A student dissolves 14. g of stilbene (C,H,,) in 450. mL of a solvent with a density of 1.09 g/mL. The student notices that the volume of the solvent does not change when the stilbene dissolves in it. Calculate the molarity and molality of the student's solution. Be sure each of your answer entries has the correct number of significant digits. molarity = Ox10 몸 molality

A student dissolves 14. g of stilbene (C,H,,) in 450. mL of a solvent with a density of 1.09 g/mL. The student notices that the volume of the solvent does not change when the stilbene dissolves in it. Calculate the molarity and molality of the student's solution. Be sure each of your answer entries has the correct number of significant digits. molarity = Ox10 몸 molality

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter8: Solutions

Section: Chapter Questions

Problem 8.53EP

See similar textbooks

Related questions

Q: A solution contains 20.5 g of sodium chloride dissolved in sufficient water to give a total mass of…

A: Molality is represented by ‘m’ and is defined as the number of moles of solute present in 1 kg of…

Q: In general, the solubility of solids increases with increasing solvent temperature. A. True B.…

A: Solubility is defined as the amount of substance that will dissolve in a given amount of a solvent…

Q: What is a colligative solution property? Name three of them.

A: Measurements of colligative properties are important because they help in the determination of molar…

Q: A student dissolves 7.9 g of glucose (C,H,,06) in 400. mL of a solvent with a density of 0.83 g/mL.…

Q: What is the mathematical definition of molality?

Q: A student dissolves 16. g of styrene (CgHg) in 250. mL of a solvent with a density of 0.93 g/mL. The…

A: Given: mass of styrene ( C8H8 ) = 16 gMolar mass of C8H8 = 104.15 g/molAs we know, No.…

Q: How the solubility of gases in liquids effected by temperature and pressure?

A: Gases and liquids are the state of matter. Gaseous particles are far away from each other as they…

Q: As the concentration of a solute in a solution increases, the freezing point of the solution…

A: Freezing point is the temperature at which the liquid changes to solid. The product of the vapor…

Q: The molality of the solution is ____ m. The boiling point of the solution is _____°C

A: Given that: Mass of manganese nitrate = 10.65 g Molar mass of manganese nitrate = 179.0…

Q: Classify the steps involved in the formation of a solution as being endothermic or exothermic. Drag…

A: A substance which is present in less quantity in a solution is called a solute. To dissolve the…

Q: Also what is the freezing point of solution?

A: Application of colligative properties 2.67 L or 0.00267 ml of ethane 1,2 -diol. or 0.00267 x…

Q: Colloidal particles settle out on standing. True False

A: A system is said to be in colloidal state if particles of one or more component have size range 10…

Q: solute will have the lowest freezing

Q: A student dissolves 14. g of stilbene (CH12) in 450. mL of a solvent with a density of 1.09 g/mL.…

A: Molarity: The mole of the solute dissolved in one liter of the solution is known as the molarity of…

Q: 12) Which of the diagrams in the figure best represents an aqueous solution of sodium sulfate? I…

A: Answer:- This question is answered by using the simple concept of solubility which follows the…

Q: 1. a. What is a colligative property? b. Name 4 colligative properties

A: The question is based on the concepts of solutions. colligative property is one of the important…

Q: how colloidal solutions can be purified?

A: There are various methods of purification of colloidal solutions.

Q: A solution contains 69.8 g of sodium chloride dissolved in sufficient water to give a total mass of…

A: Weight of NaCl = 69.8 gm Total mass = 126.1 gm -> molality is number of moles of solute in 1 kg…

Q: Differentiate molality and molarity. Name other ways of describing quantitatively compositions of…

Q: What is osmotic pressure? Why it is a colligative property?

A: Osmotic pressure can be defined as the minimum pressure that must be applied to a solution to halt…

Q: What usually happens to the solubility of solids as temperatures decreases?

A: Solubility of a substance dependent on the temperature.

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

100%

Calculating molality.

A student dissolves 14. g of stilbene (C14H2) in 450. mL of a solvent with a density of 1.09 g/mL. The student notices that the volume of the
14
solvent does not change when the stilbene dissolves in it.
Calculate the molarity and molality of the student's solution. Be sure each of your answer entries has the correct number of significant digits.
molarity
molality

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

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

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

Instead of using NaCl to melt the ice on your sidewalk you decide to use CaCl2. If you add 35.0 g of CaCl2 to 150. g of water, what is the freezing point of the solution? (Assume i = 2.7 for CaCl2.)
Calculate the molality of a solution made by dissolving 115.0 g ethylene glycol, HOCH2CH2OH, in 500. mL water. The density of water at this temperature is 0.978 g/mL. Calculate the molarity of the solution.
A patient has a “cholesterol count” of 214. Like manyblood-chemistry measurements,this result is measured inunits of milligrams per deciliter (mgdL1). Determine the molar concentration of cholesterol inthis patient’s blood, taking the molar mass of cholesterolto be 386.64gmol1. Estimate the molality of cholesterol in the patient’sblood. If 214 is a typical cholesterol reading among men inthe United States, determine the volume of such bloodrequired to furnish 8.10 g of cholesterol.
You have read that adding a solute to a solvent can both increase the boiling point and decrease the freezing point. A friend of yours explains it to you like this: The solute and solvent can be like salt in water. The salt gets in the way of freezing in that it blocks the water molecules from joining together. The salt acts like a strong bond holding the water molecules together so that it is harder to boil. What do you say to your friend?
What mass of a 4.00% NaOH solution by mass contains 15.0 g of NaOH?
Fluoridation of city water supplies has been practiced in the United States for several decades. It is done by continuously adding sodium fluoride to water as it comes from a reservoir. Assume you live in a medium-sized city of 150,000 people and that 660 L (170 gal) of water is used per person per day. What mass of sodium fluoride (in kilograms) must be added to the water supply each year (365 days) to have the required fluoride concentration of 1 ppm (part per million)that is, 1 kilogram of fluoride per 1 million kilograms of water? (Sodium fluoride is 45.0% fluoride, and water has a density of 1.00 g/cm3.)
How do colloids differ from solutions with regard to dispersed particle size and homogeneity?
Sodium chloride (NaCl) is commonly used to melt ice on roads during the winter. Calcium chloride (CaCl2) is sometimes used for this purpose too. Let us compare the effectiveness of equal masses of these two compounds in lowering the freezing point of water, by calculating the freezing point depression of solutions containing 200. g of each salt in 1.00 kg of water. (An advantage of CaCl2 is that it acts more quickly because it is hygroscopic, that is. it absorbs moisture from the air to give a solution and begin the process. A disadvantage is that this compound is more costly.)
Insulin is a hormone responsible for the regulation of glucose levels in the blood. An aqueous solution of insulin has an osmotic pressure of 2.5 mm Hg at 25C. It is prepared by dissolving 0.100 g of insulin in enough water to make 125 mL of solution. What is the molar mass of insulin?
Refer to Figure 13.10 ( Sec. 13-4b) to determine whether these situations would result in an unsaturated, saturated, or supersaturated solution. 120. g RbCl is added to 100. g H2O at 50 °C. 30. g KCl is dissolved in 100. g H2O at 70 °C. 20. g NaCl is dissolved in 50. g H2O at 60 °C. Figure 13.10 Solubility of ionic compounds versus temperature.
Consider three test tubes. Tube A has pure water. Tube B has an aqueous 1.0 m solution of ethanol, C2H5OH. Tube C has an aqueous 1.0 m solution of NaCl. Which of the following statements are true? (Assume that for these solutions 1.0m=1.0M.) (a) The vapor pressure of the solvent over tube A is greater than the solvent pressure over tube B. (b) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube A. (c) The freezing point of the solution in tube B is higher than the freezing point of the solution in tube C. (d) The boiling point of the solution in tube B is higher than the boiling point of the solution in tube C. (e) The osmotic pressure of the solution in tube B is greater than the osmotic pressure of the solution in tube C.
6-111 As noted in Section 6-8C, the amount of external pressure that must be applied to a more concentrated solution to stop the passage of solvent molecules across a semipermeable membrane is known as the osmotic pressure The osmotic pressure obeys a law similar in form to the ideal gas law (discussed in Section 5-4), where Substituting for pressure and solving for osmotic pressures gives the following equation: RT MRT, where M is the concentration or molarity of the solution. (a) Determine the osmotic pressure at 25°C of a 0.0020 M sucrose (C12H22O11) solution. (b) Seawater contains 3.4 g of salts for every liter of solution. Assuming the solute consists entirely of NaCl (and complete dissociation of the NaCI salt), calculate the osmotic pressure of seawater at 25°C. (c) The average osmotic pressure of blood is 7.7 atm at 25°C. What concentration of glucose (C6H12O6) will be isotonic with blood? (d) Lysozyme is an enzyme that breaks bacterial cell walls. A solution containing 0.150 g of this enzyme in 210. mL of solution has an osmotic pressure of 0.953 torr at 25°C. What is the molar mass of lysozyme? (e) The osmotic pressure of an aqueous solution of a certain protein was measured in order to determine the protein's molar mass. The solution contained 3.50 mg of protein dissolved in sufficient water to form 5.00 mL of solution. The osmotic pressure of the solution at 25°C was found to be 1.54 torr. Calculate the molar mass of the protein.