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Questions and Answers of General Chemistry Principles

A 625 mL sample of an aqueous solution containing 0.275 mol propionic acid, CH3CH2CO2H, has [H3O+] = 0.00239 M. What is the value of Ka for propionic acid? CH3CH₂CO₂H + H₂0 H3O+ +
Fluoroacetic acid occurs in gifblaar, one of the most poisonous of all plants. A 0.318 M solution of the acid is found to have a pH = 1.56. Calculate Ka of fluoroacetic acid. CH₂FCOOH(aq) + H₂O
Caproic acid, HC6H11O2, found in small amounts in coconut and palm oils, is used in making artificial flavors. A saturated aqueous solution of the acid contains 11 g/L and has pH = 2.94. Calculate Ka
What mass of benzoic acid, C6H5COOH, would you dissolve in 350.0 mL of water to produce a solution with a pH = 2.85? C6H5COOH + H₂O = H₂0+ + C₂H₂COO™ Ka = 6.3 x 10-5
What must be the molarity of an aqueous solution of trimethylamine, (CH3)3N, if it has a pH = 11.12? (CH3)3 + H2O — (CH3)3NH' + OH Кь = 6.3 × 10-5
What are [H3O+], [OH-], pH, and pOH of 0.55 M M HClO2?
The solubility of 1-naphthylamine, C10H7NH2, a substance used in the manufacture of dyes, is given in a handbook as 1 g per 590 g H2O. What is the approximate pH of a saturated aqueous solution of
What are [H3O+], [OH-], pH, and pOH of 0.386 M CH3NH2?
A saturated aqueous solution of o–nitrophenol, HOC6H4NO2, has pH = 4.53. What is the solubility of o-nitrophenol in water, in grams per liter? HOC6H4NO₂ + H₂O = H3O+ H3O+ + OC6H4NO₂ pKa = 7.23
A particular vinegar is found to contain 5.7% acetic acid, CH3COOH, by mass. What mass of this vinegar should be diluted with water to produce 0.750 L of a solution with pH = 4.52?
A particular household ammonia solution (d = 0.97 g/mL) is 6.8% NH3 by mass. How many milliliters of this solution should be diluted with water to produce 625 mL of a solution with pH = 11.55?
A 275 mL sample of vapor in equilibrium with propan-1-amine at 25.0 °C is removed and dissolved in 0.500 L H2O. For propan-1-amine, pKb = 3.43 and v.p. = 316 Torr.(a) What should be the pH of the
In the diagram below, the sketch on the far left represents the [H3O+] present in an acetic acid solution of molarity c. If the molarity of the solution is doubled, which of the sketches below best
One handbook lists a value of 9.5 for pKb of quinoline, C9H7N, a weak base used as a preservative for anatomical specimens and to make dyes. Another handbook lists the solubility of quinoline in
In the diagram below, the sketch on the far left represents the [OH-] present in an ammonia solution of molarity c. If the solution is diluted to half its original molarity, which of the sketches
What is the (a) Degree of ionization and (b) Percent ionization of propionic acid in a solution that is 0.45 M CH3CH2CO2H? CH3CH₂CO₂H + H₂O — H3O+ + CH3CH₂CO₂ pka = 4.89
What is the (a) Degree of ionization and (b) Percent ionization of ethylamine, C2H5NH2, in a 0.85 M aqueous solution?
What must be the molarity of an aqueous solution of NH3 if it is 4.2% ionized?
What must be the molarity of an acetic acid solution if it has the same percent ionization as 0.100 M CH3CH2CO2H (propionic acid, Ka = 1.3 x 10-5)?
What is the (a) Degree of ionization and (b) Percent ionization of trichloroacetic acid in a 0.035 M CCl3COOH solution? CC13COOH + H₂0 ⇒ H3O+ + CCl₂COO pka 0.52 =
Continuing the dilutions described in Example 16-4, should we expect the percent ionization to be 13% in 0.0010 M CH3COOH and 42% in 0.00010 M CH3COOH? Explain.Example 16-4What is the percent
For 0.045 M H2CO3, a weak diprotic acid, calculate (a) [H3O+], (b) [HCO3-],(c) [CO32-]. Use data from Table 16.5 as necessary.Table 16.5 TABLE 16.5 lonization Constants of Some Polyprotic
Explain why [PO43-] in 1.00 M H3PO4 is not simply 1/3 [H3O+], but much, much less than 1/3 [H3O+].
Cola drinks have a phosphoric acid content that is described as “from 0.057 to 0.084% of 75% phosphoric acid, by mass.” Estimate the pH range of cola drinks corresponding to this range of H3PO4
Determine [H3O+], [HS-], and [S2-] for the following H2S(aq) solutions: (a) 0.075 M H2S; (b) 0.0050 M H2S;(c) 1.0 x 10-5 M H2S.
Calculate [H3O+], [HSO4-], and [SO42-] in (a) 0.75 M H2SO4;(b) 0.075 M H2SO4; (c) 7.5 x 10-4 M H2SO4.
Adipic acid, HOOC(CH2)4COOH, is among the top 50 manufactured chemicals in the United States (nearly 1 million metric tons annually). Its chief use is in the manufacture of nylon. It is a diprotic
The antimalarial drug quinine, C20H24O2N2, is a diprotic base with a water solubility of 1.00 g/1900 mL of solution.(a) Write equations for the ionization equilibria corresponding to pKb1 = 6.0 and
From data in Table 16.4, determine (a) Ka for C5H5NH+;(b) Kb for HCOO-; (c) Kb for C6H5O-.Table 16.4 TABLE 16.4 lonization Constants of Some Weak Acids and Weak Bases in Water at 25
Codeine, C18H21O3N, is an opiate, has analgesic and antidiarrheal properties, and is widely used. In water, codeine is a weak base. A handbook gives pKa = 6.05 for protonated codeine, C18H21O3NH+.
For hydrazine, N2H4, pKb1 = 6.07 and pKb2 = 15.05. Draw a structural formula for hydrazine, and write equations to show the ionization of hydrazine in two distinctive steps. Calculate the pH of 0.245
Approximately 4 metric tons of quinoline, C9H7N, is produced annually. The principal source of quinoline is coal tar. Quinoline is a weak base in water. A handbook gives Ka = 6.3 x 10-10 for
Predict whether a solution of each of the following salts is acidic, basic, or pH neutral: (a) KCl; (b) KF;(c) NaNO3;(d) Ca(OCl)2;(e) NH4NO2.
Arrange the following 0.010 M solutions in order of increasing pH: NH3(aq), HNO3(aq), NaNO2(aq), CH3COOH(aq), NaOH(aq), NH4CH3COO(aq), NH4ClO4(aq).
What is the pH of an aqueous solution that is 0.089 M NaOCl?
For each of the following ions, write two equations—one showing its ionization as an acid and the other as a base: (a) HSO3-; (b) HS-; (c) HPO4-. Then use data from Table 16.5 to predict
What is the pH of an aqueous solution that is 0.123 M NH4Cl?
Sorbic acid, CH2CH = CH = CHCH2CO2H (pKa = 4.77), is widely used in the food industry as a preservative. For example, its potassium salt (potassium sorbate) is added to cheese to inhibit the
Pyridine, C5H5N (pKb = 8.82), forms a salt, pyridinium chloride, as a result of a reaction with HCl. Write an ionic equation to represent the hydrolysis of the pyridinium ion, and calculate the pH of
Suppose you wanted to produce an aqueous solution of pH = 8.65 by dissolving one of the following salts in water. Which salt would you use, and at what molarity?(a) NH4Cl; (b) KHSO4; (c) KNO2; (d)
Predict which is the stronger acid: (a) HClO2 or HClO3;(b) H2CO3 or HNO2; (c) H2SiO3 or H3PO4.Explain.
Explain why trichloroacetic acid, CCl3COOH, is a stronger acid than acetic acid, CH3COOH.
Which is the stronger acid of each of the following pairs of acids? Explain your reasoning. (a) HBr or HI;(b) HOClO or HOBr; (c) I3CCH2CH2COOH or CH3CH2CCl2COOH.
From the following bases, select the one with the smallest Kb and the one with the largest Kb, and give reasons for your choices. (a) -NH₂ (b) H₂C- Cl (c) CH3CH₂CH₂NH₂ -NH₂ (d)
Indicate which of the following is the weakest acid, and give reasons for your choice: HBr; CH2ClCOOH; CH3CH2COOH; CH2FCH2COOH; CI3COOH.
For the molecular models shown, write the formula of the species that is the most acidic and the one that is most basic, and give reasons for your choices. (a) (b) (c) (d)
For each reaction draw a Lewis structure for each species and indicate which is the acid and which is the base: (a) CO₂ + H₂O H₂CO3 H₂OBF3 (b) H₂O + BF3 (c) 0² + H₂O →→ 2OH- (d) S²
In the following reactions indicate which is the Lewis acid and which is the Lewis base: (a) SOI2 + BaSO3 (b) HgCl3 + CI¯ - 2+ Ba²+ + 21 +2SO₂ HgC14²-
Indicate whether each of the following is a Lewis acid or base. (a) OH-; (b) (C2H5)3B; (c) CH3NH2.
Each of the following is a Lewis acid–base reaction. Which reactant is the acid, and which is the base? Explain. (a) SO3 + H₂O → H₂SO4 (b) Zn(OH)₂(s) + 2OH(aq) [Zn(OH)4]² (aq)
The three following reactions are acid–base reactions according to the Lewis theory. Draw Lewis structures, and identify the Lewis acid and Lewis base in each reaction. (a) B(OH)3 + OH™ (b)
CO2(g) can be removed from confined quarters (such as a spacecraft) by allowing it to react with an alkali metal hydroxide. Show that this is a Lewis acid–base reaction. For example, CO₂(g) +
The following very strong acids are formed by the reactions indicated:(a) Identify the Lewis acids and bases.(b) To which atom is the H atom bonded in each acid? HF + SbF5- (called "super
The molecular solid I2(s) is only slightly soluble in water but will dissolve to a much greater extent in an aqueous solution of KI, because the I3- anion forms. Write an equation for the formation
Use Lewis structures to diagram the following reaction in the manner.Identify the Lewis acid and Lewis base. H₂O + SO₂ - H₂SO3
Use Lewis structures to diagram the following reaction in the manner.Identify the Lewis acid and Lewis base. 2 NH3 + Ag [Ag(NH3)2]*
The Brønsted–Lowry theory can be applied to acid–base reactions in nonaqueous solvents, where the relative strengths of acids and bases can differ from what they are in aqueous solutions.
Use data from Appendix D to determine whether the ion product of water, Kw, increases, decreases, or remains unchanged with increasing temperature. TABLE D.1 Ground-State Electron
Several approximate pH values are marked on the following pH scale.Some of the following solutions can be matched to one of the approximate pH values marked on the scale; others cannot. For solutions
The pH of saturated Sr(OH)2(aq) is found to be 13.12. A10.0 mL sample of saturated Sr(OH)2(aq) is diluted to 250.0 mL in a volumetric flask. A10.0 mL sample of the diluted Sr(OH)2(aq) is transferred
Show that when [H3O+] is reduced to half its original value, the pH of a solution increases by 0.30 unit, regardless of the initial pH. Is it also true that when any solution is diluted to half its
Explain why [H3O+] in a strong acid solution doubles as the total acid concentration doubles, whereas in a weak acid solution, [H3O+] increases only by about a factor of √2.
From the observation that 0.0500 M vinylacetic acid has a freezing point of -0.096 °C, determine Ka for this acid. CH2=CHCH,CO,H+H,O
You are asked to prepare a 100.0 mL sample of a solution with a pH of 5.50 by dissolving the appropriate amount of a solute in water with pH = 7.00. Which of these solutes would you use, and in what
Oxalic acid, HOOCCOOH, a weak diprotic acid, has pKa1 = 1.25 and pKa2 = 3.81. A related diprotic acid, suberic acid, HOOC(CH2)8COOH has pKa1= 4.21 and pKa2 = 5.40. Offer a plausible reason as to why
A handbook lists the following formula for the percent ionization of a weak acid.(a) Derive this equation. What assumptions must you make in this derivation?(b) Use the equation to determine the
Here is a way to test the validity of the statement made in conjunction with the three key ideas governing the ionization of polyprotic acids. Determine the pH of 0.100 M succinic acid in two ways:
Phosphorous acid is listed in Appendix D as a diprotic acid. Propose a Lewis structure for phosphorous acid that is consistent with this fact. TABLE D.1 Ground-State Electron Configurations Element
What mass of acetic acid,CH3COOH, must be dissolved per liter of aqueous solution if the solution is to have the same freezing point as 0.150 M ClCH2COOH (chloroacetic acid)?
What is the pH of a solution that is 0.68 M H2SO4 and 1.5 M HCOOH (formic acid)?
Use the concept of hybrid orbitals to describe the bonding in the strong acids given in Exercise 78.Exercise 78The following very strong acids are formed by the reactions indicated:(a) Identify the
An aqueous solution of two weak acids has a stoichiometric concentration, c, in each acid. If one acid has a Ka value twice as large as the other, show that the pH of the solution is given by the
The following four equilibria lie to the right:(a) Rank all the acids involved in order of decreasing acid strength.(b) Rank all the bases involved in order of decreasing base strength.(c) State
Given that Ka for HI is about 109, estimate the equilibrium concentrations of HI and I- in (a) 1.0 M HI(aq);(b) 1.0 M NaI(aq).
In this problem, we will use material balance and charge balance concepts to calculate the equilibrium concentrations in an extremely dilute solution of a strong acid, 1.0 x 10-7 M HCl(aq).(a) Write
Follow the approach described in Exercise 101 for 1.0 x 10-6 M HCl(aq) to verify the claim that the self-ionization of water contributes less than 1% to the total amount of H3O+ in solution.Exercise
By focusing on the relative stabilities of the anions formed by ionization, rank the following compounds in each case in order of increasing acid strength (from weakest to strongest).(a) CH3COOH,
Show that in an extremely dilute solution of an acid, the degree of ionization, α, has the value Ka/(Ka + 10-7) at 25 C.
Maleic acid is a carbon–hydrogen–oxygen compound used in dyeing and finishing fabrics and as a preservative of oils and fats. In a combustion analysis, a 1.054 g sample of maleic acid yields
In Example 16-9, rather than use the quadratic formula to solve the quadratic equation, we could have proceeded in the following way. Substitute the value yielded by our failed assumption—x =
Apply the general method for solution equilibrium calculations to determine the pH values of the following solutions. In applying the method, look for valid assumptions that may simplify the
In your own words, define or explain the following terms or symbols: (a) Kw; (b) pH; (c) pKa;(d) Hydrolysis;(e) Lewis acid.
Briefly describe each of the following ideas or phenomena:(a) Conjugate base; (b) Percent ionization of an acid or a base; (c) Self-ionization; (d) Amphiprotic behavior.
Explain the important distinctions between each pair of terms: (a) Brønsted–Lowry acid and base;(b) [H3O+] and pH; (c) Ka for NH4+ and Kb for NH3;(d) Leveling effect and electron-withdrawing
Of the following, the amphiprotic ion is (a) HCO3-;(b) CO32-;(c) NH4+;(d) CH3NH3+;(e) ClO4-.
The pH in 0.10 M CH3CH2COOH(aq) must be (a) Equal to [H3O+] in 0.10 M HNO2(aq);(b) Less than the pH in 0.10 M HI(aq); (c) Greater than the pH in 0.10 M HBr(aq); (d) Equal to 1.0.
In 0.10 M CH3NH2(aq), (a) [H3O+] = 0.10 M;(b) [OH-] = 0.10 M;(c) pH < 7;(d) pH < 13.
The reaction of CH3COOH(aq) proceeds furthest toward completion with a base when that base is (a) H2O;(b) CH3NH3+;(c) NH4+;(d) Cl-;(e) CO32-.
In 0.10 M H2SO4(aq), [H3O+] is equal to (a) 0.050 M;(b) 0.10 M; (c) 0.11 M; (d) 0.20 M.
What is the pH of the solution obtained by mixing 24.80 mL of 0.248 M HNO3 and 15.40 mL of 0.394 M KOH?
How many milliliters of a concentrated acetic acid solution (35.0% CH3COOH by mass; d = 1.044 g/mL) must be diluted with water to produce 12.5 L of solution with pH 3.25?
Several aqueous solutions are prepared. Without consulting any tables in the text, arrange these ten solutions in order of increasing pH: 1.0 M NaBr, 0.05 M CH3COOH, 0.05 M NH3, 0.02 M KCH3COO, 0.05
A solution is found to have pH = 5 x pOH. Is this solution acidic or basic? What is [H3O+] in the solution? Which of the following could be the solute in this solution: NH3, CH3COOH, or NH4CH3COO,
The equilibria OH- + HClO ⇌ H2O + ClO- and ClO- + HNO2 ⇌ HClO + NO2- both lie to the right. Which of the following is a list of acids ranked in order of decreasing strength? (a) HCIO (b) ClO (c)
The conjugate acid of HPO42- is (a) PO43-;(b) H2PO4-;(c) H3PO4;(d) H3O+;(e) None of these.
Without doing detailed calculations, determine which of the following will raise the pH when added to 1.00 L of 0.100 M NH3(aq):(a) 0.010 mol NH4Cl(s);(b) 0.010 mol (CH3CH2)2NH(l);(c) 0.010 mol
For a solution that is 0.275 M CH3CH2COOH (propionic acid, Ka = 1.3 x 10-5) and 0.0892 M HI, calculate (a) [H3O+];(b) [OH-];(c) CH3CH2COO; (d) [I-].
(a) Determine [H3O+] and [CH3COO-] in 0.100 M CH3COOH. (b) Then determine these same quantities in a solution that is 0.100 M in both CH3COOH and HCl.
(A) Determine [H3O+] and [HF] in 0.500 M HF. Then determine these concentrations in a solution that is 0.100 M HCl and 0.500 M HF.(B) How many drops of 12 M HCl would you add to 1.00 L of 0.100 M
You are asked to make a buffer with a pH value close to 4 that would best resist an increase in pH. You can select one of the following acid–conjugate base pairs: acetic acid–acetate, Ka = 1.8 x

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