ACID-BASE TITRATION PRELAB QUESTIONS NAME 1. A 4.00 mL sample of vinegar (active ingredient, acetic acid) was titrated with 0.1250M NAOH according to the following equation: HC2H3O2 + NaOH NAC2H3O2 HOH 25.19 mL of base was needed to reach the end point. Calculate the molarity of the acetic acid 2. Calculate the grams of acetic acid in one liter of the vinegar. 3. The 4.00 mL sample of vinegar had a mass of 4.056 g. Calculate the one liter. of vinegar in grams Calculate the % acetic acid in the vinegar. 4. % acetic acid g acetic acid g vinegar x 100 1 95

ACID-BASE TITRATION PRELAB QUESTIONS NAME 1. A 4.00 mL sample of vinegar (active ingredient, acetic acid) was titrated with 0.1250M NAOH according to the following equation: HC2H3O2 + NaOH NAC2H3O2 HOH 25.19 mL of base was needed to reach the end point. Calculate the molarity of the acetic acid 2. Calculate the grams of acetic acid in one liter of the vinegar. 3. The 4.00 mL sample of vinegar had a mass of 4.056 g. Calculate the one liter. of vinegar in grams Calculate the % acetic acid in the vinegar. 4. % acetic acid g acetic acid g vinegar x 100 1 95

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter16: Applications Of Neutralization Titrations

Section: Chapter Questions

Problem 16.28QAP

See similar textbooks

Similar questions

When 20.00 ml of sulfuric acid of unknown concentration is titrated with 0.1249 M NaOH, 32.50 ml of titrant are needed to reach the end point. What is the molarity of the sulfuric acid? (Give both the calculator answer and the significant figure answer).
What is the mass of aectylsaliyclic acid (HC9H7O4, MW = 180.154 g/mol) from an aspirin tablets by titrating with NaOH. One tablet is dissolved in 25 mL of 50% ethanol solution. The resulting solution needed 13.41 mL of 0.2069 standardized NaOH titrant in order to achieve the phenolphthalein endpoint. What is the mg of aectylsaliyclic acid in the asiprin tablet?
Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balance chemical equation is given below. If the student used 21.21 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)
Oxalic acid dihydrate (H2C2O4 2H2O) can be used to standardize NaOH solution through acid-base titration. To determine the molarity of an unknown NaOH solution, a student weighed out 0.56 g of solid oxalic acid dihydrate and dissolved the solid in 32.8 mL of DI water. The resulting solution was used in a titration with the unknown NaOH solution (3 drops of phenolphthalein was used as an indicator). The balanced chemical equation is given below. If the student used 25.71 mL of the unknown NaOH solution in the titration, what is the molarity of the NaOH solution? Keep the correct number of significant figures. H2C2O4 (aq) + 2NaOH (aq) --> Na2C2O4 (aq) + 2H2O (l)
Maleic acid (H2C4H2O4, represented by H2M) is the precursor of malic acid widely used in industry. food as an acidulant and in the pharmaceutical industry it is used in the treatment of wounds. This acid can be determined by neutralization titration. Answer the items below about this determination. Considering a 15.0 mL sample of maleic acid-based product used in industry, determine the maleic acid concentration, in mol/L, in the sample knowing that 21.7 mL of a solution of 0.1120 mol/L NaOH for complete neutralization of this acid. How many grams of maleic acid were in the sample analyzed and what is its percentage (%, m/v) in the sample? [Answer; m=0.1405 mol L-1; percentage = 0.9365%] NaOH(aq) + H2M(aq)  Na2M (aq) + H2O(l) Suggest an appropriate indicator for the titration of this acid by looking at the titration curve profile below (IMAGE)
Sulfamic acid ( +H 3NSO 3 - , 97.094 g/mol) is a primary standard that can be used to standardize NaOH. +H 3NSO 3 - + OH - → H 2NSO 3 - + H 2O What is the molarity of a sodium hydroxide solution if 34.26 mL reacts with 0.3337 g of sulfamic acid?
17.5 milliliters of a 0.496 M RbOH solution are required to titrate 52.1 milliliters of a H3PO4 solution. What is the molarity of the H3PO4 solution?3RbOH + H3PO4 --> Rb3PO4 + 3H2O Please put answer in box with 3 digits past decimal in regular non scientific notation.
A pharmacist is identifying the saponification value of corn oil in the lab. She weighs 1.8 g of corn oil and saponified with 25 mL of 0.4 N KOH which require 9 mL of 0.5N HCl to titrate the excess KOH. She performs blank determination, 20 mL of 0.5 N HCl was required to titrate the corn oil. What is the saponification value of the corn oil? Does the sample comply with the USP requirement? Use this formula to work your result Saponification Value = (Vblank - Vsample)N of HCl56.11/Sample weight (g)
You perform an acid-base titration to standardize an HCl solution by placing 50.00 mL of HCl in a flask with a few drops of indicator solution. You put 0.1524 M NaOH into the buret, and the initial reading is 0.55 mL. At the end point, the buret read-ing is 33.87 mL. What is the concentration of the HCl solution?
A solution of tartaric acid (H2C4H6O6) with a known concentration of 0.155 M H2C4H4O6 is titrated with a 0.425 M NaOH solution. How many mL of NaOH are required to reach the second equivalence point with a starting volume of 70.0 mL H2C4H4O6, according to the following balanced chemical equation : H2C4H4O6 + 2 NaOH --> Na2C4H4O6 + 2H2O
What is the percentage of total acid expressed as acetic acid (CH3COOH) in a sample of vinegar if 3.000 g of the vinegar requires 20.50 mL of 0.1150 N KOH solution for an endpoint with phenolphthalein indicator? (Note: Use the least significant digits in your answer.)
A 44.6 mL of 0.103 M HCI is added to an antacid sample. The solution is titrated to a bromophenol blue endpoint using 19.8 mL of 0.0998M NaOH. How many moles and how many grams of the base are in the antacid sample? Assume the active ingredient is MgCO3. Moles of NaOH? Moles of HCl? Moles of MgCO3? Mass of MgCO3?