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Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243

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Chapter
Section
BuyFindarrow_forward

Chemistry: An Atoms First Approach

2nd Edition
Steven S. Zumdahl + 1 other
Publisher: Cengage Learning
ISBN: 9781305079243
Chapter 6, Problem 15Q
Textbook Problem
276 views

Of F2, CF4, and SF2, which substance is most soluble in water? Explain.

(a)

Interpretation Introduction

Interpretation:

The solubility of given substance should be explained.

Concept introduction:

Dipole moments occur when there is a separation of charge. They can occur between two ions in an ionic bond or between atoms in a covalent bond; dipole moments arise from differences in electronegativity. The larger the difference in electronegativity, the larger the dipole moment. The distance between the charge separation is also a deciding factor into the size of the dipole moment. The dipole moment is a measure of the polarity of the molecule.  Polar molecule is soluble in polar solvent and non-polar molecule is soluble in non-polar solvent.

Explanation of Solution

To find: The solubility of F2 molecule

F2 molecule

Water is a polar solvent and will dissolve other polar covalent solutes

(b)

Interpretation Introduction

Interpretation:

The solubility of given substance should be explained.

Concept introduction:

Dipole moments occur when there is a separation of charge. They can occur between two ions in an ionic bond or between atoms in a covalent bond; dipole moments arise from differences in electronegativity. The larger the difference in electronegativity, the larger the dipole moment. The distance between the charge separation is also a deciding factor into the size of the dipole moment. The dipole moment is a measure of the polarity of the molecule.

Polar molecule is soluble in polar solvent and non-polar molecule is soluble in non-polar solvent.

(c)

Interpretation Introduction

Interpretation:

The solubility of given substance should be explained.

Concept introduction:

Dipole moments occur when there is a separation of charge. They can occur between two ions in an ionic bond or between atoms in a covalent bond; dipole moments arise from differences in electronegativity. The larger the difference in electronegativity, the larger the dipole moment. The distance between the charge separation is also a deciding factor into the size of the dipole moment. The dipole moment is a measure of the polarity of the molecule.

Polar molecule is soluble in polar solvent and non-polar molecule is soluble in non-polar solvent.

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Chapter 6 Solutions

Chemistry: An Atoms First Approach
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Ch. 6 - You have a solution of table salt in water. What...Ch. 6 - You have a sugar solution (solution A) with...Ch. 6 - You add an aqueous solution of lead nitrate to an...Ch. 6 - Order the following molecules from lowest to...Ch. 6 - Why is it that when something gains electrons, it...Ch. 6 - Consider separate aqueous solutions of HCl and...Ch. 6 - Draw molecular-level pictures to differentiate...Ch. 6 - You need to make 150.0 mL of a 0.10-M NaCl...Ch. 6 - The exposed electrodes of a light bulb are placed...Ch. 6 - Differentiate between what happens when the...Ch. 6 - Consider the following electrostatic potential...Ch. 6 - Of F2, CF4, and SF2, which substance is most...Ch. 6 - A typical solution used in general chemistry...Ch. 6 - Which of the following statements is(are) true?...Ch. 6 - A student wants to prepare 1.00 L of a 1.00-M...Ch. 6 - List the formulas of three soluble bromide salts...Ch. 6 - When 1.0 mole of solid lead nitrate is added to...Ch. 6 - What is an acid and what is a base? An acid-base...Ch. 6 - A student had 1.00 L of a 1.00-M acid solution....Ch. 6 - Differentiate between the following terms. a....Ch. 6 - How does one balance redox reactions by the...Ch. 6 - Show how each of the following strong electrolytes...Ch. 6 - Match each name below with the following...Ch. 6 - Calcium chloride is a strong electrolyte and is...Ch. 6 - Commercial cold packs and hot packs are available...Ch. 6 - Calculate the molarity of each of these solutions....Ch. 6 - A solution of ethanol (C2H5OH) in water is...Ch. 6 - Calculate the concentration of all ions present in...Ch. 6 - Calculate the concentration of all ions present in...Ch. 6 - Which of the following solutions of strong...Ch. 6 - Which of the following solutions of strong...Ch. 6 - What mass of NaOH is contained in 250.0 mL of a...Ch. 6 - If 10. g of AgNO3 is available, what volume of...Ch. 6 - Describe how you would prepare 2.00 L of each of...Ch. 6 - How would you prepare 1.00 L of a 0.50-M solution...Ch. 6 - A solution is prepared by dissolving 10.8 g...Ch. 6 - A solution was prepared by mixing 50.00 mL of...Ch. 6 - Calculate the sodium ion concentration when 70.0...Ch. 6 - Suppose 50.0 mL of 0.250 M CoCl2 solution is added...Ch. 6 - A standard solution is prepaned for the analysis...Ch. 6 - A stock solution containing Mn2+ ions was prepaned...Ch. 6 - On the basis of the general solubility rules given...Ch. 6 - On the basis of the general solubility rules given...Ch. 6 - When the following solutions are mixed together,...Ch. 6 - When the following solutions are mixed together,...Ch. 6 - For the reactions in Exercise 47, write the...Ch. 6 - For the reactions in Exercise 48, write the...Ch. 6 - Write the balanced formula and net ionic equation...Ch. 6 - Give an example how each of the following...Ch. 6 - Write net ionic equations for the reaction, if...Ch. 6 - Write net ionic equations for the reaction, if...Ch. 6 - Separate samples of a solution of an unknown...Ch. 6 - A sample may contain any or all of the following...Ch. 6 - What mass of Na2CrO4 is required to precipitate...Ch. 6 - What volume of 0.100 M Na3PO4 is required to...Ch. 6 - What mass of solid aluminum hydroxide can be...Ch. 6 - What mass of barium sulfate can be produced when...Ch. 6 - What mass of solid AgBr is produced when 100.0 mL...Ch. 6 - What mass of silver chloride can be prepared by...Ch. 6 - A 100.0-mL aliquot of 0.200 M aqueous potassium...Ch. 6 - A 1.42-g sample of a pure compound, with formula...Ch. 6 - You are given a 1.50-g mixture of sodium nitrate...Ch. 6 - Write the balanced formula, complete ionic, and...Ch. 6 - Write the balanced formula, complete ionic, and...Ch. 6 - Write the balanced formula equation for the...Ch. 6 - What acid and what base would react in aqueous...Ch. 6 - What volume of each of the following acids will...Ch. 6 - What volume of each of the following bases will...Ch. 6 - Hydrochloric acid (75.0 mL of 0.250 M) is added to...Ch. 6 - A student mixes four reagents together, thinking...Ch. 6 - A 25.00-mL sample of hydrochloric acid solution...Ch. 6 - A 10.00-mL sample of vinegar, an aqueous solution...Ch. 6 - What volume of 0.0200 M calcium hydroxide is...Ch. 6 - A 30.0-mL sample of an unknown strong base is...Ch. 6 - A student titrates an unknown amount of potassium...Ch. 6 - The concentration of a certain sodium hydroxide...Ch. 6 - Assign oxidation states for all atoms in each of...Ch. 6 - Assign the oxidation state for nitrogen in each of...Ch. 6 - Assign oxidatioo numbers to all the atoms in each...Ch. 6 - Specify which of the following are...Ch. 6 - Specify which of the following equations represent...Ch. 6 - Consider the reaction between sodium metal and...Ch. 6 - Consider the reaction between oxygen (O2) gas and...Ch. 6 - Balance each of the following oxidationreduction...Ch. 6 - Balance each of the following oxidationreduction...Ch. 6 - You wish to prepare 1 L of a 0.02-M potassium...Ch. 6 - The figures below are molecular-level...Ch. 6 - An average human being has about 5.0 L of blood in...Ch. 6 - A 230.-mL sample of a 0.275-M CaCl2 solution is...Ch. 6 - Using the general solubility rules given in Table...Ch. 6 - Consider a 1.50-g mixture of magnesium nitrate and...Ch. 6 - A 1.00-g sample of an alkaline earth metal...Ch. 6 - A mixture contains only NaCl and Al2(SO4)3. A...Ch. 6 - The thallium (present as Tl2SO4) in a 9.486-g...Ch. 6 - A mixture contains only NaCl and Fe(NO3)3. 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Solution...

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