionsStandardizing a base solution by titration3/5BisA chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 36. mg of oxalic acid (H2C2O4), a diprotic acid that canbe purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodiumhydroxide solution. When the titration reaches the equivalence point, the student finds he has used 35.1 mL of sodium hydroxide solution.Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits.ОмOPG

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Answered: O Chemical Reactions Standardizing a…

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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An analytical chemist weighs out 0.193 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1200 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 24.0 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. g mol x10 X Ś
CHEMICAL REACTIONS Determining the volume of base needed to titrate a given mass... A chemistry student weighs out 0.0878 g of phosphoric acid (H₂PO4), a triprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1500 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits. Explanation Check X MacBook Air 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center
Vinegar is a solution of the monoprotic acid HC2H3O2 in water. A 15.0 mL solution of vinegar was titrated with a 0.5250 M NaOH solution. The sample required 23.77 mL of the NaOH solution. What is the concentration of acetic acid in g/L in the vinegar?
5. Calculate the concentration of the hydrochloric acid if a 20.00 mL sample is titrated with standard sodium carbonate solution. 2 HCI (aq) + Na₂CO3(aq) → H₂O (1) + CO₂(g) + 2 NaCl (aq) The titration required 10.00 mL of 0.250 mol/L sodium carbonate to neutralize the acid. rn Lakes College
Zinc and magnesium metal each react with HCl according to the following equation: Zn + 2 HCl= ZnCl2 + H2 Mg + 2 HCl = MgCl2 + H2 A 10.00 g mixture of zinc and magnesium is reacted with just enough of HCl so that all the zinc and magnesium in the mixture have reacted and no excess HCl is added. The resulting solution requires 156 mL of 3.00 M silver nitrate to precipitate all the Cl- ions in the solution to form silver chloride. Calculate the percent by mass of magnesium in the original mixture. (2)
To a 25.00 mL volumetric flask, a lab technician adds a 0.100 g sample of a weak monoprotic acid, HA, and dilutes to the mark with distilled water. The technician then titrates this weak acid solution with 0.0841 M KOH. She reaches the endpoint after adding 44.65 mL of the KOH solution. Determine the number of moles of the weak acid in the solution. moles of weak acid: Determine the molar mass of the weak acid. molar mass= pKa mol After the technician adds 16.63 mL of the KOH solution, the pH of the mixture is 5.79. Determine the pK₁ of the weak acid. = g/mol
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 30. mg of oxalic acid (H,C,0,), a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250. mL of distilled water. The student then titrates the oxalic acid solution with his sodium hydroxide solution. When the titration reaches the equivalence point, the student finds he has used 62.3 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits. x10
it is time for the titration. You measure 15.0 mL of the H2C2O4 solution with a 100-mL graduated cylinder and add it to a 125-mL Erlenmeyer flask. Then you add two drops of the indicator, phenolphthalein, to the oxalic acid solution in the flask. You dispense the NaOH solution from the buret into the flask (while swirling the flask) until you reach the endpoint. At the endpoint, the solution in the flask turns light pink. You repeat the titration two additional times for a total of three trials. H2C2O4 (aq) + 2 NaOH (aq) --> Na2C2O4 (aq) + 2 H2O (l) (I) (II) (III) Volume of H2C2O4 used 15.00 mL 15.00 mL 15.00 mL Initial Buret Reading 0.00 mL 0.05 mL 0.10 mL Final Buret Reading 14.45 mL 14.38 mL 15.40 mL Volume NaOH used ________mL ________mL ______mL Moles NaOH _______M ________M _________M…
An analytical chemist weighs out 0.181 g of an unknown diprotic acid into a 250 mL volumetric flask and dilutes to the mark with distilled water. She then titrates this solution with 0.1700 M NaOH solution. When the titration reaches the equivalence point, the chemist finds she has added 15.9 mL of NaOH solution. Calculate the molar mass of the unknown acid. Be sure your answer has the correct number of significant digits. ol. g mol Ar
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 13.mg of oxalic acid H2C2O4, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250.mL of distilled water. The student then titrates the oxalic acid solution with her sodium hydroxide solution. When the titration reaches the equivalence point, the student finds she has used 11.9mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 2 significant digits.
= 1 = 2 = 3 4 7 = 8 10 = 11 12 A chemistry student weighs out 0.106 g of sulfurous acid (H,So,), a diprotic acid, into a 250. mL volumetric flask and dilutes to the mark with distilled water. He plans to titrate the acid with 0.1100 M NaOH solution. Calculate the volume of NaOH solution the student will need to add to reach the final equivalence point. Round your answer to 3 significant digits. I ml Continue Submit A © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center e to search 2 74°F Mostly clear
Tartaric acid, H2C4H4O6, is a diprotic acid that naturally occurs in the production of apple wine. Emma was tasked to find out the acid content in a 50.0 mL wine sample by titrating it with a standardized solution of NaOH. She was able to establish the working concentration of the NaOH solution by using 17.61 mL of NaOH to titrate a primary standard of KHP that weighed 1.501 g. The grams and %w/w of Tartaric acid present in the 50.0 mL wine sample were then determined by titrating a 12.50 mL aliquot using 21.78 mL of the standardized NaOH solution. H2C4H4O6 (aq) + 2NaOH (aq) ↔ Na2C4H4O6 (aq) + 2H2O (l) Assume that the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of H2C4H4O6 = 150.087 g/mol What is the molar concentration of the prepared NaOH solution?…

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