All Matches
Solution Library
Expert Answer
Textbooks
Search Textbook questions, tutors and Books
Oops, something went wrong!
Change your search query and then try again
Toggle navigation
FREE Trial
S
Books
FREE
Tutors
Study Help
Expert Questions
Accounting
General Management
Mathematics
Finance
Organizational Behaviour
Law
Physics
Operating System
Management Leadership
Sociology
Programming
Marketing
Database
Computer Network
Economics
Textbooks Solutions
Accounting
Managerial Accounting
Management Leadership
Cost Accounting
Statistics
Business Law
Corporate Finance
Finance
Economics
Auditing
Ask a Question
Search
Search
Sign In
Register
study help
chemistry
organic chemistry
Questions and Answers of
Organic Chemistry
At a certain temperature and a total pressure of 1.2 atm, the partial pressures of an equilibrium mixtureare PA = 0.60 atm and PB = 0.60 atm. (a) Calculate the KP for the reaction at this
The decomposition of ammonium hydrogen sulfideis an endothermic process. A 6.1589-g sample of the solid is placed in an evacuated 4.000-L vessel at exactly 24°C. After equilibrium has been
Consider the reactionAt 430°C, an equilibrium mixture consists of 0.020 mole of O2, 0.040 mole of NO, and 0.96 mole of NO2. Calculate KP for the reaction, given that the total pressure is 0.20
When heated, ammonium carbamate decomposes as follows:At a certain temperature the equilibrium pressure of the system is 0.318 atm. Calculate KP for the reaction.
A mixture of 0.47 mole of H2 and 3.59 moles of HCl is heated to 2800°C. Calculate the equilibrium partial pressures of H2, Cl2, and HCl if the total pressure is 2.00 atm. For the reactionKP is
When heated at high temperatures, iodine vapor dissociates as follows:In one experiment, a chemist finds that when 0.054 mole of I2 was placed in a flask of volume 0.48 L at 587 K, the degree of
HA and HB are both weak acids although HB is the stronger of the two. Will it take a larger volume of a 0.10 M NaOH solution to neutralize 50.0 mL of 0.10 M HB than would be needed to neutralize 50.0
A solution contains a weak monoprotic acid HA and its sodium salt NaA both at 0.1 M concentration. Show that [OH2] = Kw/Ka.
Use the data in Table 15.3 to calculate the equilibrium constant for the following reaction: HCOOH(aq) + OH-(aq) → HCOO-(aq) + H2O(l)
Use the data in Table 15.3 to calculate the equilibrium constant for the following reaction: CH3COOH(aq) 1 NO-2(aq) → CH3COO2(aq) + HNO2(aq)
Most of the hydrides of Group 1A and Group 2A metals are ionic (the exceptions are BeH2 and MgH2, which are covalent compounds). (a) Describe the reaction between the hydride ion (H2) and water in
Calculate the pH of a 0.20 M ammonium acetate (CH3COONH4) solution.
Novocaine, used as a local anesthetic by dentists, is a weak base (Kb = 8.91 × 10-6). What is the ratio of the concentration of the base to that of its acid in the blood plasma (pH 5 7.40) of a
The ion product of D2O is 1.35 3 10215 at 25°C. (a) Calculate pD where pD = - log [D+].
Give an example of (a) A weak acid that contains oxygen atoms. (b) A weak acid that does not contain oxygen atoms. (c) A neutral molecule that acts as a Lewis acid. (d) A neutral molecule that acts
What is the pH of 250.0 mL of an aqueous solution containing 0.616 g of the strong acid trifluoromethane sulfonic acid (CF3SO3H)?
(a) Use VSEPR to predict the geometry of the hydronium ion, H3O1. (b) The O atom in H2O has two lone pairs and in principle can accept two H1 ions. Explain why the species H4O2+ does not exist. What
HF is a weak acid, but its strength increases with concentration. Explain. (F- reacts with HF to form HF2-. The equilibrium constant for this reaction is 5.2 at 25°C.)
When chlorine reacts with water, the resulting solution is weakly acidic and reacts with AgNO3 to give a white precipitate. Write balanced equations to represent these reactions. Explain why
When the concentration of a strong acid is not substantially higher than 1.0 × 10-7 M, the ionization of water must be taken into account in the calculation of the solution's pH. (a) Derive an
Calculate the pH of a 2.00 M NH4CN solution.
Calculate the concentrations of all species in a 0.100 M H3PO4 solution.
In the vapor phase, acetic acid molecules associate to a certain extent to form dimers: 2CH3COOH(g2 → (CH3COOH)2(g) At 51°C the pressure of a certain acetic acid vapor system is 0.0342 atm in a
Calculate the concentrations of all the species in a 0.100 M Na2CO3 solution.
Henry's law constant for CO2 at 38°C is 2.28 × 10-3 mol/L ? atm. Calculate the pH of a solution of CO2 at 38°C in equilibrium with the gas at a partial pressure of 3.20 atm.
Hydrocyanic acid (HCN) is a weak acid and a deadly poisonous compound-in the gaseous form (hydrogen cyanide) it is used in gas chambers. Why is it dangerous to treat sodium cyanide with acids (such
How many grams of NaCN would you need to dissolve in enough water to make exactly 250 mL of solution with a pH of 10.00?
A solution of formic acid (HCOOH) has a pH of 2.53. How many grams of formic acid are there in 100.0 mL of the solution?
Calculate the pH of a 1-L solution containing 0.150 mole of CH3COOH and 0.100 mole of HCl.
A 1.87-g sample of Mg reacts with 80.0 mL of a HCl solution whose pH is 20.544. What is the pH of the solution after all the Mg has reacted? Assume constant volume.
You are given two beakers, one containing an aqueous solution of strong acid (HA) and the other an aqueous solution of weak acid (HB) of the same concentration. Describe how you would compare the
Use Le Châtelier's principle to predict the effect of the following changes on the extent of hydrolysis of sodium nitrite (NaNO2) solution: (a) HCl is added, (b) NaOH is added, (c) NaCl is added,
Describe the hydration of SO2 as a Lewis acid-base reaction. (Refer to the discussion of the hydration of CO2 on p. 700.)
The disagreeable odor of fish is mainly due to organic compounds (RNH2) containing an amino group, -NH2, where R is the rest of the molecule. Amines are bases just like ammonia. Explain why putting
A solution of methylamine (CH3NH2) has a pH of 10.64. How many grams of methylamine are there in 100.0 mL of the solution?
A 0.400 M formic acid (HCOOH) solution freezes at 20.758°C. Calculate the Ka of the acid at that temperature. (Assume that molarity is equal to molality. Carry your calculations to three significant
Both the amide ion (NH2-) and the nitride ion (N3-) are stronger bases than the hydroxide ion and hence do not exist in aqueous solutions. (a) Write equations showing the reactions of these ions with
The atmospheric sulfur dioxide (SO2) concentration over a certain region is 0.12 ppm by volume. Calculate the pH of the rainwater due to this pollutant. Assume that the dissolution of SO2 does not
Calcium hypochlorite [Ca(OCl)2] is used as a disinfectant for swimming pools. When dissolved in water it produces hypochlorous acid Ca(OCl)2(s) + 2H2O(l) → 2HClO(aq) + Ca(OH)2(s) which ionizes as
Explain the action of smelling salt, which is ammonium carbonate [(NH4)2CO3]. (The thin film of aqueous solution that lines the nasal passage is slightly basic.)
About half of the hydrochloric acid produced annually in the United States (3.0 billion pounds) is used in metal pickling. This process involves the removal of metal oxide layers from metal surfaces
Which of the following does not represent a Lewis acid-base reaction? (a) H2O + H+ → H3O+ (b) NH3 + BF3 → H3NBF3 (c) PF3 + F2 → PF5 (d) Al(OH)3 + OH2 → Al(OH)4-
True or false? If false, explain why the statement is wrong. (a) All Lewis acids are Brønsted acids. (b) The conjugate base of an acid always carries a negative charge.
How many milliliters of a strong monoprotic acid solution at pH = 4.12 must be added to 528 mL of the same acid solution at pH = 5.76 to change its pH to 5.34? Assume that the volumes are additive.
Calculate the pH and percent ionization of a 0.80 M HNO2 solution.
Consider the two weak acids HX (molar mass = 180 g/mol) and HY (molar mass = 78.0 g/mol). If a solution of 16.9 g/L of HX has the same pH as one containing 9.05 g/L of HY, which is the stronger acid
Hemoglobin (Hb) is a blood protein that is responsible for transporting oxygen. It can exist in the protonated form as HbH+. The binding of oxygen can be represented by the simplifi ed equation HbH+
A 1.294-g sample of a metal carbonate (MCO3) is reacted with 500 mL of a 0.100 M HCl solution. The excess HCl acid is then neutralized by 32.80 mL of 0.588 M NaOH. Identify M.
Prove the statement that when the concentration of a weak acid HA decreases by a factor of 10, its percent ionization increases by a factor of √10. State any assumptions.
Calculate the pH of a solution that is 1.00 M HCN and 1.00 M HF. Compare the concentration (in molarity) of the CN2 ion in this solution with that in a 1.00 M HCN solution. Comment on the difference.
Teeth enamel is hydroxyapatite [Ca3(PO4)3OH]. When it dissolves in water (a process called demineralization), it dissociates as follows: Ca5(PO4)3OH → 5Ca2+ + 3PO43- + OH- The reverse process,
Use the van't Hoff equation (see Problem 14.113) and the data in Appendix 3 to calculate the pH of water at its normal boiling point.
Calculate the concentration of OH- ions in a 1.4 3 1023 M HCl solution.
Calculate the concentration of H+ ions in a 0.62 M NaOH solution.
Calculate the pH of each of the following solutions: (a) 0.0010 M HCl, (b) 0.76 M KOH.
Calculate the pH of each of the following solutions: (a) 2.8 x 10-4 M Ba(OH)2, (b) 5.2 x 10-4 M HNO3.
Calculate the hydrogen ion concentration in mol/L for solutions with the following pH values: (a) 2.42, (b) 11.21, (c) 6.96, (d) 15.00.
The pOH of a solution is 9.40. Calculate the hydrogen ion concentration of the solution.
Calculate the number of moles of KOH in 5.50 mL of a 0.360 M KOH solution. What is the pOH of the solution?
Write the formula for the conjugate acid of each of the following bases: (a) HS-, (b) HCO3-, (c) CO32-, (d) H2PO4-, (e) HPO42-, (f) PO43-, (g) HSO4-, (h) SO42-, (i) SO32-.
A solution is made by dissolving 18.4 g of HCl in 662 mL of water. Calculate the pH of the solution. (Assume that the volume remains constant.)
Classify each of the following species as a Brønsted acid or base, or both: (a) H2O, (b) OH2, (c) H3O1, (d) NH3, (e) NH41, (f) NH22, (g) NO32, (h) CO322, (i) HBr,
Which of the following diagrams best represents a strong acid, such as HCl, dissolved in water? Which represents a weak acid? Which represents a very weak acid? (The hydrated proton is shown as a
(1) Which of the following diagrams represents a solution of a weak diprotic acid? (2) Which diagrams represent chemically implausible situations?
Classify each of the following species as a weak or strong acid: (a) HNO3, (b) HF, (c) H2SO4, (d) HSO4-, (e) H2CO3, (f) HCO3-, (g) HCl, (h) HCN, (i) HNO2.
Classify each of the following species as a weak or strong base: (a) LiOH, (b) CN-, (c) H2O, (d) ClO4-, (e) NH2-.
Which of the following statements is/are true for a 0.10 M solution of a weak acid HA?
Which of the following statements is/are true regarding a 1.0 M solution of a strong acid HA? (a) [A-] > [H+] (b) The pH is 0.00. (c) [H+] = 1.0 M (d) [HA] = 1.0 M
Predict whether the following reaction will proceed from left to right to any measurable extent:
Write the formulas of the conjugate bases of the following acids: (a) HNO2, (b) H2SO4, (c) H2S, (d) HCN, (e) HCOOH (formic acid).
The Ka for benzoic acid is 6.5 3 10-5. Calculate the pH of a 0.10 M benzoic acid solution.
A 0.0560-g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution. Calculate the concentrations of H+, CH3COO-, and CH3COOH at equilibrium.
The pH of an acid solution is 6.20. Calculate the Ka for the acid. The initial acid concentration is 0.010 M.
What is the original molarity of a solution of formic acid (HCOOH) whose pH is 3.26 at equilibrium?
Calculate the percent ionization of benzoic acid having the following concentrations: (a) 0.20 M, (b) 0.00020 M.
Calculate the percent ionization of hydrofluoric acid at the following concentrations: (a) 0.60 M, (b) 0.0046 M, (c) 0.00028 M. Comment on the trends.
A 0.040 M solution of a monoprotic acid is 14 percent ionized. Calculate the ionization constant of the acid.
Identify the acid-base conjugate pairs in each of the following reactions:
(a) Calculate the percent ionization of a 0.20 M solution of the monoprotic acetylsalicylic acid (aspirin) for which Ka 5 3.0 3 10-4. (b) The pH of gastric juice in the stomach of a certain
Calculate the pH for each of the following solutions: (a) 0.10 M NH3, (b) 0.050 M C5H5N (pyridine).
The pH of a 0.30 M solution of a weak base is 10.66. What is the Kb of the base?
What is the original molarity of a solution of ammonia whose pH is 11.22?
In a 0.080 M NH3 solution, what percent of the NH3 is present as NH4+?
Write the formula for the conjugate acid of each of the following bases: (a) HS-, (b) HCO3-, (c) CO32-, (d) H2PO4, (e) HPO42-, (f) PO43-, (g) HSO4-, (h) SO42-, (i) SO32-.
The first and second ionization constants of a diprotic acid H2A are Ka1 and Ka2 at a certain temperature. Under what conditions will [A2-] = Ka2?
Compare the pH of a 0.040 M HCl solution with that of a 0.040 M H2SO4 solution.
What are the concentrations of HSO42, SO42-, and H+ in a 0.20 M KHSO4 solution?
Calculate the concentrations of H+, HCO32, and CO32- in a 0.025 M H2CO3 solution.
Predict the acid strengths of the following compounds: H2O, H2S, and H2Se.
Compare the strengths of the following pairs of acids: (a) H2SO4 and H2SeO4, (b) H3PO4 and H3AsO4.
Which of the following is the stronger acid: CH2ClCOOH or CHCl2COOH? Explain your choice.
Oxalic acid (H2C2O4) has the following structure:
Consider the following compounds:Experimentally, phenol is found to be a stronger acid than methanol. Explain this difference in terms of the structures of the conjugate bases.
Predict the pH (7 >, < 7, or ≈ 72 of aqueous solutions containing the following salts: (a) KBr, (b) Al(NO3)3, (c) BaCl2, (d) Bi(NO3)3.
Predict whether the following solutions are acidic, basic, or nearly neutral: (a) NaBr, (b) K2SO3, (c) NH4NO2, (d) Cr(NO3)3.
A certain salt, MX (containing the M+ and X- ions), is dissolved in water, and the pH of the resulting solution is 7.0. Can you say anything about the strengths of the acid and the base from which
In a certain experiment a student finds that the pHs of 0.10 M solutions of three potassium salts KX, KY, and KZ are 7.0, 9.0, and 11.0, respectively. Arrange the acids HX, HY, and HZ in the order
Calculate the pH of a 0.36 M CH3COONa solution.
Write the formula for the conjugate base of each of the following acids: (a) CH2ClCOOH, (b) HIO4, (c) H3PO4, (d) H2PO2-4, (e) HPO2-4 (f) H2SO4, (g) HSO4-, (h) HIO3, (i) HSO (j) NH4+, (k)
Calculate the pH of a 0.42 M NH4Cl solution.
Showing 12900 - 13000
of 15575
First
123
124
125
126
127
128
129
130
131
132
133
134
135
136
137
Last