The “impure” phthalic acid was mixed with a known (to the instructor but not the student)...

The “impure” phthalic acid was mixed with a known (to the instructor but not the student) amount of resorcinol. Can you determine the amount of resorcinol (percentage) contained in the impure phthalic acid sample? Explain why or why not. Why factors play an important role in making this determination.

Expert Solution

queen_honey_blossom answered 8 months ago

A student purified a 500-mg sample of phthalic acid by recrystallization from water. The published solubility...

A student purified a 500-mg sample of phthalic acid by recrystallization from water. The published solubility of phthalic acid in 100mL of water is 0.54 g at 14C and 18 g at 99C. The smallest volume of boiling water the student could use to dissolve 500 mg of phthalic acid is 2.778 mL of water.Dissolution of phthalic acid in boiling water produced a dark-colored solution. The student allowed the solution to cool, added several spatulas full of activated carbon, and...

After recrystallizing an impure sample of benzoic acid, a student scratched it off the filter paper...

After recrystallizing an impure sample of benzoic acid, a student scratched it off the filter paper and took a melting point. Most of the compound melted between 121 and 122 degrees Celsius. A small amount remained un-melted even at temperatures above 200 degrees celsius. Explain this behavior.

Phthalic acid, H2C8H4O4, is a diprotic acid, with the following Ka values: Ka1 = 0.0012 and...

Phthalic acid, H2C8H4O4, is a diprotic acid, with the following Ka values: Ka1 = 0.0012 and Ka2 = 3.9 X 10-6. What is the pH of a solution that contains 2.50 grams of phthalic acid dissolved in enough water to make 500.00 mL of water.

A powder contains benzoic acid mixed with starch. A student finds that a 2.69 g sample...

A powder contains benzoic acid mixed with starch. A student finds that a 2.69 g sample of this powder requires 44.31 mL of a 0.101M sodium hydroxide solution for the acid to be neutralized. What is the percent by mass of benzoic acid in the powder?

Given a small amount of an impure solid (with an insoluble impurity) and a known solvent...

Given a small amount of an impure solid (with an insoluble impurity) and a known solvent to recrystallize the solid, briefly in 3 steps describe how you would go about in recrystallizing and purifying the impure solid.

How can phthalic acid not be soluble in water in both hot or cold temperatures?

"In a decomposition process, 2.40 g of impure CaCO3 (CaCO3 mixed with other substances that remain...

"In a decomposition process, 2.40 g of impure CaCO3 (CaCO3 mixed with other substances that remain as residue) was decomposed at high temperature and a total pressure of 960.0 torr. 2.00 L CO2 gas was collected over water at 25.0 C. The Water Vapor Pressure is 26.0 torr at 25.0 C. Find Percent by mass of the pure CaCO3" Thank you!

The solubility of phthalic acid in water is 0.54 g/100 mL at 14 C and 18...

The solubility of phthalic acid in water is 0.54 g/100 mL at 14 C and 18 g/100 mL at 99 C.What is the smallest volume of boiling water that should be used to recrystallize 600 mg of phthalic acid from hot water? You will have to recrystallize many compounds throughout organic I and II. Write a short procedure on how you would do a simple recrystallization( no hot gravity filtration involved). Assume you know which solvent to use but not...

1) One of the major problems is the large amount of phthalic acid (see your text...

1) One of the major problems is the large amount of phthalic acid (see your text for Kas) managed to make its way into the pond. The Company wants to know the pH of the pond. Cornelius makes some quick measurements and finds the pond is perfectly circular and has a radius of 1.000 meter and a depth of 1.000 meter. (Remember that 1 mL = 1 cm3). The tank that held the phthalic acid was a 3.00 L tank....

You are given 2.00 g of a mixture of phenol, aniline, phthalic acid and methyl benzoate....

You are given 2.00 g of a mixture of phenol, aniline, phthalic acid and methyl benzoate. Describe, how you would use an acid-base extraction technique to separate all three compounds by drawing the flowchart. Propose another way of extraction, where different order of extraction is used (e.g., adding the acid first instead of a base)

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