18. Aqueous Equilibrium

Weak Acid Strong Base Titrations

Weak Acid-Strong Base Titrations

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<img src="https://lightcat-files.s3.amazonaws.com/problem_images/b71875fd28fd33fc-1673371183681.jpg" alt="" />

Weak Acid Strong Base Titrations 3

16.5 pH Calculations for Weak Acids and Bases | General Chemistry

Weak Acid Strong Base Titrations 2

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

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?

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?

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

For this 1:1 reaction, at the equivalence point, moles of acid = moles of base or MaVa=MbVb.

The concentration of the acid is greater than that of the base in this 1:1 reaction thus requiring a larger volume of base for complete neutralization.

Correct for this reaction with 1:1 stoichiometry.

 At the equivalence point, the number of moles of strong base added is equal to the initial number of moles of weak acid. 

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. Ka for HF = 3.5 &#215; 10&#8722;4.

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.

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?

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.

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.

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

This is the pOH after the addition of the excess KOH.

A solution containing excess KOH will be basic with a pH greater than 7.

Determine the excess number of moles of KOH added and the total volume of the solution.

Correct determination of the pH based on excess KOH.

 Only the excess moles of KOH in the total volume will contribute to the pH beyond the equivalence point. 

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.

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

Weak Acid-Strong Base Reactions Concept 4

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.

Weak Acid-Strong Base Reactions Concept 3

Based on initial moles of acid, moles of base added and the total volume of the solution, determine the concentration of the acid and conjugate base.  Then use the Henderson-Hasselbalch equation to determine the pH.

At this point in the titration the concentration of the conjugate base is greater than that of the acid.

This would be the pH at half-neutralization.

 The titration is in the buffer region at this point. 

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. Ka for HC2H3O2 = 1.8 &#215; 10&#8722;5.

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?

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

A buffer contains 0.10 mol of acetic acid and 0.13 mol of
sodium acetate in 1.00 L. (b) What is the pH of the buffer after the addition of 0.02 mol of KOH?

17.2 Titrations and Titration Curves | General Chemistry

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

This is the pOH at the equivalence point.

The pH at the endpoint will be greater than 7 due to the reaction of acetate ion with water to produce OH&#215;.

The calculation of the pH involves determining the total volume at the endpoint, the concentration of acetate at the endpoint and the use of the K expression for the reaction of acetate with water.

Correct calculations in all steps required.

 At the equivalence point of the titration of a weak acid with a strong base, all of the weak acid has been converted into its conjugate base. 

Calculate the pH at the equivalence point for the titration of 20.0 mL of 0.500 M HC2H3O2 with 0.350 M KOH. Ka for HC2H3O2 = 1.8 &#215; 10&#8722;5.

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.) <img src="https://lightcat-files.s3.amazonaws.com/problem_images/7a607a4a2f3b04cd-1673024566316.jpg" alt="" />.
(c) Draw a picture that represents the equilibrium state of solution (1) after the addition of two OH-ions.

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

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.

Weak Acid Strong Base Titrations 1

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.

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.

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.

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

Weak Acid-Strong Base Reactions Concept 2

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

Weak Acid Strong Base Titration Calculations

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.

Weak Acid-Strong Base Reactions Concept 1

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.

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.

The conjugate base of any weak will react with water to produce OH&#215;.

Correct, conjugate base reacts with water to produce OH&#215;.

depends on the Ka of the acid used

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

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1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Whenever a WEAK ACID reacts with a STRONG BASE we use an ICF Chart to determine the pH of the solution.&#160;

Strong Acid Strong Base Titrations

In a Strong Acid-Strong Base Titration we do not use an ICF Chart or ICE Chart to determine the pH of the solution.&nbsp;

Titrations of Diprotic and Polyprotic Acids

A diprotic or polyprotic buffer can be approached in a way similar to monoprotic buffers. The key difference is that multiple pKa values will be involved.&#160;

Buffer

Weak Base Strong Acid Titrations

Whenever a&nbsp;WEAK BASE reacts with a&nbsp;STRONG ACID we use an&nbsp;ICF Chart to determine the pH of the solution.&nbsp;