I need help calculating the moles of acidand basebised and also the molarity ofthe base solutionolesRECORD ALL DATA IN INK using the correct number of significant figures and correct units. SHOWCOMPLETE "SET-UPS" (and the rounding off) for all calculations for Part 3 on the bottom of this page oron a separate sheet.3. Standardization of the NaOH Solution:Titration No.Acid buret, Final readingInitial readingVolume of acid usedMoles of acid usedBase buret, Final readingInitial readingVolume of base usedMoles of base usedMolarity of base solutionSet-ups:12324ml 36.24ml12- 12 m12mlAverage Molarity of the NaOH solutionAverage Deviation13 25.51313 12.5ml 12 mil.31.5456 RECORD ALL DATA IN INK using the correct number of significant figures and correct units. SHOWCOMPLETE "SET-UPS" (and the rounding off) for all calculations for Part 1 on the bottom of this page oron a separate sheet.1. Preparation of a Standard Acid Solution:Set-ups:mMMass of oxalic acid dihydrate and beakerMass of beakerMass of oxalic acid dihydrate usedMoles of oxalic acid dihydrate usedVolume of solution in volumetric flaskMolarity of oxalic acid solution1.575 -0.0125126(= ImplXO.OUT22-4 × 60125 = 0.2&L=250mly mula of shude4مان= 0.012525054464 x 15²1.85556109-6260108-07161-57590.0123m₂l2wh

Answered: Image /qna-images/answer/e4b0ba69-a73d-421d-bd7f-e74bcb0c1a44.jpg

RECORD ALL DATA IN INK using the correct number of significant figures and correct units. SHOW COMPLETE "SET-UPS" (and the rounding off) for all calculations for Part 3 on the bottom of this page or on a separate sheet. 3. Standardization of the NaOH Solution: Titration No.-> Acid buret, Final reading Initial reading Volume of acid used Moles of acid used Base buret, Final reading Initial reading Volume of base used Moles of base used Molarity of base solution Set-ups: oles = 1 12 ut 2 3 24ml 36 24ml 12- 12 ml 12m 13ML 25.5 31.5 OL 13 13 12.5ml 12 mil | Average Molarity of the NaOH solution Average Deviation 5

RECORD ALL DATA IN INK using the correct number of significant figures and correct units. SHOW COMPLETE "SET-UPS" (and the rounding off) for all calculations for Part 3 on the bottom of this page or on a separate sheet. 3. Standardization of the NaOH Solution: Titration No.-> Acid buret, Final reading Initial reading Volume of acid used Moles of acid used Base buret, Final reading Initial reading Volume of base used Moles of base used Molarity of base solution Set-ups: oles = 1 12 ut 2 3 24ml 36 24ml 12- 12 ml 12m 13ML 25.5 31.5 OL 13 13 12.5ml 12 mil | Average Molarity of the NaOH solution Average Deviation 5

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter14: Equilibria In Acid-base Solutions

Section: Chapter Questions

Problem 80QAP

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Similar questions

. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
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.
Sketch the titration curve for a weak acid titrated by a strong base. When performing calculations concerning weak acidstrong base titrations, the general two-slep procedure is to solve a stoichiometry problem first, then to solve an equilibrium problem to determine the pH. What reaction takes place in the stoichiometry part of the problem? What is assumed about this reaction? At the various points in your titration curve, list the major species present after the strong base (NaOH, for example) reacts to completion with the weak acid, HA. What equilibrium problem would you solve at the various points in your titration curve to calculate the pH? Why is pH 7.0 at the equivalence point of a weak acid-strong base titration? Does the pH at the halfway point to equivalence have to be less than 7.0? What does the pH at the halfway point equal? Compare and contrast the titration curves for a strong acidstrong base titration and a weak acidstrong base titration.
Explain why the hydrolysis of salts makes it necessary to have available in a laboratory more than one acid-base indicator for use in titrations.
A diprotic acid, H2B(MM=126g/moL), is determined to be a hydrate, H2B xH2O. A 10.00-g sample of this hydrate is dissolved in enough water to make 150.0 mL of solution. Twenty-five milliliters of this solution requires 48.5 mL of 0.425 M NaOH to reach the equivalence point. What is x?
You have a solution of the weak acid HA and add some of the salt NaA to it. What are the major species in the solution? What do you need to know to calculate the pH of the solution, and how would you use this information? How does the pH of the solution of just the HA compare with that of the final mixture? Explain.
The titration of Na2CO3 with HCl bas the following qualitative profile: a. Identify the major species in solution at points AF. b. Calculate the pH at the halfway points to equivalence, B and D. (Hint: Refer to Exercise 113.)