Determine the pH of (a) M HCN and (b) (aniline).

According to the Brnsted Lowry theory, label each of the following as an acid or a base. (a) (b) (c) (d) (e)

Write the formula of the conjugate base in the reaction of each acid with water. (a) (b) (c) (d)

For each of the following, identify the acids and bases involved in both the forward and reverse directions. (a) (b) (c) (d)

Which of the following species are amphiprotic in aqueous solution? For such a species, write one equation showing it acting as an acid, and another equation showing it acting as a base. .

With which of the following bases will the ionization of acetic acid, CH3COOH, proceed furthest toward NO2 -, HCO3 -, HBr HS-OH , -, NH4 +, H2O, C6H5NH3 + + OH- C6H5NH2 + H2O HS- + H2O H2S + OH- HSO4 - + H2O SO4 2- + H3O+ HOBr + H2O OBr- + H3O+ C2H5NH3 + HPO4 2-; HIO3; C6H5COOH; CH3NH3 + NH4 +NH2 ; -OCl ; -; HNO2; completion (to the right): (a) (b) (c) (d) Explain your answer.

In a manner similar to equation (16.6), represent the self-ionization of the following liquid solvents: (a) (b) HF; (c) (d) (e)

With the aid of Table 16.1, predict the direction (forward or reverse) favored in each of the following acid base reactions. (a) (b) (c)

With the aid of Table 16.1, predict the direction (forward or reverse) favored in each of the following acid base reactions. (a) (b) (c) H2CO3 + CO3 2- HCO3 - + HCO3 - HNO2 + ClO4 - HClO4 + NO2 - CH3COOH + CO3 2- HCO3 - + CH3COO CH3COOH + CH3O- CH3OH + CH3COO HSO4 - + NO3 - HNO3 + SO4 2- NH4 + + OH- H2O +

Calculate and for each solution: (a) 0.00165 M (b) 0.0087 M KOH; (c) 0.00213 M (d) 5.8 * 10 M HI. Sr1OH2 -4 2; HNO3; 3OH-3H3O 4 +4

What is the pH of each of the following solutions? (a) 0.0045 M HCl; (b) (c) 0.00683 M NaOH; (d) 4.8 * 10-3 M Ba1OH22.

Calculate and pH in saturated which contains 3.9 g per 100 mL of solution.

Asaturated aqueous solution of has a pH of 12.35. What is the solubility of expressed in milligrams per 100 mL of solution?

What is in a solution obtained by dissolving 205 mL HCl(g), measured at and 751 mmHg, in 4.25 L of aqueous solution?

What is the pH of the solution obtained when 125 mL of 0.606 M NaOH is diluted to 15.0 L with water?

How many milliliters of concentrated HCl(aq) (36.0% HCl by mass, ) are required to produce 12.5 L of a solution with

How many milliliters of a 15.0%, by mass solution of KOH(aq) are required to produce 25.0 L of a solution with pH = 11.55? 1d = 1.14 g>mL2 pH = 2.10? d = 1.18 g>mL 23 C 3H3O+4 Ca1OH22, Ca1OH22 Ba1OH22 # 8 H2O 3H3O Ba1OH221aq2, +4

What volume of 6.15 M HCl(aq) is required to exactly neutralize 1.25 L of

A 28.2 L volume of HCl(g), measured at 742 mmHg and is dissolved in water. What volume of measured at 762 mmHg and must be absorbed by the same solution to neutralize the HCl?

50.00 mL of 0.0155 M HI(aq) is mixed with 75.00 mL of 0.0106 M KOH(aq). What is the pH of the final solution?

25.00 mL of a solution with a pH of 2.12 is mixed with 25.00 mL of a KOH(aq) solution with a pH of 12.65. What is the pH of the final solution?

What are the and pH of

What are the and pH of

For the ionization of phenylacetic acid, (a) What is in (b) What is the pH of

A 625 mL sample of an aqueous solution containing 0.275 mol propionic acid, has What is the value of for propionic acid?

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 Calculate of fluoroacetic acid.

Caproic acid, found in small amounts in coconut and palm oils, is used in making artificial flavors. Asaturated aqueous solution of the acid contains and has Calculate for the acid.

What mass of benzoic acid, would you dissolve in 350.0 mL of water to produce a solution with a

What must be the molarity of an aqueous solution of trimethylamine, if it has a K b = 6.3 * 10-5 1CH323N + H2O 1CH323NH+ + OH- 1CH323N, pH = 11.12? Ka = 6.3 * 10-5 C6H5COOH + H2O H3O+ + C6H5COO- pH = 2.85? C6H5COOH, HC6H11O2 + H2O H3O+ + C6H11O2 - K a = ? K11 g>L pH = 2.94. a HC6H11O2, H3O+1aq2 + CH2FCOO-1aq2 K a = ? CH2FCOOH1aq2 + H2O pH = 1.56. Ka Ka = ? CH3CH2CO2H + H2O H3O+ + CH3CH2CO2 - K 3H3O 0.00239 M. a +4 = CH3CH2CO2H, 0.121 M C6H5CH2CO2H? 0.186 M C6H5CH2CO2H? 3C6H5CH2CO2 -4 K a = 4.9 * 10-5 C6H5CH2CO2H + H2O H3O+ + C6H5CH2CO2 3H3O 0.085 M C2H5NH2? +4 3H3O 0.143 M HNO2? +4

What are pH, and pOH of

What are pH, and pOH of 0.386 M

The solubility of 1-naphthylamine, a substance used in the manufacture of dyes, is given in a handbook as 1 g per What is the approximate pH of a saturated aqueous solution of 1-naphthylamine?

A saturated aqueous solution of o-nitrophenol, has What is the solubility of o-nitrophenol in water, in grams per liter?

A particular vinegar is found to contain 5.7% acetic acid, by mass. What mass of this vinegar should be diluted with water to produce 0.750 L of a solution with

A particular household ammonia solution is 6.8% by mass. How many milliliters of this solution should be diluted with water to produce 625 mL of a solution with

A 275 mL sample of vapor in equilibrium with 1-propylamine at is removed and dissolved in 0.500 L For 1-propylamine, and (a) What should be the pH of the aqueous solution? (b) How many mg of NaOH dissolved in 0.500 L of water give the same pH?

One handbook lists a value of 9.5 for of quinoline, a weak base used as a preservative for anatomical specimens and to make dyes. Another handbook lists the solubility of quinoline in water at as Use this information to calculate the pH of a saturated solution of quinoline in water.

The sketch on the far left represents the present in an acetic acid solution of molarity M. If the molarity of the solution is doubled, which of the sketches below best represents the resulting solution? (a) (b) (c) (d) 3H3O+4

The sketch on the far left represents the present in an ammonia solution of molarity M. If the solution is diluted to half its original molarity, which of the sketches below best represents the resulting solution? (a) (b) (c) (d)

What is the (a) degree of ionization and (b) percent ionization of propionic acid in a solution that is 0.45 M

What is the (a) degree of ionization and (b) percent ionization of ethylamine, in an 0.85 M aqueous solution?

What must be the molarity of an aqueous solution of if it is 4.2% ionized?

What must be the molarity of an acetic acid solution if it has the same percent ionization as (propionic acid, K )? a = 1.3 * 10CH -5 3CH2CO2H 0.100 M NH3 C2H5NH2, pKa = 4.89 CH3CH2CO2H + H2O H3O+ + CH3CH2CO2 - CH3CH2CO2H?

Continuing the dilutions described in Example 16-8, should we expect the percent ionization to be 13% in 0.0010 M and 42% in 0.00010 M Explain.

What is the (a) degree of ionization and (b) percent ionization of trichloroacetic acid in a 0.035 M solution? pK a = 0.52

Explain why in 1.00 M is not simply but much, much less than

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 content.

Determine and for the following solutions: (a) 0.075 M (b) 0.0050 M (c)

For 0.045 M a weak diprotic acid, calculate (a) (b) and (c) Use data from Table 16.4 as necessary.

Calculate and in (a) 0.75 M (b) 0.075 M (c) [Hint: Check any assumptions that you make.]

Adipic acid, is among the top 50 manufactured chemicals in the United States HOOC1CH224COOH, 7.5 * 10-4 H2SO4; H2SO4; M H2SO4. 3SO4 2-3H3O 4 +4, 3HSO4 -4, 3CO3 2-3HCO3 4. -3H3O 4, +4, H2CO3, 1.0 * 10-5 M H2S. H2S1aq2 H2S; H2S; 3S2-3H3O 4 +4, 3HS-4, H3PO4 1 3 3H3O+4. 1 3 3H3O+4, 3PO4 H3PO4 3-4 (nearly 1 million metric tons annually). Its chief use is in the manufacture of nylon. It is a diprotic acid having and A saturated solution of adipic acid is about 0.10 M Calculate the concentration of each ionic species in this solution.

The antimalarial drug quinine, is a diprotic base with a water solubility of of solution. (a) Write equations for the ionization equilibria corresponding to and (b) What is the pH of saturated aqueous quinine?

For hydrazine, and 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 M N2H41aq2.

Codeine, 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 C18H21O3N, for protonated codeine, Write the reaction for and calculate for codeine.

Approximately 4 metric tons of quinoline, is produced annually. The principal source of quinoline is coal tar. Quinoline is a weak base in water. A handbook gives for protonated quinoline, Write the ionization reaction for and calculate pK for quinoline.

Complete the following equations in those instances in which a reaction (hydrolysis) will occur. If no reaction occurs, so state. (a) (b) (c) K+1aq2 + C6H5COO-1aq2 + H2O (d) (e)

From data in Table 16.3, determine (a) for (b) for (c) for

Predict whether a solution of each of the following salts is acidic, basic, or pH neutral: (a) KCl; (b) KF; (c) (d) (e)

Arrange the following 0.010 M solutions in order of increasing pH: NaOH(aq),

What is the pH of an aqueous solution that is 0.089 M NaOCl?

What is the pH of an aqueous solution that is 0.123 M

Sorbic acid, is widely used in the food industry as a preservative. For example, its potassium salt (potassium sorbate) is added to cheese to inhibit the formation of mold. What is the pH of 0.37 M potassium sorbate solution?

Pyridine, 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 0.0482 M

For each of the following ions, write two equations one showing its ionization as an acid and the other as a base: (a) (b) (c) Then use data from Table 16.4 to predict whether each ion makes the solution acidic or basic.

Suppose you wanted to produce an aqueous solution of 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) NaNO3. pH = 8.65 HPO4 -HS . -HSO3 ; -; C5H5NH+Cl-1aq2. 1pKb C5H5N = 8.822, 4.772, CH2CH CH

Predict which is the stronger acid: (a) or (b) or (c) or Explain.

Explain why trichloroacetic acid, is a stronger acid than acetic acid,

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) or

Indicate which of the following is the weakest acid, and give reasons for your choice: HBr; CH3CH2COOH; CH2FCH2COOH; CI3COOH. CH2ClCOOH; CH3CH2CCl2COOH. I3CCH2CH2CO

From the following bases, select the one with the smallest and the one with the largest and give reasons for your choices. (a) (b) (c) (d)

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. CH3CH2CH2NH2 N

For each reaction draw a Lewis structure for each species and indicate which is the acid and which is the base: (a) (b) (c) (d)

In the following reactions indicate which is the Lewis acid and which is the Lewis base: (a) (b)

Indicate whether each of the following is a Lewis acid or base. (a) (b) (c)

Each of the following is a Lewis acid base reaction. Which reactant is the acid, and which is the base? Explain. (a) (b)

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) (c)

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, CO21g2 + LiOH1s2 LiHCO31s2 CO21g2 1C2H522O + BF3 1C2H522OBF3 N2H4 + H3O+ N2H5 + + H2O B1OH23 + OH- 3B1OH244- Zn(OH)2(s) + 2 OH-(aq) 3Zn(OH)442-(aq) SO3 + H2O H2SO4 OH 1C2H523B; CH3NH2. -; HgCl3 - + Cl - HgCl4 2- SOI2 + BaSO3 Ba2+ + 2 I - + 2 SO2 S2- + SO3 S2O3 2- O2- + H2O 2 OH- H2O + BF3 H2OBF3 CO2 + H2O H2CO3

The molecular solid is only slightly soluble in water but will dissolve to a much greater extent in an aqueous solution of KI, because the anion forms. Write an equation for the formation of the anion, and indicate the Lewis acid and Lewis base.

The following very strong acids are formed by the reactions indicated: (called super acid, hexafluoroantimonic acid) (tetrafluoroboric acid) (a) Identify the Lewis acids and bases. (b) To which atom is the H atom bonded in each acid?

Use Lewis structures to diagram the following reaction in the manner of reaction (16.20). Identify the Lewis acid and Lewis base.

Use Lewis structures to diagram the following reaction in the manner of reaction (16.19). Identify the Lewis acid and Lewis base.

The Brnsted 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. Indicate whether each of the following would be an acid, a base, or amphiprotic in pure liquid acetic acid, as a solvent. (a) (b) (c) (d) [Hint: Refer to Table 16.1.]

The pH of saturated is found to be 13.12. A10.0 mL sample of saturated is diluted to 250.0 mL in a volumetric flask. A10.0 mL sample of the diluted is transferred to a beaker, and some water is added. The resulting solution requires 25.1 mL of a HCl solution for its titration. What is the molarity of this HCl solution?

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 that can be matched to a pH value, identify each solution and its pH value. Identify the solutions that cannot be matched, and give reasons why matches are not possible. (a) 0.010 M 1 2 3 4 5 6 7 8 9 10 11 12 13 14 Sr1OH221aq2 Sr1OH221aq2 Sr1OH221aq2 CH3COOH; HClO4. CH3COO H2O; -CH3COOH, ; (b) 1.0 M (c) 0.050 M KI; (d) 0.0020 M (e) 1.0 M NaOCl; (f) 0.10 M (g) 0.10 M HOCl; (h) 0.050 M (i) 0.050 M .

Show that when 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 original concentration, the pH increases by 0.30 unit? Explain.

Explain why in a strong acid solution doubles as the total acid concentration doubles, whereas in a weak acid solution, increases only by about a factor of

Use data from Appendix D to determine whether the ion product of water, increases, decreases, or remains unchanged with increasing temperature.

From the observation that 0.0500 M vinylacetic acid has a freezing point of determine for this acid.

You are asked to prepare a 100.0 mLsample of a solution with a pH of 5.50 by dissolving the appropriate amount of a solute in water with Which of these solutes would you use, and in what quantity? Explain your choice. (a) (b) 12 M HCl(aq); (c) NH4Cl1s2; (d) glacial (pure) acetic acid, CH3COOH.

Determine the pH of (a) M HCN and (b) (aniline).

It is possible to write simple equations to relate pH, pK, and molarities (M) of various solutions. Three such equations are shown here. Weak acid: Weak base: Salt of weak acid and strong base: (a) Derive these three equations, and point out the assumptions involved in the derivations. (b) Use these equations to determine the pH of 0.10 M 0.10 M and 0.10 M Verify that the equations give correct results by determining these pH values in the usual way.

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 percent ionization of a formic acid solution, HCOOH(aq), with a pH of 2.50. (c) A 0.150 M solution of propionic acid, has a pH of 2.85. What is for propionic acid?

Oxalic acid, HOOCCOOH, a weak diprotic acid, has and Arelated diprotic acid, suberic acid, has and Offer a plausible reason as to why the difference between and is so much greater for oxalic acid than for suberic acid.

Here is a way to test the validity of the statement made on page 719 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: first by assuming that is produced only in the first ionization step, and then by allowing for the possibility that some is also produced in the second ionization step. Compare the results, and discuss the significance of your finding.

What mass of acetic acid, must be dissolved per liter of aqueous solution if the solution is to have the same freezing point as 0.150 M (chloroacetic acid)?

What is the pH of a solution that is 0.68 M and 1.5 M (formic acid)?

An aqueous solution of two weak acids has a stoichiometric molarity, M, in each acid. If one acid has a value twice as large as the other, show that the pH of the solution is given by the equation Assume that the criteria for the simplifying assumption on page 715 are met.

Use the concept of hybrid orbitals to describe the bonding in the strong acids given in Exercise 78.

Phosphorous acid is listed in Appendix D as a diprotic acid. Propose a Lewis structure for phosphorous acid that is consistent with this fact.

The following four equilibria lie to the right: and (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 whether each of the following two equilibria lies primarily to the right or to the left: (i) (ii) CH3NH2 H2SO3.

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 1.599 g and 0.327 g In a freezing-point depression experiment, a 0.615 g sample of maleic acid dissolved in 25.10 g of glacial acetic acid, (which has the freezing-point depression constant and in which maleic acid does not ionize), lowers the freezing point by In a titration experiment, a 0.4250 g sample of maleic acid is dissolved in water and requires 34.03 mL of 0.2152 M KOH for its complete neutralization. The pH of a 0.215 g sample of maleic 0.82C. Kf = 3.90 C m-1 CH3COOH1l2 CO2 H2O. acid dissolved in 50.00 mL of aqueous solution is found to be 1.80. (a) Determine the empirical and molecular formulas of maleic acid. [Hint: Which experiment(s) provide the necessary data?] (b) Use the results of part (a) and the titration data to rewrite the molecular formula to reflect the number of ionizable H atoms in the molecule. (c) Given that the ionizable H atom(s) is(are) associated with the carboxyl group(s), write the plausible condensed structural formula of maleic acid. (d) Determine the ionization constant(s) of maleic acid. If the data supplied are insufficient, indicate what additional data would be needed. (e) Calculate the expected pH of a 0.0500 M aqueous solution of maleic acid. Indicate any assumptions required in this calculation.

In Example 16-7, 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 into the denominator of the quadratic equation; that is, use as the value of and solve for a new value of x. Use this second value of x to re-evaluate Solve the simple quadratic equation for a third value of x, and so on. After three or four trials, you will find that the value of x no longer changes. This is 3CH3NH24 = 10.00250 - second value of x2. 3CH3NH24: 3CH3NH24 10.00250 - 0.00102 x = 0.0010 the answer you are seeking. (a) Complete the calculation of the pH of 0.00250 M by this method, and show that the result is the same as that obtained by using the quadratic formula. (b) Use this method to determine the pH of 0.500 M

Apply the general method for solution equilibrium calculations outlined on page 720 to determine the pH values of the following solutions. In applying the method, look for valid assumptions that may simplify the numerical calculations. (a) a solution that is 0.315 M and 0.250 M (b) a solution that contains 1.55 g and 12.5 g in 375 mL (c) 1.0 M NH4CN1aq2

In your own words, define or explain the following terms or symbols: (a) (b) pH; (c) (d) hydrolysis; (e) Lewis acid.

Briefly describe each of the following ideas or phenomena: (a) conjugate base; (b) percent ionization of an acid or base; (c) self-ionization; (d) amphiprotic behavior.

Explain the important distinctions between each pair of terms: (a) Brnsted Lowry acid and base; (b) and pH; (c) for and for (d) leveling effect and electron-withdrawing effect.

Of the following, the amphiprotic ion is (a) (b) (c) (d) (e)

The pH in 0.10 M must be (a) equal to in 0.10 M (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 (a) (b) (c) (d)

The reaction of proceeds furthest toward completion with a base when that base is (a) (b) (c) (d) (e)

In 0.10 M is equal to (a) 0.050 M; (b) 0.10 M; (c) 0.11 M; (d) 0.20 M.

For and In 0.10 M (a) (b) (c) (d) (e)

What is the pH of the solution obtained by mixing 24.80 mL of 0.248 M and 15.40 mL of 0.394 M KOH?

How many milliliters of a concentrated acetic acid solution (35.0% by mass; ) must be diluted with water to produce 12.5 L of solution with pH 3.25? CH d = 1.044 g>mL 3COOH HNO3 3SO3 2-3H3O 4 = 0.036 M. +4 = 0.013 M; 3H3O+3SO3 4 = 0.10 M; 2-4 = 6.3 * 10-8 M; 3HSO3 -10 H2SO31aq2, 4 = 0.013 M; -8. K a2 H2SO31aq2, K = 6.3 * a1 = 1.3 * 10-2 H2SO41aq2, 3H3O+4 CO3 2-Cl . -NH4 ; +CH3NH3 ; +H2O; ; CH3COOH1aq2 3OH pH 6 7; pH 6 13. -4 = 0.10 M; 3H3O+CH3NH21aq2, 4 = 0.10 M; 3H3O HNO21aq2; +4 CH3CH2COOH1aq2 ClO4 -CH3NH3 . +NH4 ; +CO3 ; 2-; HCO3 -; NH3; K NH4 b + K 3H3O a +4 pK a; K w;

Determine the pH of 2.05 M (Use data from Table 16.3, as necessary.)

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 0.05 M 0.02 M 0.05 M 0.05 M 0.10 M HI, 0.06 M NaOH, 0.05 M and 0.05 M .

A solution is found to have Is this solution acidic or basic? What is in the solution? Which of the following could be the solute in this solution: or and what would be its molarity?

Propionic acid, is 0.42% ionized in 0.80 M solution. The for this acid is (a) (b) (c) (d) (e) none of these.

The conjugate acid of is (a) (b) (c) (d) (e) none of these.

The equilibria and both lie to the right. Which of the following is a list of acids ranked in order of decreasing strength? (a) (b) (c) (d) (e) none of these

3.00 mol of calcium chlorite is dissolved in enough water to produce 2.50 L of solution. for HClO, and for Compute the pH of the solution.

Appendix E describes a useful study aid known as concept mapping. Using the method presented in Appendix E, construct a concept map that summarizes the material discussed in Section 16-8.