Design a detailed procedure (with estimated masses and volumes) that allows you to determine the enthalpy of salt dissolution (AHsalt dissolution), whether it is an endothermic or exothermic reaction. Hint: AHsalt dissolution = - AHwater. And AHwater = (sp. ht. of water) x (mass of water) x (Tf – Ti). Be careful that you don't exceed the solubility of the salt, which is given in the Lab Supplies section. Create a table to record the data for this lab exercise. Leave space for each piece of data you need to record during the lab (measurements, observations, etc.), as well as information you will look up and /or calculate

Design a detailed procedure (with estimated masses and volumes) that allows you to determine the enthalpy of salt dissolution (AHsalt dissolution), whether it is an endothermic or exothermic reaction. Hint: AHsalt dissolution = - AHwater. And AHwater = (sp. ht. of water) x (mass of water) x (Tf – Ti). Be careful that you don't exceed the solubility of the salt, which is given in the Lab Supplies section. Create a table to record the data for this lab exercise. Leave space for each piece of data you need to record during the lab (measurements, observations, etc.), as well as information you will look up and /or calculate

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter7: Statistical Data Treatment And Evaluation

Section: Chapter Questions

Problem 7.26QAP

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Although other solvents are available, dichloromethane(CH₂Cl₂) is still often used to “decaffeinate” drinks because thesolubility of caffeine in CH₂Cl₂ is 8.35 times that in water.(a) A 100.0-mL sample of cola containing 10.0 mg of caffeine is extracted with 60.0 mL of CH₂Cl₂. What mass of caffeine re-mains in the aqueous phase? (b) A second identical cola sampleis extracted with two successive 30.0-mL portions of CH₂Cl₂.What mass of caffeine remains in the aqueous phase after each extraction? (c) Which approach extracts more caffeine?
An excess amount of Ba(NO3)2 was added to 2 liters of water at 25 oC until the solution is saturated. Because Ba(NO3)2 is only slightly soluble in water, the excess Ba(NO3)2 was filtered out to get a solid-free mixture. The proponents of the experiment thought about using the concept of colligative properties, specifically boiling point elevation, to determine Ksp. It was observed in their experiments that the solution boils at 100.15 deg C. Kb of water = 0.51 K-kg/mol. Barium nitrate dissociates using: Solve the ff: a) Amount of Ba(NO3)2 dissolved in grams. MW of Ba(NO3)2 = 261.3 g/molb) Solubility product, Kspc) Vapor pressure of the solution in kPa
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At a certain temperature, the solubility of zinc(I) chromate is (7.6x10^-5) M. What is the Ksp? Report your answer to 2 sig figs. Note: Your answer is assumed to be reduced to the highest power possible
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the freezing point of the solution(in C to 2 decimal places)
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the vapor pressure of the solution to 3 decimal places in atm.
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Find the osmotic pressure in atm to three decimal places
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the boiling point of the solution(in C to 2 decimal places)
A solution is prepared by dissolving 40.00 g of NaCl (f.w. = 58.44 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 1 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the following: Boiling point of solution (in °C to two decimal places) Freezing point of solution (in °C to two decimal places) Vapor pressure of the solution (in atm to three decimal places) Osmotic pressure (in atm to three decimal places)
A solution is prepared by dissolving 40.00 g of MgCl2 (f.w. = 95.211 g mol–1), a non-volatile solute, in enough water (m.w. = 18.02 g mol–1) to result in exactly 2 L of solution at 25 °C. Assume the density of the solution is that of pure water (dsolution = 1.000 g mL–1). The ebullioscopic constant (Kb) for water is 0.513 °C m–1. The cryoscopic constant (Kf) for water is 1.86 °C m–1. The vapor pressure of pure water is 0.0313 atm. Determine the freezing point of the solution.
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