The boiling point of a liquid will change when a solute is added. Explain how the addition of salt impacts the boiling point of water. Calculate the boiling point change for a given concentration. Given that water's boiling point is 100°C and the elevation constant (Kb) is 0.512 °Ckg/mol,

The boiling point of a liquid will change when a solute is added. Explain how the addition of salt impacts the boiling point of water. Calculate the boiling point change for a given concentration. Given that water's boiling point is 100°C and the elevation constant (Kb) is 0.512 °Ckg/mol,

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

Related questions

Q: The solubility of Mg(OH), in water at 25 °C is measured to be 0.0096 Use this information to…

Q: onsider the solubilities of a particular solute at two different temperatures.…

A: For a saturated solution, the amount of solute dissolved is equal to the solubility . that is…

Q: 4. A 16.0 °C. Determine the solubility in g solute/100 g H₂O. Determine the mole fraction of solute…

A: Answer: Saturated solution is the type of solution in which no more solute can be dissolved in…

Q: a reaction, 0.700g of Ca is added to 75.0mL of 1.0M HCl. Once the reaction is completed as…

A: “Since you have posted multiple subparts questions, we will provide the solution only to the first…

Q: The normal freezing point of a certain liquid X is -4.4 °C, but when 12.06 g of urea freezes at -8.3…

A: The normal freezing point of a certain liquid X is -4.4o CWhen 12.06 g of urea is dissolved in 350…

Q: Imagine that a few tenths of a mole of each compound is dissolved in a liter of water. Then, write…

Q: The boiling point of a liquid will change when a solute is added. Explain how the addition of salt…

Q: Determine the freezing point of a solution consisting of 0.350 m KCl in water. The freezing point…

A: Cryoscopic constant of water is 1.86oC/molal Van’t Hoff factor (i) is 2 since each KCl give on one…

Q: Determine the freezing point of a solution consisting of 0.350 m KCl in water. The freezing point…

A: Given Data: The molarity of the solution is 0.350 m. The value of Kf, of water is 1.86 °C/m. The…

Q: The freezing point of water is 0.00 °C at 1 atmosphere. How many grams of zinc chloride (136.3…

Q: The boiling point of water is 100.00 °C at 1 atmosphere. A student dissolves 10.01 grams of zinc…

Q: 1. The solubility of L-glutamic acid (an amino acid) in water has been determined to be as follows…

A: Solubility: When the maximum amount of solute is dissolve in the solvent is called solubility. On…

Q: A certain liquid X has a normal boiling point of 114.40 °C and a boiling point elevation constant K…

A: The boiling point of the pure liquid = 114.40 0C. The boiling point of the solution = 115.1 0C.…

Q: Which of the following statements is the most true regarding the solubility of KCl in water? The…

Q: When sodium chloride (NaCl) dissolves in water, energy is absorbed (endothermic process). Which of…

A: The strong ionic bonds are dissolved when NaCl dissolves in water (requiring heat energy) and the…

Q: What is the boiling point of 0.600 m lactose in water? Use 100.00 °C as the boiling point of water.…

A: Molality of lactose = 0.600 m Boiling point of water = 100.00°C -> Boiling point elevation is…

Q: An aqueous solution has 0.0065 g of oxygen dissolved in 2.5 L of water. Calculate the dissolved…

Q: The boiling point of water is 100.0°C at 1 atmosphere. How many grams of aluminum chloride (133.3…

Q: 1. The boiling point elevation of an aqueous sucrose solution is found to be 0.39°C. What mass of…

A: Elevation in boiling point : Boiling point elevation indicates to the increase in the boiling point…

Q: At 20.0∘C, the concentration of dissolved oxygen in water exposed to gaseous oxygen at a partial…

Q: At 70 °C, the solubility of an unknown solute is 65.7 g/100.0 g of water. What mass of the solute…

Q: At 298 K, the Henry's law constant for oxygen is 0.00130 M/atm. Air is 21.0% oxygen. At 298 K, what…

Q: water. When 8.46 g of CsBr is dissolved in 117.00 g of water, the temperature of the solution…

A: We have to find enthalpy of dissolution of CsBr (in kJ/mol). Given m = 117g C = 4.184 J/g °C ∆T…

Q: q Preq Visited 2req [Review Topics] [References] Use the References to access important values if…

A: B.p of ethanol= 78.500 0C B.p of solution= 78.723 0C Kb of ethanol =1.22 0C/m Mass of ethanol=204.5…

Q: The freezing point of water is 0.00 °C at 1 atmosphere. How many grams of iron(III) bromide (295.6…

A: The formula of the depression in the freezing point is = ..............(1)Where, the ∆Tf is the…

Q: Remember that the boiling point elevation constant for water is Kb = 0.512 C/kg, and the freezing…

Q: Determine the freezing point of a solution consisting of 0.350 m KCl in water. The freezing point…

Q: [References] Use the References to access important values if needed for this question. The boiling…

Q: Which temperature would allow the highest solubility of CO2 in water? 40C 50C 60C 70C

A: A multiple choice question based on the solubility of gases, which is to be accomplished.

Q: 3. If a solution is made up by mixing 6.0 g of benzoic acid in 1.00 L of water at 42 °C, would the…

A: In this question we have to define the saturated Solution of the benzoic acid and water, first of…

Q: Which of the following phenomena is best described by Henry’s Law? a. Increasing temperature favors…

A: Henry's law is exclusively for gases, it is used to study the solubility of gasesIt states that at…

Q: The molar mass of an enzyme was measured by dissolving the 3.221 grams of the enzyme in 1.00 liter…

A: Concept based on the osmotic pressure of the solution. By using osmotic pressure of solution…

Q: The boiling point of water is 100.0°C at 1 atmosphere. How many grams of silver acetate (166.9…

A: Answer:- This question is answered by using the simple concept of elevation in boiling point. Using…

Q: 10.0 g ZnCl2 is dissolved in 100.0 g of water at 23.6 °C. The solution reaches a temperature of 36.5…

A: Information of question

Q: Select one of the following formulas and describe all that it tells you about the ç.p's it…

A: Since we can choose any one formula, here I am describing H2S.

Q: What is the boiling point of 0.400 m lactose in water? Use 100.00 °C as the boiling point of water.…

Concept explainers

Solutions

Solutions can be considered as homogeneous mixtures which contain two or more than two chemical substances. The chemical substance which is the greater part is defined as solvent. And the chemical substance that is dissolved in a solvent is referred to as solute. Solution chemistry plays an important role in chemistry since it supports many commercial applications of solutions.

Question

The boiling point of a liquid will
change when a solute is added.
Explain how the addition of salt
impacts the boiling point of
water. Calculate the boiling point
change for a given
concentration.
Given that water's boiling point
is 100°C and the elevation
constant (Kb) is 0.512 °Ckg/mol,
calculate the boiling point
increase for a 4.50 molal
solution (moles/kg) of aqueous
NaCl. Assume ideal behavior of
the ions.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

Step 2

Step 3

Step 4

Trending now

This is a popular solution!

Step by step

Solved in 4 steps

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

None
1 for a certain substance X. When 38.6 g of urea (NH,), CO) The molal boiling point elevation constant K, =1.54 °C·kg mol are dissolved in 950. g of X, the 9. 2 solution boils at 113.3 °C. Calculate the boiling point of pure X. Round your answer to 4 significant digits. x10
Use the solubility curve below to determine how much NaNO, can dissolve in 300 g of water at 10 degrees Celsius. 100 90 NANO, 80 70 60 CaCl 50 Pb(NO)2 40 KCI NaCi 30 20 KCIO, 10 Ce,(SO 10 20 30 40 50 60 70 80 90 100 Temperature (°C) O 240 g O 160 g O 40 g O 80 g Solubility (g of salt in 100 g H,O) EONY K,Cr,O,
A certain liquid X has a normal freezing point of 0.90°C and a freezing point depression constant Kf=6.96·°C·kgmol−1.A solution is prepared by dissolving some barium hydroxide (Ba(OH)2) in 900.g of X. This solution freezes at−3.7°C. Calculate the mass of Ba(OH)2 that was dissolved. Round your answer to 2 significant digits.
A solution is prepared by adding 0.108 moles of Mg(NO3)2 to 1.00 mole of water. Calculate the vapor pressure of this solution at 55 °C.The vapor pressure of pure water at 55 °C is 118.1 Torr. Assume that the Mg(NO3)2 is completely dissociated. 365 Torr 28.9 Torr 89.2 Torr 107 Torr 97.1 Torr
A certain liquid X has a normal freezing point of 7.00°C and a freezing point depression constant =Kf 7.41·°C·kgmol−1. A solution is prepared by dissolving some iron(III) chloride (FeCl3) in 700.g of X. This solution freezes at 3.5°C. Calculate the mass of FeCl3 that was dissolved. Be sure your answer is rounded to the correct number of significiant digits.
Calculate the dissolved oxygen in mg/L at an altitude of 1,000 m above sea level that has an atmospheric pressure of 0.89 atm; assuming constant temperature of 25 °C. The Henry Law constant (kH) for the solubility of O2 in water at 25 ° C is 1.3 x 10-3 mol/L.atm.
Vapor pressure of water is 31.8 torr at 30°C. If 17.9 g AlCl3 is dissolved in 100. g of water, calculate the vapor pressure of the solution. O 29.0 torr 28.2 torr O26.5 torr O 31.0 torr
Suppose a group of students tell you that they added solid sodium chloride NaCls to 35 mL of deionized water and they did not record how many grams of NaCl they added but they got a freezing point depression of 1.25°C. Calculate how many grams of NaCl the students added. The pure freezing point of water is 0.00°C and the freezing point depression constant (K) of water is 1.858 °C/m. Remember that NaCl is a solid salt and an ionic compound therefore it contributes a negligible amount to the overall additive volume and keep track of its van't Hoff factor. The density of water at 20°C is 0.9982 g/mL.
A solution contains 6.56 g of KCl per 100 g of water at 30 °C. KNO, NANO, 100 CaCl, Pb(NO,), 90 - Use the solubility graph to determine if the KCl solution K,Cr,O, 80 is saturated, unsaturated or supersaturated. 70 - supersaturated 60 KCI saturated Na,SO, 50 unsaturated 40 NaCl 30 KCIO, 20- A solution contains 90.0 g of CaCl, per 100 g of water at 10 °C. 10 - 10 20 30 40 50 60 70 80 90 100 Temperature (°C) Use the solubility graph to determine if the CaCI, solution is saturated, unsaturated or supersaturated. supersaturated unsaturated saturated Solubility (g solute in 100 g H,O)
The salt cesium sulfate is soluble in water. When 22.7 g of Cs2SO4 is dissolved in 120.00 g of water, the temperature of the solution decreases from 25.00 to 22.96 °C. Based on this observation, calculate the enthalpy of dissolution of Cs2SO4 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible.