Chemistry (Instructor's)
10th Edition
ISBN: 9781305957787
Author: ZUMDAHL
Publisher: CENGAGE L
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 4, Problem 40E
High-density lipoprotein (HDL) cholesterol is the “good” cholesterol because adequate levels reduce the risk of heart disease and stroke. HDL levels between 40. and 59 mg/dL are typical for a healthy individual. What is this range of HDL cholesterol in units of mol/L? The formula for cholesterol is C27H46O.
Expert Solution & Answer
Trending nowThis is a popular solution!
Chapter 4 Solutions
Chemistry (Instructor's)
Ch. 4 - The (aq) designation listed after a solute...Ch. 4 - Characterize strong electrolytes versus weak...Ch. 4 - Distinguish between the terms slightly soluble and...Ch. 4 - Molarity is a conversion factor relating moles of...Ch. 4 - What is a dilution? What stays constant in a...Ch. 4 - When the following beakers are mixed, draw a...Ch. 4 - Differentiate between the formula equation, the...Ch. 4 - What is an acid-base reaction? Strong bases are...Ch. 4 - Define the terms oxidation, reduction, oxidizing...Ch. 4 - Assume you have a highly magnified view of a...
Ch. 4 - You have a solution of table salt in water. What...Ch. 4 - You have a sugar solution (solution A) with...Ch. 4 - You add an aqueous solution of lead nitrate to an...Ch. 4 - Order the following molecules from lowest to...Ch. 4 - Why is it that when something gains electrons, it...Ch. 4 - Consider separate aqueous solutions of HCl and...Ch. 4 - Prob. 8ALQCh. 4 - On the basis of the general solubility rules given...Ch. 4 - Prob. 11ALQCh. 4 - The exposed electrodes of a light bulb are placed...Ch. 4 - The equation Ag(aq) + Cu(s) Cu2(aq) + Ag(s) has...Ch. 4 - In balancing oxidation-reduction reactions, why is...Ch. 4 - Differentiate between what happens when the...Ch. 4 - A typical solution used in general chemistry...Ch. 4 - Prob. 19QCh. 4 - A student wants to prepare 1.00 L of a 1.00-M...Ch. 4 - List the formulas of three soluble bromide salts...Ch. 4 - When 1.0 mole of solid lead nitrate is added to...Ch. 4 - What is an acid and what is a base? An acid-base...Ch. 4 - A student had 1.00 L of a 1.00-M acid solution....Ch. 4 - Differentiate between the following terms. a....Ch. 4 - Prob. 27ECh. 4 - Match each name below with the following...Ch. 4 - Calcium chloride is a strong electrolyte and is...Ch. 4 - Commercial cold packs and hot packs are available...Ch. 4 - Calculate the molarity of each of these solutions....Ch. 4 - A solution of ethanol (C2H5OH) in water is...Ch. 4 - Calculate the concentration of all ions present in...Ch. 4 - Prob. 34ECh. 4 - Prob. 35ECh. 4 - Prob. 36ECh. 4 - Prob. 37ECh. 4 - If 10. g of AgNO3 is available, what volume of...Ch. 4 - The sodium level in a patients blood was measured...Ch. 4 - High-density lipoprotein (HDL) cholesterol is the...Ch. 4 - A solution is prepared by dissolving 10.8 g...Ch. 4 - A solution was prepared by mixing 50.00 mL of...Ch. 4 - Calculate the sodium ion concentration when 70.0...Ch. 4 - Suppose 50.0 mL of 0.250 M CoCl2 solution is added...Ch. 4 - Prob. 47ECh. 4 - A stock solution containing Mn2+ ions was prepaned...Ch. 4 - On the basis of the general solubility rules given...Ch. 4 - On the basis of the general solubility rules given...Ch. 4 - When the following solutions are mixed together,...Ch. 4 - When the following solutions are mixed together,...Ch. 4 - For the reactions in Exercise 47, write the...Ch. 4 - For the reactions in Exercise 48, write the...Ch. 4 - Write the balanced formula and net ionic equation...Ch. 4 - Give an example how each of the following...Ch. 4 - Write net ionic equations for the reaction, if...Ch. 4 - Write net ionic equations for the reaction, if...Ch. 4 - Separate samples of a solution of an unknown...Ch. 4 - A sample may contain any or all of the following...Ch. 4 - What mass of Na2CrO4 is required to precipitate...Ch. 4 - What volume of 0.100 M Na3PO4 is required to...Ch. 4 - What mass of iron(III) hydroxide precipitate can...Ch. 4 - What mass of silver chloride can be prepared by...Ch. 4 - A 100.0-mL aliquot of 0.200 M aqueous potassium...Ch. 4 - A 1.42-g sample of a pure compound, with formula...Ch. 4 - You are given a 1.50-g mixture of sodium nitrate...Ch. 4 - Write the balanced formula, complete ionic, and...Ch. 4 - Write the balanced formula, complete ionic, and...Ch. 4 - Write the balanced formula equation for the...Ch. 4 - Prob. 74ECh. 4 - What volume of each of the following acids will...Ch. 4 - Prob. 76ECh. 4 - Hydrochloric acid (75.0 mL of 0.250 M) is added to...Ch. 4 - A student mixes four reagents together, thinking...Ch. 4 - A 25.00-mL sample of hydrochloric acid solution...Ch. 4 - A 10.00-mL sample of vinegar, an aqueous solution...Ch. 4 - What volume of 0.0200 M calcium hydroxide is...Ch. 4 - A 30.0-mL sample of an unknown strong base is...Ch. 4 - A student titrates an unknown amount of potassium...Ch. 4 - The concentration of a certain sodium hydroxide...Ch. 4 - Assign oxidation states for all atoms in each of...Ch. 4 - Assign the oxidation state for nitrogen in each of...Ch. 4 - Assign oxidatioo numbers to all the atoms in each...Ch. 4 - Specify which of the following are...Ch. 4 - Specify which of the following equations represent...Ch. 4 - Balance the following oxidation-reduction...Ch. 4 - Balance the following oxidation-reduction...Ch. 4 - Balance the following oxidation-reduction...Ch. 4 - Balance the following oxidation-reduction...Ch. 4 - Chlorine gas was first prepared in 1774 by C. W....Ch. 4 - Prob. 96ECh. 4 - The iron content of iron ore can be determined by...Ch. 4 - You wish to prepare 1 L of a 0.02-M potassium...Ch. 4 - The figures below are molecular-level...Ch. 4 - Prob. 103AECh. 4 - Prob. 104AECh. 4 - Many plants are poisonous because their stems and...Ch. 4 - Many over-the-counter antacid tablets are now...Ch. 4 - Using the general solubility rules given in Table...Ch. 4 - Consider a 1.50-g mixture of magnesium nitrate and...Ch. 4 - A 1.00-g sample of an alkaline earth metal...Ch. 4 - A mixture contains only NaCl and Al2(SO4)3. A...Ch. 4 - A mixture contains only NaCl and Fe(NO3)3. A...Ch. 4 - A student added 50.0 mL of an NaOH solution to...Ch. 4 - Some of the substances commonly used in stomach...Ch. 4 - Acetylsalicylic acid is the active ingredient in...Ch. 4 - When hydrochloric acid reacts with magnesium...Ch. 4 - A 2.20-g sample of an unknown acid (empirical...Ch. 4 - Carminic acid, a naturally occurring red pigment...Ch. 4 - Chlorisondamine chloride (C14H20Cl6N2) is a drug...Ch. 4 - Saccharin (C7H5NO3S) is sometimes dispensed in...Ch. 4 - Douglasite is a mineral with the formula 2KC1...Ch. 4 - Many oxidationreduction reactions can be balanced...Ch. 4 - Prob. 123AECh. 4 - Calculate the concentration of all ions present...Ch. 4 - A solution is prepared by dissolving 0.6706 g...Ch. 4 - For the following chemical reactions, determine...Ch. 4 - What volume of 0.100 M NaOH is required to...Ch. 4 - Prob. 128CWPCh. 4 - A 450.0-mL sample of a 0.257-M solution of silver...Ch. 4 - The zinc in a 1.343-g sample of a foot powder was...Ch. 4 - A 50.00-mL sample of aqueous Ca(OH)2 requires...Ch. 4 - When organic compounds containing sulfur are...Ch. 4 - Assign the oxidation state for the element Listed...Ch. 4 - A 10.00-g sample consisting of a mixture of sodium...Ch. 4 - The units of parts per million (ppm) and parts per...Ch. 4 - In the spectroscopic analysis of many substances,...Ch. 4 - In most of its ionic compounds, cobalt is either...Ch. 4 - Polychlorinated biphenyls (PCBs) have been used...Ch. 4 - Consider the reaction of 19.0 g of zinc with...Ch. 4 - A mixture contains only sodium chloride and...Ch. 4 - Prob. 141CPCh. 4 - Zinc and magnesium metal each react with...Ch. 4 - You made 100.0 mL of a lead(II) nitrate solution...Ch. 4 - Consider reacting copper(II) sulfate with iron....Ch. 4 - Consider an experiment in which two burets, Y and...Ch. 4 - Complete and balance each acid-base reaction. a....Ch. 4 - What volume of 0.0521 M Ba(OH)2 is required to...Ch. 4 - A 10.00-mL sample of sulfuric acid from an...Ch. 4 - A 0.500-L sample of H2SO4 solution was analyzed by...Ch. 4 - A 6.50-g sample of a diprotic acid requires 137.5...Ch. 4 - Citric acid, which can be obtained from lemon...Ch. 4 - Prob. 152CPCh. 4 - It took 25.06 0.05 mL of a sodium hydroxide...Ch. 4 - Triiodide ions are generated in solution by the...Ch. 4 - Chromium has been investigated as a coating for...Ch. 4 - Prob. 156IPCh. 4 - In a 1-L beaker, 203 mL of 0.307 M ammonium...Ch. 4 - The vanadium in a sample of ore is converted to...Ch. 4 - The unknown acid H2X can be neutralized completely...Ch. 4 - Three students were asked to find the identity of...Ch. 4 - You have two 500.0-mL aqueous solutions. Solution...
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
- What mass of solid NaOH (97.0% NaOH by mass) is required to prepare 1.00 L of a 10.0% solution of NaOH by mass? The density of the 10.0% solution is 1.109 g/mL.arrow_forwardYou take 1.00 g of an aspirin tablet (a compound consisting solely of carbon, hydrogen, and oxygen), burn it in air, and collect 2.20 g CO2 and 0.400 g H2O. You know that the molar mass of aspirin is between 170 and 190 g/mol. Reacting 1 mole of salicylic acid with I mole of acetic anhydride (C4H6O3) gives you 1 mole of aspirin and 1 mole of acetic acid (C2H4O2). Use this information to determine the molecular formula of salicylic acid.arrow_forwardA 2.00-L bottle of a solution of concentrated HCl was purchased for the general chemistry laboratory. The solution contained 868.8 g of HCl. What is the molarity of the solution?arrow_forward
- The carbon dioxide exhaled in the breath of astronauts is often removed from the spacecraft by reaction with lithium hydroxide 2LiOH(s)+CO2(g)Li2CO3(s)+H2O(l) Estimate the grams of lithium hydroxide required per astronaut per day. Assume that each astronaut requires 2.50 103 kcal of energy per day. Further assume that this energy can be equated to the heat of combustion of a quantity of glucose, C6H12O6, to CO2(g) and H2O(l). From the amount of glucose required to give 2.50 103 kcal of heat, calculate the amount of CO2 produced and hence the amount of LiOH required. The H for glucose(s) is 1273 kJ/mol.arrow_forward3.120 1f you have 32.6 g of sodium carbonate that is dissolved to give 2.10 L of solution, what is the molarity of the solution? What is the molarity of the sodium ions?arrow_forward4.69 The pictures below show a molecular-scale view of a chemical reaction between H2 and CO to produce methanol, CH3OH. The box on the left represents the reactants at the instant of mixing, and the box on the right shows what is left once the reaction has gone to completion. Was there a limiting reactant in this reaction? If so, what was it? Write a balanced chemical equation for this reaction. As usual, your equation should use the smallest possible whole number coefficients for all substances.arrow_forward
- Silicon is produced for the chemical and electronics industries by the following reactions. Give the balanced equation for each reaction. a. SiO2(s)+C(s)arefurnaceElectricSi(s)+CO(g) b. Liquid silicon tetrachloride is reacted with very pure solid magnesium, producing solid silicon and solid magnesium chloride. c. Na2SiF6(s) + Na(s) Si(s) + NaF(s)arrow_forwardThe molecular formula of acetylsalicylic acid (aspirin), one of the most commonly used pain relievers, is C9H8O4. a. Calculate the molar mass of aspirin. b. A typical aspirin tablet contains 500. mg C9H8O4. What amount (moles) of C9H8O4 molecules and what number of molecules of acetylsalicylic acid are in a 500.-mg tablet?arrow_forwardA soft drink contains an unknown mass of citric acid, C3H5O(COOH)3. It requires 6.42 mL of 9.580 × 10−2-M NaOH to neutralize the citric acid in 10.0 mL of the soft drink. C3H5O(COOH)3(aq) + 3 NaOH(aq) → Na3C3H5O(COO)3(aq) + 3 H2O(ℓ) Determine which step in these calculations for the mass of citric acid in 1 mL soft drink is incorrect? Why? n (NaOH) = (6.42 mL)(1L/1000 mL)(9.580 × 10−2 mol/L) n (citric acid) = (6.15 × 10−4 mol NaOH) × (3 mol citric acid/1 mol NaOH) m (citric acid in sample) = (1.85 × 10−3 mol citric acid) × (192.12 g/mol citric acid) m (citric acid in 1 mL soft drink) = (0.354 g citric acid)/(10 mL soft drink) Determine the correct result.arrow_forward
- What is the mass of fish, in kilograms, that one would have to consume to obtain a fatal dose of mercury, if the fish contains 30 parts per million of mercury by weight? (Assume that all the mercury from the fish ends up as mercury (II) chloride in the body and that a fatal dose is 0.20 g of HgCl2.) How many pounds of fish is this?arrow_forwardA student wants to prepare 1.00 L of a 1.00-M solution of NaOH (molar mass = 40.00 g/mol). If solid NaOH is available, how would the student prepare this solution? If 2.00 M NaOH is available, how would the student prepare the solution? To help ensure three significant figures in the NaOH molarity, to how many significant figures should the volumes and mass be determined?arrow_forwardThe space shuttle environmental control system handles excess CO2 (which the astronauts breathe out; it is 4.0% by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets to form lithium carbonate, Li2CO3, and water. If there are seven astronauts on board the shuttle, and each exhales 20. L of air pee minute, how long could clean air be generated if there were 25,000 g of LiOH pellets available for each shuttle mission? Assume the density of air is 0.0010 g/mL.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
Publisher:Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:OpenStax
Step by Step Stoichiometry Practice Problems | How to Pass ChemistryMole Conversions Made Easy: How to Convert Between Grams and Moles; Author: Ketzbook;https://www.youtube.com/watch?v=b2raanVWU6c;License: Standard YouTube License, CC-BY