Concept explainers
Which of the following solutions contains the greatest number of particles? Support your answer.
.0 mL of 0 10 M sodium chloride
.0 mL of 0.10 M calcium chloride
.0 mL of 0.10 M iron(III) chloride
.0 mL of 0.10 M potassium bromide
.0 mL of 0.10 M sucrose (table sugar)
Interpretation:
The solution containing the greatest number of particles is to be predicted.
Concept Introduction:
There are many ways to determine the concentration of the solution. One of the most used methods is molarity. Molarity may be defined as the number of moles of the solute in one liter of the whole solution. Thus, the molarity can be calculated as,
Answer to Problem 11ALQ
The correct option is (b).
Explanation of Solution
Reason for correct option:
(b) The molarity of the
Substitute the values of molarity and volume in the given formula.
The total number of moles in the given solution is
To calculate the number of particles in a solution the formula used is,
Avogadro number is equal to the number of particles present in one mole, that is,
Substitute the values of moles and Avogadro number in the given formula.
One mole of
Reasons for incorrect options:
(a) The molarity of the
Substitute the values of molarity and volume in the given formula.
The total number of moles in the given solution is
To calculate the number of particles in a solution the formula used is,
Avogadro number is equal to the number of particles present in one mole, that is,
Substitute the values of moles and Avogadro number in the given formula.
One mole of
(c) The molarity of the
Substitute the values of molarity and volume in the given formula.
The total number of moles in the given solution is
To calculate the number of particles in a solution the formula used is,
Avogadro number is equal to the number of particles present in one mole, that is,
Substitute the values of moles and Avogadro number in the given formula.
One mole of
(d) The molarity of the
Substitute the values of molarity and volume in the given formula.
The total number of moles in the given solution is
To calculate the number of particles in a solution the formula used is,
Avogadro number is equal to the number of particles present in one mole, that is,
Substitute the values of moles and Avogadro number in the given formula.
One mole of
(e) The molarity of the
Substitute the values of molarity and volume in the given formula.
The total number of moles in the given solution is
To calculate the number of particles in a solution the formula used is,
Avogadro number is equal to the number of particles present in one mole, that is,
Substitute the values of moles and Avogadro number in the given formula.
The total number of particles present in the solution is
Want to see more full solutions like this?
Chapter 15 Solutions
Student Solutions Manual for Zumdahl/DeCoste's Introductory Chemistry: A Foundation, 9th
Additional Science Textbook Solutions
Chemistry: Structure and Properties
General, Organic, and Biological Chemistry: Structures of Life (5th Edition)
Principles of General, Organic, Biological Chemistry
- A student weighs out a 4.80-g sample of aluminum bromide, transfers it to a 100-mL volumetric flask, adds enough water to dissolve it, and then adds water to the 100-mL mark. What is the molarity of aluminum bromide in the resulting solution?arrow_forwardou have two solutions containing solute A. To determine which solution has the highest concentration of A in molarity, which of the following must you know? (There may be more than one answer.) the mass in grams of A in each solution the molar mass of A the volume of’ water added to each solution the total volume of the solution plain your answer.arrow_forward34. For each of the following solutions, the number of moles of solute is given, followed by the total volume of the solution prepared. Calculate the molarity of each solution. a. 0.754 mol KNO; 225 mL b. 0.0105 in of CaCl; 10.2 mL c. 3.15 mol NaCl; 5.00 L d. 0.499 mol NaBr; 100. mLarrow_forward
- m>5. Which of the following do you need to know to calculate the molarity of a salt solution? (There may be more than one answer.) the mass of salt added the molar mass of the salt the volume of water added the total volume of the solution plain your answer.arrow_forwardThe units of parts per million (ppm) and parts per billion (ppb) are commonly used by environmental chemists. In general, 1 ppm means 1 part of solute for every 106 parts of solution. Mathematically, by mass: ppm=gsolutegsolution=mgsolutekgsolution In the case of very dilute aqueous solutions, a concentration of 1.0 ppm is equal to 1.0 g of solute per 1.0 mL, which equals 1.0 g solution. Parts per billion is defined in a similar fashion. Calculate the molarity of each of the following aqueous solutions. a. 5.0 ppb Hg in H2O b. 1.0 ppb CHCl3 in H2O c. 10.0 ppm As in H2O d. 0.10 ppm DDT (C14H9Cl5) in H2Oarrow_forwardWithout consulting your textbook, list and explain the main postulates of the kinetic molecular theory for gases. How do these postulates help us account for the following bulk properties of a gas: the pressure of the gas and why the pressure of the gas increases with increased temperature; the fact that a gas tills its entire container; and the fact that the volume of a given sample of gas increases as its temperature is increased.arrow_forward
- Characterize strong electrolytes versus weak electrolytes versus nonelectrolytes. Give examples of each. How do you experimentally determine whether a soluble substance is a strong electrolyte, weak electrolyte, or nonelectrolyte?arrow_forwardYou wish to prepare 1 L of a 0.02-M potassium iodate solution. You require that the final concentration be within 1% of 0.02 M and that the concentration must be known accurately to the fourth decimal place. How would you prepare this solution? Specify the glassware you would use, the accuracy needed for the balance, and the ranges of acceptable masses of KIO3 that can be used.arrow_forwardCitric acid, which can be obtained from lemon juice, has the molecular formula C6H8O7. A 0.250-g sample of citric acid dissolved in 25.0 mL of water requires 37.2 mL of 0.105 M NaOH for complete neutralization. What number of acidic hydrogens per molecule does citric acid have?arrow_forward
- What is the molarity of pure water with a density of 1.00 g/mL?arrow_forwardWhat volume of 0.250 M HCI is required to neutralize each of the following solutions? a. 25.0 mL of 0.103 M sodium hydroxide, NaOH b. 50.0 mL of 0.00501 M calcium hydroxide, Ca(OH)2 c. 20.0 mL of 0.226 M ammonia, NH3 d. 15.0 mL of 0.0991 M potassium hydroxide, KOHarrow_forwardConsider a 13.0% solution of sulfuric acid, H2SO4,whose density is 1.090 g/mL. (a) Calculate the molarity of this solution. (b) To what volume should 100. mL of this solution bediluted to prepare a 1.10-M solution?arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningWorld of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
- General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage LearningChemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning