5. Determining the percent sulfuric acid in an unknown solution. Experimental Procedure and Results: You determine that there are exactly 20 drops in one mL and you are using 1.65 M sodium hydroxide in the experiment. Assume the solution densities are the same as water at room temperature. You select an aqueous solution of dilute sulfuric acid and pour between 10 and 20 mL of it into a 50 mL beaker, then add 2 drops of phenolphthalein indicator. You then add sodium hydroxide dropwise until the solution just turns pink. The following is your experimental data. Mass of the empty 50 mL beaker: 52.25 g Mass of beaker plus unknown solution: 66.55 g Drops of NaOH to get the pink color: 65 Answer the following question and show your calculations a) What is the percent by mass of sulfuric acid in the unknown solution?

5. Determining the percent sulfuric acid in an unknown solution. Experimental Procedure and Results: You determine that there are exactly 20 drops in one mL and you are using 1.65 M sodium hydroxide in the experiment. Assume the solution densities are the same as water at room temperature. You select an aqueous solution of dilute sulfuric acid and pour between 10 and 20 mL of it into a 50 mL beaker, then add 2 drops of phenolphthalein indicator. You then add sodium hydroxide dropwise until the solution just turns pink. The following is your experimental data. Mass of the empty 50 mL beaker: 52.25 g Mass of beaker plus unknown solution: 66.55 g Drops of NaOH to get the pink color: 65 Answer the following question and show your calculations a) What is the percent by mass of sulfuric acid in the unknown solution?

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter4: Chemical Reactions In Solution

Section: Chapter Questions

Problem 4.9QE: Addition of water to concentrated sulfuric acid is dangerous because it generates enough heat to...

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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.
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