18. Aqueous Equilibrium

Intro to Acid-Base Titration Curves

18. Aqueous Equilibrium

Intro to Acid-Base Titration Curves

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Acid-Base Titration Curve

The Equivalence Point

Intro to Acid-Base Titration Curves Example

Shape of a Titration Curve

Intro to Acid-Base Titration Curves Example

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Basic Principles of Acid-Base Titrations

Acid Base Titration Curves

PremedHQ Science Academy

Professor Dave Explains

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17.2 Titrations and Titration Curves | General Chemistry

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17.2 Titrations and Titration Curves | General Chemistry

Chad's Prep

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Multiple Choice

What will be the color of the indicator in the above question in a solution that has a pH of 6?

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Multiple Choice

Consider the titration of 60.0 mL of 0.200 M H₃PO₃ solution with 0.350 M potassium hydroxide, KOH solution. How many milliliters of base would be required to reach each of its equivalence points?

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Multiple Choice

Which of the following acids would be needed to combine with its potassium salt to produce a solution buffered at pH 5.00?

Chlorous acid: pK_a = 1.95
Nitrous acid: pK_a = 3.34
Formic acid: pK_a = 3.74
Acetic acid: pK_a = 4.74
Hypochlorous acid: pK_a = 7.54

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Multiple Choice

Consider the titration of 100.0 mL of 0.40 M HCl with 0.40 M NaOH. If sodium hydroxide is the titrant, which volume would place it in excess?

a) 70.0 mL b) 25.0 mL c) 100.0 mL d) 110.0 mL e) 9.0 mL

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Textbook Question

Which of the following mixtures has the highest pH? (a) Equal volumes of 1.0 M HCl and 1.0 M NaOH (b) Equal volumes of 0.1 M HNO3 and 0.1 M KOH (c) Equal volumes of 0.1 M HCN and 0.1 M NaOH (d) Equal volumes of 0.1 M NaF and 0.1 M HCl

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Textbook Question

The following figure represents solutions at various stages of the titration of a weak acid, HA, with NaOH. (The Na+ ions and water molecules have been omitted for clarity.) To which of the following regions of the titration curve does each drawing correspond: (b) after addition of NaOH but before the equivalence point? [Section 17.3]

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Textbook Question

Match the following descriptions of titration curves with the diagrams: (a) strong acid added to strong base. [Section 17.3]

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Textbook Question

Which data set, of the two graphed here, would you expect to observe from a titration like that shown in Figure 4.18?

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Textbook Question

The accompanying graph shows the titration curves for two monoprotic acids. (d) Estimate the pKa of the weak acid.

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Textbook Question

Compare the titration of a strong, monoprotic acid with a strong base to the titration of a weak, monoprotic acid with a strong base. Assume the strong and weak acid solutions initially have the same concentrations. Indicate whether the following statements are true or false. (a) More base is required to reach the equivalence point for the strong acid than the weak acid.

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Textbook Question

The samples of nitric and acetic acids 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 NaOH1aq2 is needed to reach the equivalence point in the titration of HNO3.

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Textbook Question

Determine whether each of the following statements concerning the titrations in Problem 17.35 is true or false. (b) The titration curves will both be essentially the same after passing the equivalence point.

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Textbook Question

Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (b) NH3 titrated with HCl.

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Textbook Question

The strong acid HA is mixed with an equal molar amount of aqueous NaOH. Which of the following pictures represents the equilibrium state of the solution? (Na+ ions and solvent water molecules have been omitted for clarity.)

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Textbook Question

Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (c) pyridine titrated with nitric acid.

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Textbook Question

Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (b) calcium hydroxide titrated with perchloric acid.

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Textbook Question

Predict whether the equivalence point of each of the following titrations is below, above, or at pH 7: (a) formic acid titrated with NaOH.

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Textbook Question

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 HA. (c) Is the pH 7, less than 7, or more than 7 at the equivalence point?

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Textbook Question

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 HA. (a) How many moles of HA have been added at the equivalence point?

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Textbook Question

The following plot shows two pH titration curves, each representing the titration of 50.0 mL of 0.100 M acid with 0.100 M NaOH:

. (b) What is the approximate pH at the equivalence point for each of the acids?

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Textbook Question

The following plot shows two pH titration curves, each representing the titration of 50.0 mL of 0.100 M acid with 0.100 M NaOH:

. (a) Which of the two curves represents the titration of a strong acid? Which represents a weak acid?

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Textbook Question

The following plot shows two pH titration curves, each representing the titration of 50.0 mL of 0.100 M acid with 0.100 M NaOH:

. (c) What is the approximate pKa of the weak acid?

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Textbook Question

The following pictures represent solutions at various stages in the titration of a weak base B with aqueous HCl. (Cl- ions and solvent water molecules have been omitted for clarity.)

. (b) Is the pH at the equivalence point more or less than 7?

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Textbook Question

How many milliliters of 0.105 M HCl are needed to titrate each of the following solutions to the equivalence point: (b) 22.5 mL of 0.118 M NH3?

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Textbook Question

Is the pH greater than, equal to, or less than 7 after the neutralization of each of the following pairs of acids and bases? (c) HBr and aniline (C6H5NH2)

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Textbook Question

Is the pH greater than, equal to, or less than 7 after the neutralization of each of the following pairs of acids and bases? (c) KOH and HI

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Textbook Question

Is the pH greater than, equal to, or less than 7 after the neutralization of each of the following pairs of acids and bases? (a) NaOH and benzoic acid (C6H5CO2H)

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Textbook Question

Which of the following mixtures has the higher pH? (a) Equal volumes of 0.10 M HCN and 0.10 M NaOH (b) Equal volumes of 0.10 M HClO4 and 0.10 M NaOH

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Textbook Question

The graphs labeled (a) and (b) show the titration curves for two equal-volume samples of monoprotic acids, one weak and one strong. Both titrations were carried out with the same concentration of strong base. (a) (b) (i) What is the approximate pH at the equivalence point of each curve?

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Textbook Question

(b)

(ii) Which graph corresponds to the titration of the strong acid and which one to the titration of the weak acid?

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Textbook Question

The graphs labeled (a) and (b) show the titration curves for two equal-volume samples of bases, one weak and one strong. Both titrations were carried out with the same concentration of strong acid. a. b. (ii) Which graph corresponds to the titration of the strong base and which one to the weak base?

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Textbook Question

Consider the curve shown here for the titration of a weak monoprotic acid with a strong base and answer each question.

d. At what volume of added base is the pH calculated by working an equilibrium problem based on the concentration and Kb of the conjugate base?

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Textbook Question

Consider the curve shown here for the titration of a weak base with a strong acid and answer each question.

d. At what volume of added acid is the pH calculated by working an equilibrium problem based on the concentration and Ka of the conjugate acid?

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Textbook Question

Consider the curve shown here for the titration of a weak base with a strong acid and answer each question.

a. What is the pH and what is the volume of added acid at the equivalence point?

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Textbook Question

Consider the titration of a 20.0-mL sample of 0.105 M HC2H3O2 with 0.125 M NaOH. Determine each quantity. b. the volume of added base required to reach the equivalence point

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Textbook Question

Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH. (a)

(b)

(i) Which acid solution is more concentrated?

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Textbook Question

Consider the titration curves (labeled a and b) for two weak acids, both titrated with 0.100 M NaOH. (a)

(b)

(ii) Which acid has the larger Ka?

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Textbook Question

Consider the titration curves (labeled a and b) for two weak bases, both titrated with 0.100 M HCl. (a)

(b)

(ii) Which base has the larger Kb?

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Textbook Question

A 0.229-g sample of an unknown monoprotic acid is titrated with 0.112 M NaOH. The resulting titration curve is shown here. Determine the molar mass and pKa of the acid.

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Textbook Question

The distinctive odor of vinegar is due to acetic acid, CH3COOH, which reacts with sodium hydroxide according to: CH3COOH1aq2 + NaOH1aq2¡ H2O1l2 + NaCH3COO1aq2 If 3.45 mL of vinegar needs 42.5 mL of 0.115 M NaOH to reach the equivalence point in a titration, how many grams of acetic acid are in a 1.00-qt sample of this vinegar?

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Textbook Question

A 4.36-g sample of an unknown alkali metal hydroxide is dissolved in 100.0 mL of water. An acid–base indicator is added, and the resulting solution is titrated with 2.50 M HCl(aq) solution. The indicator changes color, signaling that the equivalence point has been reached, after 17.0 mL of the hydrochloric acid solution has been added. (b) What is the identity of the alkali metal cation: Li+, Na+, K+, Rb+, or Cs+?

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Textbook Question

On the same graph, sketch pH titration curves for the titra-tion of (1) a strong acid with a strong base and (2) a weak acid with a strong base. How do the two curves differ with respect to the following? (a) The initial pH

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Textbook Question

A sample of 0.2140 g of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.0950 M NaOH. The acid required 30.0 mL of base to reach the equivalence point. (a) What is the molar mass of the acid?

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Textbook Question

A 1.248-g sample of limestone rock is pulverized and then treated with 30.00 mL of 1.035 M HCl solution. The excess acid then requires 11.56 mL of 1.010 M NaOH for neutralization. Calculate the percentage by mass of calcium carbonate in the rock, assuming that it is the only substance reacting with the HCl solution.

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Textbook Question

The equivalence point was reached in titrations of three unknown acids at pH 9.16 (acid A), 8.88 (acid B), and 8.19 (acid C). (a) Which is the strongest acid? (b) Which is the weakest acid?

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Textbook Question

The equivalence point was reached in titrations of three unknown bases at pH 5.53 (base A), 4.11 (base B), and 6.00 (base C). (a) Which is the strongest base? (b) Which is the weakest base?

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Textbook Question

(a) By titration, 15.0 mL of 0.1008 M sodium hydroxide is needed to neutralize a 0.2053-g sample of a weak acid. What is the molar mass of the acid if it is monoprotic?

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Textbook Question

(a) A 0.1044-g sample of an unknown monoprotic acid requires 22.10 mL of 0.0500 M NaOH to reach the end point. What is the molar mass of the unknown?

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Textbook Question

In analytical chemistry, bases used for titrations must often be standardized; that is, their concentration must be precisely determined. Standardization of sodium hydroxide solutions can be accomplished by titrating potassium hydrogen phthalate (KHC8H4O4), also known as KHP, with the NaOH solution to be standardized. b. The titration of 0.5527 g of KHP required 25.87 mL of an NaOH solution to reach the equivalence point. What is the concentration of the NaOH solution?

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Textbook Question

A 5.55-g sample of a weak acid with Ka = 1.3 * 10 - 4 was combined with 5.00 mL of 6.00 M NaOH, and the resulting solution was diluted to 750.0 mL. The measured pH of the solution was 4.25. What is the molar mass of the weak acid?

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Textbook Question

A 40.0 mL sample of a mixture of HCl and H3PO4 was titrated with 0.100 M NaOH. The first equivalence point was reached after 88.0 mL of base, and the second equiva-lence point was reached after 126.4 mL of base. (c) What percent of the HCl is neutralized at the first equivalence point?

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18. Aqueous Equilibrium

Intro to Acid-Base Titration Curves

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