Data TableFinal buret readingInitial buret readingVolume usedSample 1Vinegar Base VinegarSample 2Sample 3(if needed)BaseVinegarBaseJOMLSom0,05110mL/802 10ML 884JUML 0.00 10μL OMLTome 0.0010mL 80.2 mL 10ML 88mL come some*If a pipet is used to measure the volume of vinegar, record only in the space for volume used.Molarity of base (NaOH) 1685 M Vinegar numberN/ACALCULATIONS: In the spaces below, show calculation setups for Sample 1 only. Showanswers for both samples in the boxes.1. Moles of base (NaOH)2. Moles of acid (HC2H3O2) used to neutralize(react with) the above number of moles ofbase3. Molarity of acetic acid in the vinegarSample 1Sample 2Sample 3(if needed)4. Average molarity of acetic acid in the vinegar5. Grams of acetic acid per liter (from average molarity)6. Mass percent acetic acid in vinegar sample(density of vinegar = 1.005 g/mL)- 252 -

5. Grams of Acetic Acid per LiterTo calculate grams per liter, use the molarity and molar mass of…

Answered: Data Table Final buret reading Initial…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter11: Solutions

Section: Chapter Questions

Problem 10P

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An experiment calls for 100. mL of 1.25 M HC1. All that is available in the lab is a bottle of concentrated HC1, whose label indicates that it is 12.1 M. How much of the concentrated HC1 would be needed to prepare the desired solution?
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?
Addition of water to concentrated sulfuric acid is dangerous because it generates enough heat to boil the water, causing it to spatter out of the container. For this reason, chemists remember to add acid to water. In a dilution experiment, we calculate the amount of the more concentrated solution that must be measured out. If we place this concentrated solution (Figure 4.7) in the volumetric flask first, then dilute with water, we violate the caution Add acid to water. Describe a safer variation on the method shown in Figure 4.7 that allows the quantitative dilution of concentrated sulfuric acid. Figure 4.7 Preparing a dilute solution from a concentrated solution. (a) Draw the concentrated solution into a pipet to a level just above the calibration mark. (b) Allow the liquid to settle down to the calibration line. Touch the tip of the pipet to the side of the container to remove any extra liquid. (c) Transfer this solution to a volumetric flask. Again touch the pipet to the wall of the flask to ensure complete transfer, but do not blow out the pipet because it is calibrated for a small amount of liquid to remain in the tip. (d) Dilute to the mark with solvent. Frequently, especially with concentrated acids, it is best to have some solvent present in the volumetric flask before you add the concentrated sample.
What volume of 0.220 M HBr solution (in mL) is required to obtain 0.060 moles of HBr? A) 3.67 L B) 273 mL C) 2.73 x 10^-4 mL D) 13.2 mL
Pls help ASAP ON ALL ASKED QUESTIONS PLS PLS
3. 8.0 mL of HCI was added into a 10.0 mL graduated cylinder and weighed on a centigram balance. Looking at the photo to the right, record the mass to the nearest 0.01 Sost ha 12.71 gram in your data table (line 4)
Do the dilutions for the given concentration.
Given chart attached Calculate the number of moles of base (NaOH) required to reach the endpoint
You have 505mL of a 0.145M HCl solution and you want to dilute it to exactly 0.100M How much water should you add? Round your answer to 3 significant digits.
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The molarity and normality of a diprotic acid is the same. True False
50 mL of stock solution were taken and added to flask. Then 50 mL of Di water were added to the flask. This is solution 1. Then 50mL of solution 1 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 2. Then 50mL of solution 2 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 3. Then 50mL of solution 3 were taken and added to a flask and 50 mL of Di water were added to the flask. This is solution 4. Find the concetrations of each solution. Information of stock solution - molar mass- 534.3g/mole 0.587g in MilliQ

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