Titration of Acetic Acid CH3COOH 1) Record the exact Molarity of the freshly prepared solution of NaOH by reading the label on the bottle, include all digits provided. This is the solution that will be in the buret. MB = 0.0500 M 2) Record the exact volume of acid CH3COOH that was pipetted into the Erlenmeyer mL. Note the concentration is unknown and what you will solve for. flask 10.00 (This was diluted with 50 mL of water in the Erlenmeyer flask) Trial 1 Trial 2 Trial 3 Final base (mL) 30.46 30.98 29.88 Initial base (mL)__ 0.45 0.05 0.04 Total base (mL) *Molarity (M) CH COOH *Use stoichiometry to determine the molarity of your CH,COOH solution from each of trial. Show all work including units for one. Calculate Average Molarity

Titration of Acetic Acid CH3COOH 1) Record the exact Molarity of the freshly prepared solution of NaOH by reading the label on the bottle, include all digits provided. This is the solution that will be in the buret. MB = 0.0500 M 2) Record the exact volume of acid CH3COOH that was pipetted into the Erlenmeyer mL. Note the concentration is unknown and what you will solve for. flask 10.00 (This was diluted with 50 mL of water in the Erlenmeyer flask) Trial 1 Trial 2 Trial 3 Final base (mL) 30.46 30.98 29.88 Initial base (mL)__ 0.45 0.05 0.04 Total base (mL) Molarity (M) CH COOH Use stoichiometry to determine the molarity of your CH,COOH solution from each of trial. Show all work including units for one. Calculate Average Molarity

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

Chapter4: Types Of Chemical Reactions And Solution Stoichiometry

Section: Chapter Questions

Problem 47E

See similar textbooks

Similar questions

ssume a highly magnified view of a solution of HCI that allows you to “see” the HCl. Draw this magnified view. If you dropped in a piece of magnesium, the magnesium would disappear, and hydrogen gas would he released. Represent this change using symbols for the elements, and write the balanced equation.
A sample of solid calcium hydroxide, Ca(OH)2, is allowed to stand in water until a saturated solution is formed. A titration of 75.00 mL of this solution with 5.00102M HCl requires 36.6 mL of the acid to reach the end point. Ca(OH)2(aq)+2HCl(aq)CaCl2(aq)+2H2O(l) What is the molarity?
Describe in words the titration of an acid with a base. Be sure to use the terms equivalence point, indicator, and end point correctly.
Hydrochloric acid. HCl, with a concentration of 0.100 M can be purchased from chemical supply houses, and this solution can be used to standardize the solution of a base. If titrating 25.00 mL of a sodium hydroxide solution to the equivalence point requires 29.67 mL of 0.100 M HCI, what is the concentration of the base?
Lead poisoning has been a hazard for centuries. Some scholars believe that the decline of the Roman Empire can be traced, in part, to high levels of lead in water from containers and pipes, and from wine that was stored in leadglazed containers. If we presume that the typical Roman water supply was saturated with lead carbonate, PbCO3 (Ksp = 7.4 1014), how much lead will a Roman ingest in a year if he or she drinks 1 L/day from the container?
A mountain lake that is 4.0 km × 6.0 km with an average depth of 75 m has an H+(aq) concentration of 1.3 × 10−6 M. Calculate the mass of calcium carbonate that would have to be added to the lake to change the H+(aq) concentration to 6.3 × 10−8 M. Assume that all the carbonate is converted to carbon dioxide, which bubbles out of the solution.
The equation for a reaction by which a solution of sodium carbonate may be standardized is 2HC7H5O2+Na2CO32NaC7H5O2+H2O+CO2. A student determines that 5.038g of HC7H5O2 uses 51.89mL of sodium carbonate solution in the titration. Find the molarity of the sodium carbonate.
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.
Write a net ionic equation for any precipitation reaction that occurs when 1 M solutions of the following are mixed. (a) copper(II) sulfate and sodium chloride (b) manganese(II) nitrate and ammonium hydroxide (c) silver nitrate and hydrochloric acid (d) nickel(II) sulfate and potassium hydroxide (e) ammonium carbonate and sodium nitrate
One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total solution volume after mixing is 750. mL, what is the concentration of hydrochloric acid in the resulting solution? What is its pH?
Two liters of a 1.5 M solution of sodium hydroxide are needed for a laboratory experiment. A stock solution of 5.0 M NaOH is available. How is the desired solution prepared?
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.