Flow Diagram for Mixtures You are given a mixture of three solids: AgCl, NaCl, and PbCl2. The following information is important. NaCl is soluble in hot and cold water. AgCl is insoluble in hot or cold water. PbCl2 is soluble in hot water and insoluble in cold water. Using this information, complete a flow diagram for their separation. NaCl, AgCl, PBC12 Step 1. Add cold water and filter. Pocla Step 3. Add hot water and filter Step 2. Heat to dryness. Step 4. Dry Step 5. Cool solution and filter. Step 6. Dry On the back of this page create another flow diagram for a mixture of the same three solids--AgCl, NaCI, and PbCl2. In your separation this time, Step 1 is adding hot water. Be sure to include all steps and finish with the three solids, each separate and dry.

Flow Diagram for Mixtures You are given a mixture of three solids: AgCl, NaCl, and PbCl2. The following information is important. NaCl is soluble in hot and cold water. AgCl is insoluble in hot or cold water. PbCl2 is soluble in hot water and insoluble in cold water. Using this information, complete a flow diagram for their separation. NaCl, AgCl, PBC12 Step 1. Add cold water and filter. Pocla Step 3. Add hot water and filter Step 2. Heat to dryness. Step 4. Dry Step 5. Cool solution and filter. Step 6. Dry On the back of this page create another flow diagram for a mixture of the same three solids--AgCl, NaCI, and PbCl2. In your separation this time, Step 1 is adding hot water. Be sure to include all steps and finish with the three solids, each separate and dry.

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

Chapter14: Chemical Equilibrium

Section: Chapter Questions

Problem 94AP

See similar textbooks

Similar questions

Write the balanced NET ionic equation for the reaction when aqueous SrBr₂ and aqueous K₂SO₄ are mixed in solution to form solid SrSO₄ and aqueous KBr. Be sure to include the proper phases for all species within the reaction.
4.0g of potassium hydrogen tartrate was added to 300mL distilled water. The temperature of the solution is 23.1C. The liquid was filtered and 50mL of the filtered solution was transferred to 250mL beaker, two drops of phenolpthalein was added to the 250mL beaker. The concentration of NaOH is 1.0 M that is filled in the 2mL graduate pipette, single drops of NaOH was added to the 250mL beaker until the solution turns pink and the potassium hydrogen tartrate reach the endpoint. The datd of four trials was collected. Please answer the following questions 4) calculate ksp for potassium hydrogen tartrate for each trial and average ksp for thr experiment 5) calculate the percent error in you value of ksp using reference that is found as the theoretical value. 6) why was the temperature of the saturated solution recorded?
4.0g of potassium hydrogen tartrate was added to 300mL distilled water. The temperature of the solution is 23.1C. The liquid was filtered and 50mL of the filtered solution was transferred to 250mL beaker, two drops of phenolpthalein was added to the 250mL beaker. The concentration of NaOH is 1.0 M that is filled in the 2mL graduate pipette, single drops of NaOH was added to the 250mL beaker until the solution turns pink and the potassium hydrogen tartrate reach the endpoint. The datd of four trials was collected. Please answer the following questions 1) calculate the total volume and moles of NaOH required to reach the endpoint for each trial. 2) calculate the molar solubility of potassium hydrogen tartate ( in mol/L) for each trial. 3) calculate the average molar solubility of potassium hydrogen tartate for the four trials. What is the average solubility of potassium hydrogen tartrate in g/L? 4) calculate ksp for potassium hydrogen tartrate for each trial and average ksp for thr…
Saturated aqueous sodium chloride (d = 1.2 g/mL) is added to the followingmixtures in order to dry the organic layer. Which layer is likely to be on thebottom in each case?a. Sodium chloride layer or a layer containing a high-density organic compound dissolved in methylene chloride (d = 1.4 g/mL)b. Sodium chloride layer or a layer containing a low-density organic compound dissolved in methylene chloride (d = 1.1 g/mL)
True or false reflux is the process of heating a reaction mixture and condensing the solvent vaports back into the reaction vessel, whereas boiling is the process of heating a reaction mixture and allowing tye vapor to eacape
A student using a calibrated solution calorimeter measured a temperature decrease of 1.10 K when 1.00 g of KNO3 was added to 74.40 g of deionized water in the calorimeter. The specific heat capacity of the solution calorimeter was found to be 4.15 J/gK. Calculate the experimental value of the molar heat of solution of KNO3, ΔH soln. Was the dissolution of this salt exothermic or endothermic?
In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) Question: Is the reaction balanced?
In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) What were the actual, theoretical, and percent yields of sodium chloride (NaCl)?
In an experiment, 0.500 grams of sodium bicarbonate were added to an evaporating dish and an excess of 6.0 M hydrochloric acid was added. The bicarbonate bubbled with the addition of the aqueous HCl. The evaporating dish was gently swirled until the bubbling stopped. The evaporating dish was placed on a hot plate and heated carefully to dryness so that it was completely dry and at constant mass. The amount of sodium chloride obtained from the evaporating dish was 0.114 g. The reaction is given below. NaHCO3 (s) + HCl (aq) ---> NaCl (s) + CO2 (g) + H2O (l) Question: What were the actual, theoretical, and percent yields of sodium chloride (NaCl)?
A student determines the molar mass of a liquid unknown by the method used in this experiment. She found that the equilibrum temperature of a mixture of ice and water was 1.0 degrees C on her thermometer. When she added 11.1 g of her unknown sample to the mixture, the temperature, after thorough stirring, fell to -3.0 degrees C. She then poured off the solution through a screen into a beaker. The mass of the solution was 90.4 g. Kf=1.86 degrees C/m How much water was in the decanted solution? What did she find to be the molar mass of the unknown liquid, assuming she made the calculation properly?
A student determines the molar mass of a liquid unknown by the method used in this experiment. She found that the equilibrum temperature of a mixture of ice and water was 1.0 degrees C on her thermometer. When she added 11.1 g of her unknown sample to the mixture, the temperature, after thorough stirring, fell to -3.0 degrees C. She then poured off the solution through a screen into a beaker. The mass of the solution was 90.4 g. Kf=1.86 degrees C/m 1. What is the freezing point depression? 2. What is the molality of the unknown solution? 3. How much unknown liquid was in the decanted solution?
The solubility of Ni(OH)2 in water at 25c is measured to be 4.9 x 10^-4 g/L. Use this information to calculate Ksp for Ni(OH)2.