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General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
Publisher: Cengage Learning
ISBN: 9781305580343

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Chapter
Section
BuyFindarrow_forward

General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
Publisher: Cengage Learning
ISBN: 9781305580343
Chapter 4, Problem 4.55QP
Textbook Problem
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Obtain the oxidation number for the element noted in each of the following.

  1. a Sn in SnO2
  2. b Ta in Ta2O3
  3. c Br in KBrO4
  4. d Os in K2O5O4

(a)

Interpretation Introduction

Interpretation:

The oxidation number of the given elements has to be found.

Concept introduction:

Oxidation number of an element is the number of electrons gained or lost by an atom or ion, during a chemical reaction.  Oxidation number can be positive negative or zero values.  If electrons are removed from an atom or ion, the process is known as oxidation.  Oxidation increases the oxidation number.  If electrons are added to an atom or ion, the process is known as reduction.  Reduction decreases the oxidation number.

Explanation of Solution

There are two oxygen atoms in SnO2 .  The oxidation number of tin is calculated as given

below.

Charge of one oxygen atom =-2

Charge of two oxygen atoms =-4

Total charge on SnO2=0

Charge on tin(x)

(b)

Interpretation Introduction

Interpretation:

The oxidation number of the given elements has to be found.

Concept introduction:

Oxidation number of an element is the number of electrons gained or lost by an atom or ion, during a chemical reaction.  Oxidation number can be positive negative or zero values.  If electrons are removed from an atom or ion, the process is known as oxidation.  Oxidation increases the oxidation number.  If electrons are added to an atom or ion, the process is known as reduction.  Reduction decreases the oxidation number.

(c)

Interpretation Introduction

Interpretation:

The oxidation number of the given elements has to be found.

Concept introduction:

Oxidation number of an element is the number of electrons gained or lost by an atom or ion, during a chemical reaction.  Oxidation number can be positive negative or zero values.  If electrons are removed from an atom or ion, the process is known as oxidation.  Oxidation increases the oxidation number.  If electrons are added to an atom or ion, the process is known as reduction.  Reduction decreases the oxidation number.

(d)

Interpretation Introduction

Interpretation:

The oxidation number of the given elements has to be found.

Concept introduction:

Oxidation number of an element is the number of electrons gained or lost by an atom or ion, during a chemical reaction.  Oxidation number can be positive negative or zero values.  If electrons are removed from an atom or ion, the process is known as oxidation.  Oxidation increases the oxidation number.  If electrons are added to an atom or ion, the process is known as reduction.  Reduction decreases the oxidation number.

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Chapter 4 Solutions

General Chemistry - Standalone book (MindTap Course List)
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Ch. 4.4 - Write the molecular equation and the net ionic...Ch. 4.4 - At times, we want to generalize the formula of...Ch. 4.5 - Obtain the oxidation numbers of the atoms in each...Ch. 4.6 - Use the half-reaction method to balance the...Ch. 4.7 - A sample of sodium chloride, NaCl, weighing 0....Ch. 4.7 - How many milliliters of 0. 163 M NaCl are required...Ch. 4.7 - How many moles of sodium chloride should be put in...Ch. 4.8 - You have a solution that is 1.5 M H2SO4 (sulfuric...Ch. 4.8 - Consider the following beakers. Each contains a...Ch. 4.9 - You are given a sample of limestone, which is...Ch. 4.10 - Nickel sulfate, NiSO4, reacts with sodium...Ch. 4.10 - A 5.00-g sample of vinegar is titrated with 0.108...Ch. 4.10 - Consider three flasks, each containing 0.10 mol of...Ch. 4 - Explain why some electrolyte solutions are...Ch. 4 - Define the terms strong electrolyte and weak...Ch. 4 - Explain the terms soluble and insoluble. Use the...Ch. 4 - What are the advantages and disadvantages of using...Ch. 4 - What is a spectator ion? Illustrate with a...Ch. 4 - What is a net ionic equation? What is the value in...Ch. 4 - What are the major types of chemical reactions?...Ch. 4 - Describe in words how you would prepare pure...Ch. 4 - Give an example of a neutralization reaction....Ch. 4 - Give an example of a polyprotic acid and write...Ch. 4 - Why must oxidation and reduction occur together in...Ch. 4 - Give an example of a displacement reaction. What...Ch. 4 - Why is the product of molar concentration and...Ch. 4 - Describe how the amount of sodium hydroxide in a...Ch. 4 - What is the net ionic equation for the following...Ch. 4 - An aqueous sodium hydroxide solution mixed with an...Ch. 4 - Which of the following compounds would produce the...Ch. 4 - In an aqueous 0.10 M HNO2 solution (HNO2 is a weak...Ch. 4 - The Behavior of Substances in Water Part 1: a...Ch. 4 - Working with Concentration (Molarity Concepts)...Ch. 4 - You need to perform gravimetric analysis of a...Ch. 4 - In this problem you need to draw two pictures of...Ch. 4 - You come across a beaker that contains water,...Ch. 4 - Three acid samples are prepared for titration by...Ch. 4 - Would you expect a precipitation reaction between...Ch. 4 - Equal quantities of the hypothetical strong acid...Ch. 4 - Try and answer the following questions without...Ch. 4 - If one mole of the following compounds were each...Ch. 4 - Using solubility rules, predict the solubility in...Ch. 4 - Using solubility rules, predict the solubility in...Ch. 4 - Using solubility rules, decide whether the...Ch. 4 - Using solubility rules, decide whether the...Ch. 4 - Write net ionic equations for the following...Ch. 4 - Write net ionic equations for the following...Ch. 4 - Lead(II) nitrate solution and sodium sulfate...Ch. 4 - Lithium carbonate solution reacts with aqueous...Ch. 4 - Write the molecular equation and the net ionic...Ch. 4 - Write the molecular equation and the net ionic...Ch. 4 - For each of the following, write molecular and net...Ch. 4 - For each of the following, write molecular and net...Ch. 4 - Classify each of the following as a strong or weak...Ch. 4 - Classify each of the following as a strong or weak...Ch. 4 - Complete and balance each of the following...Ch. 4 - Complete and balance each of the following...Ch. 4 - For each of the following, write the molecular...Ch. 4 - For each of the following, write the molecular...Ch. 4 - Complete the right side of each of the following...Ch. 4 - Complete the right side of each of the following...Ch. 4 - Write molecular and net ionic equations for the...Ch. 4 - Write molecular and net ionic equations for the...Ch. 4 - The following reactions occur in aqueous solution....Ch. 4 - The following reactions occur in aqueous solution....Ch. 4 - Write the molecular equation and the net ionic...Ch. 4 - Write the molecular equation and the net ionic...Ch. 4 - Obtain the oxidation number for the element noted...Ch. 4 - Obtain the oxidation number for the element noted...Ch. 4 - Obtain the oxidation number for the element noted...Ch. 4 - Obtain the oxidation number for the element noted...Ch. 4 - Determine the oxidation numbers of all the...Ch. 4 - Determine the oxidation numbers of all the...Ch. 4 - In the following reactions, label the oxidizing...Ch. 4 - In the following reactions, label the oxidizing...Ch. 4 - In the following reactions, label the oxidizing...Ch. 4 - In the following reactions, label the oxidizing...Ch. 4 - Balance the following oxidationreduction reactions...Ch. 4 - Balance the following oxidationreduction reactions...Ch. 4 - A sample of 0.0606 mol of iron(III) chloride,...Ch. 4 - A 50.0-mL volume of AgNO3 solution contains 0.0345...Ch. 4 - An aqueous solution is made from 0.798 g of...Ch. 4 - A sample of oxalic acid, H2C2O4, weighing 1.200 g...Ch. 4 - What volume of 0.120 M CuSO4 is required to give...Ch. 4 - How many milliliters of 0.126 M HClO4 (perchloric...Ch. 4 - An experiment calls for 0.0353 g of potassium...Ch. 4 - What is the volume (in milliliters) of 0.100 M...Ch. 4 - Heme, obtained from red blood cells, binds oxygen,...Ch. 4 - Insulin is a hormone that controls the use of...Ch. 4 - How many grams of sodium dichromate, Na2Cr2O7,...Ch. 4 - Describe how you would prepare 2.50 102 mL of...Ch. 4 - You wish to prepare 0.12 M HNO3 from a stock...Ch. 4 - Use the rearranged version of the dilution formula...Ch. 4 - A 8.50 g sample of KCl is dissolved in 66.0 mL of...Ch. 4 - Calculate the concentrations of each ion present...Ch. 4 - A chemist added an excess of sodium sulfate to a...Ch. 4 - A soluble iodide was dissolved in water. Then an...Ch. 4 - Copper has compounds with copper(I) ion or...Ch. 4 - Gold has compounds containing gold(I) ion or...Ch. 4 - A compound of iron and chlorine is soluble in...Ch. 4 - A 1.345-g sample of a compound of barium and...Ch. 4 - What volume of 0.230 M HNO3 (nitric acid) reacts...Ch. 4 - A flask contains 49.8 mL of 0.150 M Ca(OH)2...Ch. 4 - How many milliliters of 0.250 M H2SO4 (sulfuric...Ch. 4 - How many milliliters of 0.250 M KMnO4 are needed...Ch. 4 - A solution of hydrogen peroxide, H2O2, is titrated...Ch. 4 - A 3.75-g sample of iron ore is transformed to a...Ch. 4 - Magnesium metal reacts with hydrobromic acid to...Ch. 4 - Aluminum metal reacts with perchloric acid to...Ch. 4 - Nickel(II) sulfate solution reacts with sodium...Ch. 4 - Potassium sulfate solution reacts with barium...Ch. 4 - Decide whether a reaction occurs for each of the...Ch. 4 - Decide whether a reaction occurs for each of the...Ch. 4 - Complete and balance each of the following...Ch. 4 - Complete and balance each of the following...Ch. 4 - Describe in words how you would do each of the...Ch. 4 - Describe in words how you would do each of the...Ch. 4 - Classify each of the following reactions as a...Ch. 4 - Classify each of the following reactions as a...Ch. 4 - Consider the reaction of all pairs of the...Ch. 4 - Consider the reaction of all pairs of the...Ch. 4 - An aqueous solution contains 5.00 g of calcium...Ch. 4 - An aqueous solution contains 3.75 g of iron(III)...Ch. 4 - A stock solution of potassium dichromate, K2Cr2O7,...Ch. 4 - A 71.2-g sample of oxalic acid, H2C2O4, was...Ch. 4 - A solution contains 6.00% (by mass) NaBr (sodium...Ch. 4 - An aqueous solution contains 3.75% NH3 (ammonia)...Ch. 4 - A barium mineral was dissolved in hydrochloric...Ch. 4 - Bone was dissolved in hydrochloric acid, giving...Ch. 4 - You have a sample of a rat poison whose active...Ch. 4 - An antacid tablet has calcium carbonate as the...Ch. 4 - A sample of CuSO45H2O was heated to 110C, where it...Ch. 4 - A sample of CuSO45H2O was heated to 100C, where it...Ch. 4 - A water-soluble compound of gold and chlorine is...Ch. 4 - A solution of scandium chloride was treated with...Ch. 4 - A 0.608-g sample of fertilizer contained nitrogen...Ch. 4 - An antacid tablet contains sodium hydrogen...Ch. 4 - You order a glass of juice in a restaurant, only...Ch. 4 - If 45.1 mL of a solution containing 8.30 g of...Ch. 4 - If 38.2 mL of 0.248 M aluminum sulfate solution is...Ch. 4 - An aluminum nitrate solution is labeled 0.256 M....Ch. 4 - Zinc acetate is sometimes prescribed by physicians...Ch. 4 - Arsenic acid, H3AsO4, is a poisonous acid that has...Ch. 4 - When the following equation is balanced by the...Ch. 4 - Identify each of the following reactions as being...Ch. 4 - A 414-mL sample of 0.196 M MgBr2 solution is...Ch. 4 - Three 1.0-g samples of PbCl2, KCl, and CaCl2 are...Ch. 4 - A 25-mL sample of 0.50 M NaOH is combined with a...Ch. 4 - What is the molarity of pure water with a density...Ch. 4 - Nitric acid can be reacted with zinc according to...Ch. 4 - How many grams of precipitate are formed if 175 mL...Ch. 4 - You are asked to prepare 0.250 L of a solution...Ch. 4 - Potassium hydrogen phthalate (abbreviated as KHP)...Ch. 4 - Lead(II) nitrate reacts with cesium sulfate in an...Ch. 4 - Silver nitrate reacts with strontium chloride in...Ch. 4 - Elemental bromine is the source of bromine...Ch. 4 - Barium carbonate is the source of barium...Ch. 4 - Mercury(II) nitrate is treated with hydrogen...Ch. 4 - Mercury(II) nitrate is treated with hydrogen...Ch. 4 - Iron forms a sulfide with the approximate formula...Ch. 4 - A transition metal X forms an oxide of formula...Ch. 4 - What volume of a solution of ethanol, C2H6O, that...Ch. 4 - What volume of a solution of ethylene glycol,...Ch. 4 - A 10.0-mL sample of potassium iodide solution was...Ch. 4 - A 25.0-mL sample of sodium sulfate solution was...Ch. 4 - A metal, M, was converted to the sulfate,...Ch. 4 - A metal, M, was converted to the chloride MCl2....Ch. 4 - Phosphoric acid is prepared by dissolving...Ch. 4 - Iron(III) chloride can be prepared by reacting...Ch. 4 - An alloy of aluminum and magnesium was treated...Ch. 4 - An alloy of iron and carbon was treated with...Ch. 4 - Determine the volume of sulfuric acid solution...Ch. 4 - Determine the volume of sodium hydroxide solution...Ch. 4 - The active ingredients of an antacid tablet...Ch. 4 - The active ingredients in an antacid tablet...Ch. 4 - When using H2SO4 in aqueous reactions, many...

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