New Semester Started Get 50% OFF Study Help! --h --m --s Claim Now

Question Answers

Textbooks

Find textbooks, questions and answers

Oops, something went wrong!

Change your search query and then try again

Result Not Found

Books FREE
Study Help
Tutors
AI Study Planner NEW
Sell Books

Search
Sign In
Register

study help
engineering
chemical engineering

Chemistry The Central Science 12th edition Theodore Brown, Eugene LeMay, Bruce Bursten, Catherine Murphy, Patrick Woodward - Solutions

The average pH of normal arterial blood is 7.40. At normal body temperature (37 (C), Kw = 2.4 ( 10-14. Calculate [H+], [OH-], and pOH for blood at this temperature.
In which of the following cases is the approximation that the equilibrium concentration of H+ (aq) is small relative to the initial concentration of HA likely to be most valid: (a) Initial [HA] = 0.100 M and Ka = 1.0 ( 10-6, (b) Initial [HA] = 0.100 M and Ka = 1.0 ( 10-4, (c) Initial [HA] = 1.00 M
Carbon dioxide in the atmosphere dissolves in raindrops to produce carbonic acid (H2CO3), causing the pH of clean, unpolluted rain to range from about 5.2 to 5.6. What are the ranges of [H+] and [OH-] in the raindrops?
(a) What is a strong acid?
(a) What is a strong base?
Calculate the pH of each of the following strong acid solutions: (a) 8.5 ( 10-3 M HBr, (b) 1.52 g of HNO3 in 575 mL of solution, (c) 5.00 mL of 0.250 M HClO4 diluted to 50.0 mL, (d) A solution formed by mixing 10.0 mL of 0.100 MHBr with 20.0 mL of 0.200 M HCl.
Calculate the pH of each of the following strong acid solutions: (a) 0.0167 M HNO3, (b) 0.225 g of HClO3 in 2.00 L of solution, (c) 15.00 mL of 1.00 M HCl diluted to 0.500 L, (d) A mixture formed by adding 50.0 mL of 0.020 MHCl to 125 mL of 0.010 M HI.
Calculate [OH-] and pH for (a) 1.5 ( 10-3 M Sr(OH2),
Calculate [OH-] and pH for each of the following strong base solutions:(a) 0.182MKOH,(b) 3.165 g of KOH in 500.0 mL of solution,(c) 10.0 mL of 0.0105 MCa(OH)2 diluted to 500.0 mL,(d) A solution formed by mixing 20.0 mL of 0.015 M Ba(OH)2 with 40.0 mL of 8.2 ( 10-3 M NaOH.
Calculate the concentration of an aqueous solution of NaOH that has a pH of 11.50.
Calculate the concentration of an aqueous solution of Ca(OH)2 that has a pH of 10.05.
Write the chemical equation and the Ka expression for the ionization of each of the following acids in aqueous solution. First show the reaction with H+(aq) as a product and then with the hydronium ion:(a) HBrO2,(b) C2H5COOH.
The indicator methyl orange has been added to both of these solutions. Based on the colors, classify each statement as true or false: (a) The pH of solution A is definitely less than 7.00. (b) The pH of solution B is definitely greater than 7.00. (c) The pH of solution B is greater than that of
Write the chemical equation and the Ka expression for the acid dissociation of each of the following acids in aqueous solution. First show the reaction with H+(aq) as a product and then with the hydronium ion:(a) C6H5COOH,(b) HCO3-.
Lactic acid (CH3CH(OH)COOH) has one acidic hydrogen. A 0.10 M solution of lactic acid has a pH of 2.44. Calculate Ka.
Phenylacetic acid (C6H5CH2COOH) is one of the substances that accumulates in the blood of people with phenylketonuria, an inherited disorder that can cause mental retardation or even death. A 0.085 M solution of C6H5CH2COOH has a pH of 2.68. Calculate the Ka value for this acid.
A 0.100 Msolution of chloroacetic acid (ClCH2COOH) is 11.0% ionized.Using this information, calculate [ClCH2COO-], [H+], [ClCH2COOH], and Ka for chloroacetic acid.
A 0.100 Msolution of bromoacetic acid (BrCH2COOH) is 13.2% ionized. Calculate [H+], [BrCH2COOH] and Ka for bromoacetic acid.
A particular sample of vinegar has a pH of 2.90. If acetic acid is the only acid that vinegar contains (Ka = 1.8 ( 10-5), calculate the concentration of acetic acid in the vinegar.
If a solution of HF (Ka = 6.8 ( 10-4) has a pH of 3.65, calculate the concentration of hydrofluoric acid.
The acid-dissociation constant for benzoic acid (C6H5COOH) is 6.3 ( 10-5. Calculate the equilibrium concentrations of H3O+, C6H5COOH in the solution if the initial concentration of C6H5COOH is 0.050 M.
The acid-dissociation constant for chlorous acid (HClO2) is 1.1 ( 10-2. Calculate the concentrations of H3O+, ClO2-, and HClO2 at equilibrium if the initial concentration of HClO2 is 0.0125 M.
Calculate the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (a) 0.095 M propionic acid (C2H5COOH), (b) 0.100 M hydrogen chromate ion (HCrO4-, (c) 0.120 M pyridine (C5H5N).
(a) Which of these three lines represents the effect of concentration on the percent ionization of a weak acid?(b) Explain in qualitative terms why the curve you chose has the shape it does.
Determine the pH of each of the following solutions (Ka and Kb values are given in Appendix D): (a) 0.095Mhypochlorous acid, (b) 0.0085 M hydrazine, (c) 0.165 M hydroxylamine.
Saccharin, a sugar substitute, is a weak acid with pKa = 2.32 at 25 (C. It ionizes in aqueous solution as follows: HNC7H4SO3(aq) H+(aq) + NC7H4SO3 -(aq) What is the pH of a 0.10 M solution of this substance?
The active ingredient in aspirin is acetylsalicylic acid (HC9H7O4), a monoprotic acid with Ka = 3.3 ( 10-4 at 25 (C. What is the pH of a solution obtained by dissolving two extra-strength aspirin tablets, containing 500 mg of acetylsalicylic acid each, in 250 mL of water?
Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations (Ka is given in Appendix D): (a) 0.400 M, (b) 0.100 M, (c) 0.0400 M.
Calculate the percent ionization of propionic acid (C2H5COOH) in solutions of each of the following concentrations (Ka is given in Appendix D):(a) 0.250 M,(b) 0.0800 M,(c) 0.0200 M.
Show that for a weak acid, the percent ionization should vary as the inverse square root of the acid concentration.
For solutions of a weak acid, a graph of pH versus the logarithm of the initial acid concentration should be a straight line. What is the magnitude of the slope of that line?
Citric acid, which is present in citrus fruits, is a triprotic acid (Table 16.3). Calculate the pH of a 0.040 M solution of citric acid. Explain any approximations or assumptions you make in your calculations. Is the concentration of citrate ion (C6H5O7)3- equal to, less than, or greater than the
Tartaric acid is found in many fruits, including grapes, and is partially responsible for the dry texture of certain wines. Calculate the pH and the tartarate ion (C4H4O62-) concentration for a 0.250 M solution of tartaric acid, for which the aciddissociation constants are listed in Table 16.3.
Consider the base hydroxylamine, NH2OH. (a) What is the conjugate acid of hydroxylamine? (b) When it acts as a base, which atom in hydroxylamine accepts a proton? (c) There are two atoms in hydroxylamine that have nonbonding electron pairs that could act as proton acceptors. Use Lewis structures
Each of the three molecules shown here contains an OH group, but one molecule acts as a base, one as an acid, and the third is neither acid nor base.(a) Which one acts as a base? Why does only this molecule act as a base?(b)Which one acts as an acid?(c) Why is the remaining molecule neither acidic
The hypochlorite ion, ClO-, acts as a weak base. (a) Is ClO- a stronger or weaker base than hydroxylamine? (b) When ClO- acts as a base, which atom, Cl or O, acts as the proton acceptor? (c) Can you use formal charges to rationalize your answer to part (b)?
Write the chemical equation and the Kb expression for the reaction of each of the following bases with water: (a) Dimethylamine, (CH3)2NH; (b) Carbonate ion, CO32-; (c) Formate ion, CHO2-.
Write the chemical equation and the Kb expression for the reaction of each of the following bases with water: (a) Propylamine, C3H7NH2; (b) Monohydrogen phosphate ion, HPO42-; (c) Benzoate ion, C6H5CO2-.
Calculate the molar concentration of OH- ions in a 0.075 M solution of ethylamine (C2H5NH2; Kb = 6.4 ( 10-4). Calculate the pH of this solution.
Calculate the molar concentration of OH- ions in a 0.724 M solution of hypobromite ion (BrO-; Kb = 4.0 ( 10-6). What is the pH of this solution?
Ephedrine, a central nervous system stimulant, is used in nasal sprays as a decongestant. This compound is a weak organic base:
Codeine (C18H21NO3) is a weak organic base. A 5.0 ( 10-3 M solution of codeine has a pH of 9.95. Calculate the value of Kb for this substance.What is the pKb for this base?
Although the acid-dissociation constant for phenol (C6H5OH) is listed in Appendix D, the base-dissociation constant for the phenolate ion (C6H5O-) is not. (a) Explain why it is not necessary to list both Ka for phenol and Kb for the phenolate ion. (b) Calculate Kb for the phenolate ion. (c) Is the
Use the acid-dissociation constants in Table 16.3 to arrange these oxyanions from strongest base to weakest: SO42-, CO32-, SO32-, and PO43-.
(a) Given that Ka for acetic acid is 1.8 ( 10-5 and that for hypochlorous acid is 3.0 ( 10-8, which is the stronger acid? (b)Which is the stronger base, the acetate ion or the hypochlorite ion? (c) Calculate Kb values for CH3COO- and ClO-.
Which of the following diagrams best represents an aqueous solution of NaF? The water molecules are not shown for clarity. Will this solution be acidic, neutral, or basic?
(a) Given that Kb for ammonia is 1.8 ( 10-5 and that for hydroxylamine is 1.1 ( 10-8, which is the stronger base? (b) Which is the stronger acid, the ammonium ion or the hydroxylammonium ion? (c) Calculate Ka values for NH4+ and H3NOH+.
Using data from Appendix D, calculate [OH-] and pH for each of the following solutions: (a) 0.10MNaBrO,(b) 0.080MNaHS,(c) A mixture that is 0.10 Min NaNO2 and 0.20 M in Ca(NO2)2.
Using data from Appendix D, calculate [OH-] and pH for each of the following solutions: (a) 0.105 M NaF,(b) 0.035 M Na2S,(c) A mixture that is 0.045 Min CH3COONa and 0.055 M in (CH3COO)2Ba.
Predict whether aqueous solutions of the following compounds are acidic, basic, or neutral: (a) NH4Br, (b) FeCl3, (c) Na2CO3, (d) KClO4, (e) NaHC2O4.
Predict whether aqueous solutions of the following substances are acidic, basic, or neutral: (a) AlCl3, (b) NaBr, (c) NaClO, (d) [CH3NH3] NO3, (e) Na2SO3.
An unknown salt is either NaF,NaCl, or NaOCl. When 0.050 mol of the salt is dissolved in water to form 0.500 L of solution, the pH of the solution is 8.08.What is the identity of the salt?
An unknown salt is either KBr, NH4Cl, KCN, or K2CO3. If a 0.100 M solution of the salt is neutral, what is the identity of the salt?
How does the acid strength of an oxyacid depend on (a) The electronegativity of the central atom; (b) The number of nonprotonated oxygen atoms in the molecule?
(a) Why is NH3 a stronger base than H2O? (b) Why is NH3 a stronger base than CH4?
Explain the following observations: (a) HNO3 is a stronger acid than HNO2; (b) H2S is a stronger acid than H2O; (c) H2SO4 is a stronger acid than HSO4-; (d) H2SO4 is a stronger acid than H2SeO4; (e) CCl3COOH is a stronger acid than CH3COOH.
Consider the molecular models shown here, where X represents a halogen atom.(a) If X is the same atom in both molecules, which one will be more acidic?(b) Does the acidity of each molecule increase or decrease as the electronegativity of the atom X increases?(a)(b)
Explain the following observations: (a) HCl is a stronger acid than H2S; (b) H3PO4 is a stronger acid than H3AsO4; (c) HBrO3 is a stronger acid than HBrO2; (d) H2C2O4 is a stronger acid than HC2O4-; (e) benzoic acid (C6H5COOH) is a stronger acid than phenol (C6H5OH).
Based on their compositions and structures and on conjugate acid-base relationships, select the stronger base in each of the following pairs: (a) BrO- or ClO-, (b) BrO- or BrO2-, (c) HPO42- or H2PO4-.
Based on their compositions and structures and on conjugate acid-base relationships, select the stronger base in each of the following pairs:(a) NO3- or NO2-,(b) PO43- or AsO43-,(c) HCO3- or CO32-.
Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) In general, the acidity of binary acids increases from left to right in a given row of the periodic table. (b) In a series of acids that have the same
Indicate whether each of the following statements is true or false. For each statement that is false, correct the statement to make it true. (a) Acid strength in a series of H-X molecules increases with increasing size of X. (b) For acids of the same general structure but differing
If a substance is an Arrhenius base, is it necessarily a Brønsted- Lowry base? Is it necessarily a Lewis base? Explain.
If a substance is a Lewis acid, is it necessarily a Brønsted-Lowry acid? Is it necessarily an Arrhenius acid? Explain.
Identify the Lewis acid and Lewis base among the reactants in each of the following reactions:(lq denotes liquid ammonia as solvent)
Identify the Lewis acid and Lewis base in each of the following reactions:
Predict which member of each pair produces the more acidic aqueous solution: (a) K+ or Cu2+, (b) Fe2+ or Fe3+, (c) Al3+ or Ga3+. Explain.
The following boxes represent aqueous solutions containing a weak acid, HX, and its conjugate base, X-. Water molecules, hydronium ions and cations are not shown. Which solution has the highest pH? Explain. [Section 17.1]
Ca(OH)2 has a Ksp of 6.5 X 10-6(a) If 0.370 g of Ca(OH)2 is added to 500 mL of water and the mixture is allowed to come to equilibrium,will the solution be saturated?(b) If 50 mL of the solution from part (a) is added to each of the beakers shown here, in which beakers, if any,will a precipitate
Three cations, Ni2+,Cu2+, and Ag +, are separated using two different precipitating agents. Based on Figure 17.23, what two precipitating agents could be used? Using these agents, indicate which of the cations is A, which is B, and which is C. [Section 17.7]
(a) What is the common-ion effect?
(a) Consider the equilibrium B(aq) + H2O. HB+ (aq) + OH- (aq). Using Le ChÃ¢telier's principle, explain the effect of the presence of a salt of on the ionization of B.(b) Give an example of a salt that can decrease the ionization of NH3 in solution.
Use information from Appendix D to calculate the pH of(a) A solution that is 0.060 M in potassium propionate (C2H5COOK or KC3H5O2) and 0.085 M in propionic acid (C2H5COOH or HC3H5O2);(b) A solution that is 0.075 M in trimethylamine, (CH3)3N, and 0.10 M in trimethylammonium chloride, (CH3)3NHCl;(c)
(a) Calculate the percent ionization of 0.0075 Mbutanoic acid (ka = 1.5 x 10. (b) Calculate the percent ionization of 0.0075 M butanoic acid in a solution containing 0.085 M sodium butanoate.
(a) Calculate the percent ionization of 0.125 M lactic acid (ka = 1.4 x 10-4).
Explain why a mixture of CH3COOH and CH3COONa can act as a buffer while a mixture of HCl and NaCl cannot.
The beaker on the right contains 0.1 M acetic acid solution with methyl orange as an indicator. The beaker on the left contains a mixture of 0.1 M acetic acid and 0.1 M sodium acetate with methyl orange. (a) Using Figure 16.7, what can you say about the pH of each solution? (b) Which solution is
Explain why a mixture formed by mixing 100 mL of 0.100 M CH3COOH and 50 mL of 0.100 M NaOH will act as a buffer.
(a) Calculate the pH of a buffer that is 0.12 M in lactic acid and 0.11 M in sodium lactate. (b) Calculate the pH of a buffer formed by mixing 85 mL of 0.13 M lactic acid with 95 mL of 0.15 M sodium lactate.
(a) Calculate the pH of a buffer that is 0.105 M in NaHCO3 and 0.125 M in Na2CO3.
A buffer is prepared by adding 20.0 g of sodium acetate (CH3COONa) to 500 mL of a 0.150 Macetic acid (CH3COOH) solution. (a) Determine the pH of the buffer. (b) Write the complete ionic equation for the reaction that occurs when a few drops of hydrochloric acid are added to the buffer. (c) Write
A buffer is prepared by adding 10.0 g of ammonium chloride (NH4Cl) to 250 mL of 1.00 M NH3 solution. (a) What is the pH of this buffer? (b) Write the complete ionic equation for the reaction that occurs when a few drops of nitric acid are added to the buffer. (c) Write the complete ionic equation
You are asked to prepare a pH = 3.00 buffer solution starting from 1.25 L of a 1.00 M solution of hydrofluoric acid (HF) and an excess of sodium fluoride (NaF). (a) What is the pH of the hydrofluoric acid solution prior to adding sodium fluoride? (b) How many grams of sodium fluoride should be
You are asked to prepare a pH = 4.00 buffer starting from 1.50 L of 0.0200 M solution of benzoic acid (C6H5COOH) and an excess of sodium benzoate (C6H5COONa). (a)What is the pH of the benzoic acid solution prior to adding sodium benzoate? (b) How many grams of sodium benzoate should be added to
A buffer contains 0.10 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. (a) What is the pH of this buffer? (b) What is the pH of the buffer after the addition of 0.02 mol of KOH? (c) What is the pH of the buffer after the addition of 0.02 mol of HNO3?
A buffer contains 0.15 mol of propionic acid (C2H5COOH) and 0.10 mol of sodium propionate (C2H5COONa) in 1.20 L. (a) What is the pH of this buffer? (b) What is the pH of the buffer after the addition of 0.01 mol of NaOH? (c) What is the pH of the buffer after the addition of 0.01 mol of HI?
(a) What is the ratio of HCO3 - to H2CO3 in blood of pH 7.4? (b) What is the ratio of HCO3- to H2CO3 in an exhausted marathon runner whose blood pH is 7.1?
A buffer contains a weak acid, HX, and its conjugate base. The weak acid has pka of 4.5, and the buffer has a pH of 4.3. Without doing a calculation, predict whether [HX] = [X-], [HX] > [X-], or [HX] < [X-]. Explain. [Section17.2]
A buffer, consisting of H2PO4- and HPO42-, helps control the pH of physiological fluids. Many carbonated soft drinks also use this buffer system. What is the pH of a soft drink in which the major buffer ingredients are 6.5 g of NaH2PO4 and 8.0 g of Na2HPO4 per 355 mL of solution?
You have to prepare a pH 3.50 buffer, and you have the following 0.10 M solutions available: HCOOH, CH3COOH, H3PO4, HCOONa, CH3COONa, and NaH2PO4. Which solutions would you use? How many milliliters of each solution would you use to make approximately a liter of the buffer?
You have to prepare a pH 5.00 buffer, and you have the following 0.10 M solutions available: HCOOH, HCOONa, CH3COOH, CH3COONa, HCN,and NaCN.Which solutions would you use? How many milliliters of each solution would you use to make approximately a liter of the buffer?
The accompanying graph shows the titration curves for two monoprotic acids.(a)Which curve is that of a strong acid?(b) What is the approximate pH at the equivalence point of each titration?(c) 40.0 mL of each acid was titrated with 0.100 M base.Which acid is more concentrated?
How does titration of a strong,monoprotic acid with a strong base differ from titration of a weak, monoprotic acid with a strong base with respect to the following: (a) Quantity of base required to reach the equivalence point, (b) Ph at the beginning of the titration, (c) Ph at the equivalence
The samples of nitric and acetic acid shown here are both titrated with a 0.100 M solution of NaOH(aq). Determine whether each of the following statements concerning these titrations is true or false. (a) A larger volume of NaOH(aq) is needed to reach the equivalence point in the titration of
Determine whether each of the following statements concerning the titrations in Problem 17.35 is true or false. (a) The pH at the beginning of the two titrations will be the same. (b) The titration curves will both be essentially the same after passing the equivalence point. (c) Methyl red would be
Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (a) NaHCO3 titrated with NaOH, (b) NH3 titrated with HCl, (c) KOH titrated with HBr.
Predict whether the equivalence point of each of the following titrations is below, above, or at pH7: (a) Formic acid titrated with NaOH, (b) Calcium hydroxide titrated with perchloric acid, (c) Pyridine titrated with nitric acid.
As shown in Figure 16.7, the indicator thymol blue has two color changes.Which color change will generally be more suitable for titration of a weak acid with a strong base?
The drawing on the left represents a buffer composed of equal concentrations of a weak acid, HX, and its conjugate base, X-. The heights of the columns are proportional to the concentrations of the components of the buffer.(a) Which of the three drawings, (1), (2), or (3), represents the buffer
Assume that 30.0 mL of a 0.10 M solution of a weak base B that accepts one proton is titrated with a 0.10 M solution of the monoprotic strong acid HX. (a) How many moles of HX have been added at the equivalence point? (b)What is the predominant form of B at the equivalence point? (c)What factor

Showing 4100 - 4200 of 6778

First
35
36
37
38
39
40
41
42
43
44
45
46
47
48
49
Last

Step by Step Answers

Services

Sitemap
Fun
Definitions
Become Tutor
Used Textbooks
Study Help Categories
Recent Questions
Expert Questions
Campus Wear
Sell Your Books

Company Info

Security
Copyrights
Privacy Policy
Terms & Conditions
SolutionInn Fee
Scholarship
Online Quiz
Give Feedback, Get Rewards

Get In Touch

About Us
Contact Us
Career
Jobs
FAQ
Student Discount
Campus Ambassador

Secure Payment

Download Our App

© 2026 SolutionInn. All Rights Reserved