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18. Aqueous Equilibrium

Titrations: Weak Acid-Strong Base

18. Aqueous Equilibrium

Titrations: Weak Acid-Strong Base

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Before the Equivalence Point

Before the Equivalence Point

Titrations: Weak Acid-Strong Base Example

Titrations: Weak Acid-Strong Base Example

At the Equivalence Point

At the Equivalence Point

Titrations: Weak Acid-Strong Base Example

Titrations: Weak Acid-Strong Base Example

After the Equivalence Point

After the Equivalence Point

Titrations: Weak Acid-Strong Base Example

Titrations: Weak Acid-Strong Base Example

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Acid - Base Equilibria | Weak Acid - Strong Base Titration.

Acid - Base Equilibria | Weak Acid - Strong Base Titration.

Weak Acid-Strong Base Titrations

Weak Acid-Strong Base Titrations

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17.2 Titrations and Titration Curves | General Chemistry

17.2 Titrations and Titration Curves | General Chemistry

Titration of a weak acid with a strong base (continued) | Khan Academy

Titration of a weak acid with a strong base (continued) | Khan Academy

Khan Academy Organic Chemistry

Titration of a weak acid with a strong base | Chemistry | Khan Academy

Titration of a weak acid with a strong base | Chemistry | Khan Academy

Khan Academy Organic Chemistry

16.5 pH Calculations for Weak Acids and Bases | General Chemistry

16.5 pH Calculations for Weak Acids and Bases | General Chemistry

Showing 6 of 6 videos

Practice this topic

Multiple Choice

Calculate the volume (mL) of 0.500 M NaOH required to reach the equivalence point in the titration of 25.0 mL of 0.650 M HF. K_a for HF = 3.5 × 10⁻⁴.

Multiple Choice

For a titration of a weak acid with a strong base, the pH at the equivalence point ________.

Multiple Choice

20.0 mL of 0.500 M HC₂H₃O₂ is titrated with 0.350 M KOH. Determine the pH after 15.0 mL of the base has been added. K_a for HC₂H₃O₂ = 1.8 × 10⁻⁵.

Multiple Choice

20.0 mL of 0.500 M HC₂H₃O₂ is titrated with 0.350 M KOH. Determine the pH after 15.0 mL of the base has been added. K_a for HC₂H₃O₂ = 1.8 × 10⁻⁵.

Multiple Choice

Determine the pH when 5.00 mL of excess KOH (beyond the equivalence point) has been added to the titration of 20.0 mL of 0.500 M HC₂H₃O₂ with 0.350 M KOH.

Multiple Choice

Calculate the pH at the equivalence point for the titration of 20.0 mL of 0.500 M HC₂H₃O₂ with 0.350 M KOH. K_a for HC₂H₃O₂ = 1.8 × 10⁻⁵.

Multiple Choice

In order to create a buffer 7.510 g of sodium cyanide is mixed with 100.0 mL of 0.250 M hydrocyanic acid, HCN. What is the pH of the buffer solution after the addition of 12.0 mL of 0.300 M NaH? K_a = 4.9 × 10⁻¹⁰.

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Multiple Choice

Consider the titration of 75.0 mL of 0.60 M HNO₂ with 0.100 M NaOH at the equivalence point. What would be the pH of the solution at the equivalence point? The K_a of HNO₂ is 4.6 × 10⁻⁴.

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Multiple Choice

Calculate the pH of the solution resulting from the mixing of 55.0 mL of 0.100 M NaCN and 75.0 mL of 0.100 M HCN with 0.0090 moles of NaOH.

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Textbook Question

The following pictures represent initial concentrations in solutions that contain a weak acid HA (pKa = 6.0) and its sodium salt NaA. (Na+ ions and solvent water molecules have been omitted for clarity.)

. (c) Draw a picture that represents the equilibrium state of solution (1) after the addition of two OH-ions.

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Textbook Question

Calculate the pH of the solution that results from each mixture. b. 125.0 mL of 0.10 M NH3 with 250.0 mL of 0.10 M NH4Cl

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Textbook Question

A 35.0-mL sample of 0.150 M acetic acid 1CH3COOH2 is titrated with 0.150 M NaOH solution. Calculate the pH after the following volumes of base have been added: (b) 17.5 mL.

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Textbook Question

Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (c) benzoic acid 1C6H5COOH2.

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Textbook Question

Calculate the pH at the equivalence point in titrating 0.100 M solutions of each of the following with 0.080 M NaOH: (b) chlorous acid 1HClO22.

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Textbook Question

A 100.0-mL buffer solution is 0.175 M in HClO and 0.150 M in NaClO. c. What is the pH after addition of 85.0 mg of NaOH?

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Textbook Question

For each solution, calculate the initial and final pH after adding 0.010 mol of NaOH. c. 250.0 mL of a buffer solution that is 0.255 M in CH3CH2NH2 and 0.235 M in CH3CH2NH3Cl

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Textbook Question

Phenol (C6H5OH, Ka = 1.3 x 10^-10) is a weak acid used in mouthwashes, and pyridine (C5H5N, Kb = 1.8 x 10^-9) is a weak base used as a solvent. Calculate the value of Kn for the neutralization of phenol by pyridine. Does the neutralization reaction proceed very far toward completion?

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Textbook Question

The equilibrium constant Kn for the neutralization of lactic acid (C3H6O3) and urea (CH4N2O) is 2.1 x 10^-4. What is Kb for urea? The Ka of lactic acid is 1.4 x 10^-4.

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Textbook Question

Blood is buffered by carbonic acid and the bicarbonate ion. Normal blood plasma is 0.024 M in HCO3- and 0.0012 M H2CO3 (pKa1 for H2CO3 at body temperature is 6.1). c. Given the volume from part (b), what mass of NaOH can be neutralized before the pH rises above 7.8?

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Textbook Question

Determine the [H3O+] and pH of a 0.100 M solution of benzoic acid.

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Textbook Question

Determine the [H3O+] and pH of a 0.200 M solution of formic acid.

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Textbook Question

Calculate the pH of 0.375 L of a 0.18 M acetic acid–0.29 M sodium acetate buffer before and after the addition of (a) 0.0060 mol of KOH. Assume that the volume remains constant.

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Textbook Question

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 25 mL.

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Textbook Question

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 5 mL.

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Textbook Question

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 20 mL.

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Textbook Question

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 10 mL.

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Textbook Question

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: equivalence point.

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Textbook Question

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 0 mL.

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Textbook Question

A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 M KOH. Calculate the pH at each volume of added base: 0 mL, 5 mL, 10 mL, equivalence point, one-half equivalence point, 20 mL, 25 mL. Sketch the titration curve.

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Textbook Question

Consider the titration of 40.0 mL of 0.250 M HF with 0.200 M NaOH. How many milliliters of base are required to reach the equivalence point? Calculate the pH at each of the following points. (d) After the addition of 80.0 mL of base

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Textbook Question

A sample of 0.1687 g of an unknown monoprotic acid was dissolved in 25.0 mL of water and titrated with 0.1150 M NaOH. The acid required 15.5 mL of base to reach the equivalence point. (b) After 7.25 mL of base had been added in the titration, the pH was found to be 2.85. What is the Ka for the unknown acid?

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Textbook Question

What is the pH at the equivalence point for the titration of 0.10 M solutions of the following acids and bases, and which of the indicators in Figure 17.5 would be suitable for each titration? (a) HNO2 and NaOH

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Textbook Question

Consider the titration of 50.0 mL of a 0.100 M solution of the protonated form of the amino acid alanine (H2A+: Ka1 = 4.6 x 10^-3, Ka2 = 2.0 x 10^-10) with 0.100 M NaOH. Calculate the pH after the addition of each of the following volumes of base. (a) 10.0 mL

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