An impure sample contains 1.09 g of impurities and 5.07 g of benzoic acid. The impure sample is dissolved in water, then heated. The solution is then cooled. How many grams of benzoic acid will recrystallize when the solution has cooled? The solubilities of the impurity and benzoic acid in hot water are given below: Compound Cold Water solubility Hot Water Solubility Benzoic acid 0.42 g per 100 mL of water 5.79 g per 100 mL of water Impurity 0.61 g per 100 mL of water 4.62 g per 100 mL of water

An impure sample contains 1.09 g of impurities and 5.07 g of benzoic acid. The impure sample is dissolved in water, then heated. The solution is then cooled. How many grams of benzoic acid will recrystallize when the solution has cooled? The solubilities of the impurity and benzoic acid in hot water are given below: Compound Cold Water solubility Hot Water Solubility Benzoic acid 0.42 g per 100 mL of water 5.79 g per 100 mL of water Impurity 0.61 g per 100 mL of water 4.62 g per 100 mL of water

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter7: Solutions And Colloids

Section: Chapter Questions

Problem 7.1E

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Magnesium sulfate (MgSO4) has a solubility of 38.9 g/ 100 g H2O at 30C. A solution is prepared by adding 9.50 g of MgSO4 to 25.0 g of water at 40C. A homogeneous mixture is obtained. Is the solution saturated, unsaturated, or supersaturated? One gram of magnesium sulfate is added to the solution cooled to 30C. Would you expect some of the MgSO4 to precipitate? If so, how much? If not, how much more MgSO4 can be added before precipitation takes place?
A 25mL volumetric pipet is used to deliver a sample of the stock solution marked “0.6000M X2SO4” into a 100mL volumetric flask. Distilled water is added to the flask until it is about 3/4thfull, the solution is mixed well, then more water is added to fill it up to the calibration mark, then it is mixed again. Calculate the concentration of X+ion in the dilute solution made above.
Using the Solubility Data for Report below answer the question: Compound Cold water Solubility Hot Water Solubility Benzoic Acid 0.42 g per 100mL of water 5.79 g per 100mL of water Impurity 0.61 g per 100mL of water 4.62 g per 100mL of water An impure sample contains 1.14 g of impurities and 5.14 g of benzoic acid. The sample is dissloved in 100mL of water and heated. The solution is then cooled. How many grams of impurity will crystalize when the solution has cooled?
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An impure sample contains 0.74 g of impurities and 4.55 g of benzoic acid. The sample is dissolved in 100 mL of water and heated. The solution is then cooled. How many grams of the impurity will crystallize when the solution has cooled? Include the unit and two decimal places in your answer. The solubilities of the impurity and benzoic acid in cold and hot water are found as an "item" in the "Recrystallization" folder. Solubility Data for Report Questions 11 Compound Cold Water solubility Hot Water Solubility Benzoic acid 0.42 g per 100 mL of water 5.79 g per 100 mL of water Impurity 0.61 g per 100 mL of water 4.62 g per 100 mL of water
A 10 ml of concentrated acetic acid was added in a sufficient quantity of water to make 350 ml of the acid solution. SG acetic acid= 1.05 kb acetate = 5.556x10^-10 What is the weight of acetic acid in grams? What is the molarity (mole/Liter) of acetic acid solution? What is the ka of acetic acid? What is the Hydronium ion concentration? What is the pH of the solution?
Part 1: Preparation of the Primary Citric Acid Standard Mass of empty 250-mL glass beaker: 100.7g Mass of 250-mL beaker and anhydrous citric acid First weighing : 103.4 g Second weighing: 106.5 g Third weighing: 106.1 3. Total volume of citric acid solution: 75.0 mL please help me with part Part 1: Preparation of the Primary Citric Acid Standard Mass of Citric Acid _________________________ Volume of Citric Acid Solution ____________ Moles of Citric Acid _________________ (Molar Mass = 192.0 g/mol) Molarity of Citric Acid Solution ____________
One way in which the useful metal copper is produced is by dissolving the mineral azurite, which contains copper(I) carbonate, in concentrated sulfuric acid The sulfuric acid reacts with the copper(I) carbonate to produce a blue solution of copper(I) sulfate. Scrap iron is then added to this solution, and pure copper metal precipitates out because of the following chemical reaction: Fe(s) + CuSO4(aq) -> Cu(s) + FeSO4(aq) Suppose an industrial quality-control cherist analyzes a sample from a copper processing plant in the following way. He adds powdered iron to a 300. mL copper(I) sulfate sample from the plant until no more copper will precipitate. He then washes, dries, and weighs the precipitate, and finds that it has a mass of 75. mg Calculate the oriqinal concentration of copper(I) sulfate in the sample. Round your answer to 2 significant digits.
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Compound	Cold Water solubility	Hot Water Solubility
Benzoic acid	0.42 g per 100 mL of water	5.79 g per 100 mL of water
Impurity	0.61 g per 100 mL of water	4.62 g per 100 mL of water