25.0 mL sample of vinegar was analyzed via titration in the same manner as you will use in this experiment. The standardized solution of NaOH was 0.950 M. A total of 10.5 mL of the sodium hydroxide were required to reach the pink endpoint. What was the concentration of the acetic acid in the vinegar solution?

25.0 mL sample of vinegar was analyzed via titration in the same manner as you will use in this experiment. The standardized solution of NaOH was 0.950 M. A total of 10.5 mL of the sodium hydroxide were required to reach the pink endpoint. What was the concentration of the acetic acid in the vinegar solution?

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter15: Solutions

Section: Chapter Questions

Problem 121AP: Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion...

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Calcium carbonate, CaCO3, can be obtained in a very pure state. Standard solutions of calcium ion are usually prepared by dissolving calcium carbonate in acid. What mass of CaCO3 should be taken to prepare 500. mL of 0.0200 M calcium ion solution?
In the experiment, the amount of acetic acid in vinegar was determined by titrating with 0.1 M NaOH solution. In the analysis, three trials were performed to obtain more precise result. The table shows the initial and final burette readings for three titrations: Initial Burette Reading (mL) Final Burette Reading (mL) Trial 1 2.9 10.6 Trial 2 10.6 18.1 Trial 3 18.1 25.7 According to the given data, calculate molarity of acetic acid in the commercial vinegar. Please be sure that your answer includes followings; a) moles of NaOH for each trial b) average mole of NaOH c) average mole of acetic acid in 50 mL solution d) average mole of acetic acid in 250 mL solution e) molarity of acetic acid in vinegar.
Acid-Base Titration: 10 mL of unknown acid sample was placed in a 250 mL Flask. 3 drops (0.15 mL) of Phenolphthalein was added to the unknown acid sample. The 10.0 M NaOH solution titrant was also dispensed into the unkown acid sample until it changed color. The final volume of the unknown acid sample is 11.680 mL. Please provide the computation for the final concentration of the unknown acid sample.
You want to determine the concentration of NaCl in a water. In preliminary analysis, it appears to be saline water with a NaCl content of approximately 4%. Should you dilute the sample if your titrant has a concentration of 0.1 M and you want to spend 25 mL of sample? Solution: You must dilute approximately ten times, taking 10 mL of sample and making up to 100 mL. In this way, 17.20 mL of titrant will be spent.
5. The concentration of an unknown sample of sulfuric acid was determined by the method used in this experiment, using two sets of titrations. In the first titration the sodium hydroxide was standardized by titrating 0.1355g of oxalic acid dihydrate (molar mass - 126.07g/mole) with 25.30mL of sodium hydroxide solution. In the second titration 20.00mL of the unknown sulfuric acid solution was titrated with 22.85mL of the sodium hydroxide solution. What was the concentration of the sulfuric acid? (Show your work!!)
You have a solution of a standardized titrant of 0.01254 M and a sample that approximately has a molarity of 0.48 M. What dilution do you have to do to spend approximately 15 mL of titrant if you have 25 mL and 10 mL pipettes to take the diluted sample and value it ? Solution: With the 10 mL pipette, the sample should only be previously diluted 1:25, with the 25 mL one 1:64. Therefore, 10 mL of the sample can be taken and made up to 250 mL.
5. Suppose there was a large air bubble in the tip of the acid burette during the titration and it was dislodged toward the end of your titration. Explain the effect that this would have on the calculated value of the acid's molarity. 6. A student titrated 30.00 mL of a hydrochloric acid solution with 1.00 M sodium hydroxide. The sodium hydroxide was initially filled to the 2.30 mL mark on the burette. Once the level in the burette reached 50.00 mL, the student wasforced to refill the burette and did so to the 5.06 mL mark. The endpoint was finally reached when the sodium hydroxide level dropped to 32.09 mL on the burette. What is the molarity of the acid solution? Show work. 7. How many milliliters of a 0.250 M sulfuric acid solution would be required to completely react with 2.398 grams of solid aluminum hydroxide? Work must be shown.
The solubility product of a sparingly soluble salt, XF2, was determined by titration and found to be 2.9 x 10-10 M3. The procedure involved the following steps: A saturated solution of the salt XF2 was prepared. 25.00 mL of this solution was titrated against a standardized 0.005 M HCl solution. Determine the titre value obtained in the experiment
A student did not read the directions to the experiment properly and mixed up where to put the NaOH and the HCl solutions. He put the HCl in the buret and the NaOH in the flask. He then added a drop of phenolphthalein to the solution in the flask. Does the student need to empty out all of the solutions and start over again or can he go ahead and run the titration? Explain
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A student is analyzing an unknown chloride mixture to discover the percentage of chloride in the sample. The following three sets of titration data were collected using a 0.05205 M silver nitrate solution. Find the percent chloride value for each sample, the average percent chloride value, and the parts per thousand value for the three samples. Sample #1: 0.1100 g sample required 18.25 mL of silver nitrate Sample #2: 0.1050 g sample required 17.30 mL of silver nitrate Sample #3: 0.1199 g sample required 20.42 mL of silver nitrate
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