CHAPTER 8 - SOLUTIONS Submit Qu O Previous Page 9 of 35 E Next O References Use the References to access important values if needed for this question. A certain salt is known to have a solubility in water of 28.9g/100g water at 100°C and 10.9g/100g water at 20°C. The salt is dissolved in 230 g of water at 100°C until no more solid will dissolve How much salt will crystallize out when the solution is cooled to 20°C?

CHAPTER 8 - SOLUTIONS Submit Qu O Previous Page 9 of 35 E Next O References Use the References to access important values if needed for this question. A certain salt is known to have a solubility in water of 28.9g/100g water at 100°C and 10.9g/100g water at 20°C. The salt is dissolved in 230 g of water at 100°C until no more solid will dissolve How much salt will crystallize out when the solution is cooled to 20°C?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Match the following aqueous solutions with the appropriate letter from the column on the right. 1.0.13 m Cr(NO3)3 A. Lowest freezing point 2.0.23 m AgCH3COO 3.0.14 m CuCl2 B. Second lowest freezing point C. Third lowest freezing point D. Highest freezing point 4.0.49 m Ethylene glycol (nonelectrolyte) Submit Answer [Review Topics] [References] Use the References to access important values if needed for this question. In progress Retry Entire Group 9 more group attempts remaining Previo
A 690 g of 59% strontium bromide solution is cooled from 60 oC to a certain temperature. Upon addition of around 2 g of strontium bromide, excess solute above saturation started to crystallize. Total recovered crystals is 146.003 g. At what temperature is the solution cooled?
An aqueous solution containing 17.5 g of an unknown molecular compound in 100.g water was found to have a freezing point of -1.8°C. Calculate the molar mass of this unknown compound. You can use the following steps to solve this problem. Show your work. a. What is the freezing point change (AT) from pure water? The freezing point of water is 0.0°C. b. What is the freezing point depression constant (K₂) of water? c. What is the molality of the solution? (m= d. Solve the moles of the solute. moles of solute kg of solvent e. Knowing the mass of the compound, and the moles of the compound, solve the molar mass of the compound.
please explain
You add an excess of solid MX in 250 g water. You measure the freezing point and find it to be -0.015°C. What is the Ksp of the solid? Assume the density of the solution is 1.0 g/cm³. Kf for water is 1.86°C · kg/mol KsP 1.37x10^-5
The Van't Hoff factor does NOT A. indicate something about the intermolecular interactions occurring in a solution. B. depend on the number of ions that form when a solute dissolves. C. equal one (1) for a non-electrolyte. D. equal three (3) for calcium chloride. Which of the following solutions will have the lowest freezing point? A. 0.10 molal NaCl B. 0.10 molal sugar C. 0.10 molal K2SO4 D. 0.10 molal Caco3 Why is it important to maintain the rock salt/ice mixture at a temperature of -10oC? A. Because it can be done B. Due to the limitations of the temperature probes or thermometers being used in lab. C. Because that is as cold as a salt/water mixture can get D. So all 3 solutions being measured will freeze
4*) Consider the three solutions listed below that are prepared by dissolving 1 mole of the indicated solute in 1 kg of water: Solution 1: 1-mole KBr Solution 2: 1 mole CO(NH2)2Solution 3: 1 mole Na2SO4 a)Which solution will have the lowest vapor pressure of water above it? Explain. b)Which solution will have the highest vapor pressure of water above it? Explain.
Match the following aqueous solutions with the appropriate letter from the column on the right. A. Lowest freezing point B. Second lowest freezing point C. Third lowest freezing point D. Highest freezing point 1.0.20 m 2.7.8x10-2 m Cr(CH3COO) 3 Cr(CH3COO)2 Ethylene glycol (nonelectrolyte) KI 3.0.11 m 4.0.37 m
Name Time M T W R F The freezing point of pure benzene (CH,) is 5.50°C. The freezing point of a solution containing 5.00 g of an unknown non-dissociating solute in 444 g of benzene is 5.07°C. K, of benzene = 4.90°C/m. Show complete calculations for each question below. 1. What is the freezing point depression for this solution?
27. Find the freezing point of a solution of 990 g of CH3OH in 2.5 kg of water. Use the water f.R-depression constant: K(H,0) = = 1.86 °C/{mol(solute)/kg(solvent)} A) +123 °C B) +77 °C C) +23 °C D) -0.74 °C E) -23 °C
Explain why dissolving a nonvolatile solute in water affects the system in the following ways by selecting all true statements: Incorrect. The system has a higher boiling point than water. O The solute lowers the vapor pressure of the water. O The solute increases the vapor pressure of the water. O A higher temperature is required to obtain a vapor pressure of water equal to 1 atm. O A lower temperature is required to obtain a vapor pressure of water equal to 1 atm. O The normal boiling point is the temperature at which the vapor pressure is 1 atm. Hint Incorrect. The system has a lower freezing point than water. O Presence of the solute lowers the triple point. O Presence of the solute increases the triple point. O For all substances, the change in the triple point results in a lower freezing point. O For water, the change in the triple point results in a lower freezing point. O None of these. Hint
Calculate the vapor pressure of ethanol, CH;CH2OH, in a water solution containing 70.0% ethanol by volume at 19.0°C. The vapor pressure of pure ethanol at 19.0°C is 40.0 Torr. The density of ethanol is 0.789 g-mL¯1 and the density of water is 1.000 g-mL¯1. Torr 2 6. C 8 9. +/- х 100 3. 1.