For this pr H2 SO4(aq) + 2 N2OH(aq) → Na2 SO4(aq) + 2H20(1) A titration is performed on a sample containing sulfuric acid (H2SO4) to assess its concentration. 3.73 mL of this sample are used to perform the titration. If 13.5 mL of a 1.00 M NAOH solution are required to reach the endpoint of the titration (neutralize all of the sulfuric acid), what was the molarity of sulfuric acid in that sample?

For this pr H2 SO4(aq) + 2 N2OH(aq) → Na2 SO4(aq) + 2H20(1) A titration is performed on a sample containing sulfuric acid (H2SO4) to assess its concentration. 3.73 mL of this sample are used to perform the titration. If 13.5 mL of a 1.00 M NAOH solution are required to reach the endpoint of the titration (neutralize all of the sulfuric acid), what was the molarity of sulfuric acid in that sample?

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...

See similar textbooks

Similar questions

MnO4 (aq) + H2O2 (aq) → Mn2+ (aq) + O2 (g) (a) Sketch a flask containing an analyte solution before any potassium permanganate KMnO4 is added, list out all species present. (b) Once a stoichiometric amount of permanganate ion is added to the analyte solution (the equivalence point of the titration!), sketch the beaker with all the species remaining after the reaction goes to completion. (c) Sketch the flask one more time, past the equivalence point. How do you know when you have passed the equivalence point?
A chemistry student needs to standardize a fresh solution of sodium hydroxide. He carefully weighs out 360. mg of oxalic acid (H,C,O), 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 97.4 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits. M
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 303 mg of oxalic acid, a diprotic acid that can be purchased inexpensively in high purity, and dissolves it in 250mL 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 104.5 mL of sodium hydroxidesolution. Calculate the molarity of the student's sodium hydroxide solution. Round your answer to 3 significant digits.
Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+H2O(l)An aqueous solution of Ca(OH)2with a concentration of 0.209 M was used to titrate 25.00 mL of aqueous HCl. 15.93 mL of the Ca(OH)2was required to reach the endpoint of the titration. A. How many moles of base were required to react completely with the acid in this reaction? _____mol Ca(OH)2 B. How many moles of HCl were present in the original 25.00 mL of acid?______mol HCl
You are preparing standard acid and base solutions for the laboratory, using potassium hydrogen phthalate (KHC₈H₄O₄, abbreviated KHP) as the primary standard. KHP (molar mass = 204.22 g/mol) has one acidic hydrogen. You prepared solutions of both NaOH and HCl. It took 22.65 mL of the NaOH solution to titrate (react exactly with) 1.55 g KHP. It then took 32.35 mL of HCl solution to titrate 25.00 mL of the NaOH solution. What is the molarity of the HCl solution?
A chemist titrates a 25.00 mL sample of 0.1041 M benzoic acid (C6H5COOH) against a 0.1000 M solution of NaOH.The overall reaction is shown by the equation below: C6H5COOH(aq)+NaOH(aq)C6H5COONa(aq)+H2O(l) What volume of NaOH solution (in mL) is required to reach the equivalence point? Which of the following quantities will be needed to calculate the pH at the equivalence point of the reaction?Choose one or more: total solution volume Kb for C6H5COO–[C6H5COOH]equivalencemoles C6H5COOHmoles C6H5COO– Using your answers to Parts 1 through 3, calculate the pH at the equivalence point of the reaction. Ka for C6H5COOH is equal to 6.28 × 10–5 and Kb for C6H5COO– is equal to 1.59 × 10–10. Give your answer to two places after the decimal.
A student titrates 10.0 mL of the 2.000 M HC2H3O2(aq) with an NaOH(aq) solution of unknown concentration. The student monitors the pH during the titration. The following titration curve was created using the experimental data. Write the balanced net ionic equation for the reaction that occurs when HC2H3O2(aq) and NaOH(aq) are combined. 2.Calculate the molar concentration of the NaOH(aq) solution. 3.Explain how the student can estimate the value of Ka for HC2H3O2(aq) using the titration curve.
Malic acid (C4H6O5) is a dicarboxylic acid that naturally occurs in the production of bignay wine. Maria was tasked to find out the acid content in a 200.0 mL wine sample by titrating it with a standardized solution of KOH. He was able to establish the working concentration of the KOH solution by using 39.12 mL of it to titrate a primary standard of KHP that weighed 3.021 g. The grams and %w/w of Malic acid present in the 200.0 mL wine sample were then determined by titrating a 20.00 mL aliquot using 48.95 mL of the standardized KOH solution. C4H6O5 (aq) + 2KOH (aq) ↔ K2C4H4O5 (aq) + 2H2O (l) Assume the density of the wine sample is 1.000 g/mL MM of KHP = 204.22 g/mol MM of C4H6O5 = 134.0874 g/mol What is the molar concentration of the prepared KOH solution?…
By titration, it is found that 51.5 mL51.5 mL of 0.143 M NaOH(aq)0.143 M NaOH(aq) is needed to neutralize 25.0 mL of HCl(aq).HCl(aq). Calculate the concentration of the HClHCl solution. [HCl]=[HCl]= M
A chemistry student needs to standardize a fresh solution of sodium hydroxide. She carefully weighs out 51 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 19.2 mL of sodium hydroxide solution. Calculate the molarity of the student's sodium hydroxide solution.
The standardized NaOH was used to determine the unknown concentration of H3PO4. The standard NaOH concentrtion is 0.126M. The standard sulfuric acid concentration is 0.150M. 3 NaOH(aq) + H3PO4(aq) → Na3PO4(aq) + 3 H2O(l) Three flasks containing 25.00 mL H3PO4 each was titrated with NaOH. The data is below: Titration 1 Titration 2. Titration 3 Starting volume buret 2.62 mL 18.60 mL 1.20mL Buret volume at end 18.46 mL 34.40mL 16.84mL Calculate the concentration of H3PO4.
A solution of sodium hydroxide is standardized against potassium hydrogen phthalate (molecular mass = 204.224 g mol-1). From the following data, calculate the molarity of the NaOH solution. The mass of the KHP is 0.7840 g. Before the titration the buret reading was 0.8400 mL and afterwards it was 39.20 mL. A 85.12 mL sample of a solution of sulfuric acid, H2SO4, is neutralized by 59.82 mL of the NaOH solution from the problem above. Calculate the molarity of the sulfuric acid solution.