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

18. Aqueous 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

A 25.0-mL sample of 0.125 M pyridine is titrated with
0.100 M HCl. Calculate the pH at each volume of added acid:
10 mL.

Ethylenediamine (NH2CH2CH2NH2, abbreviated en) is an organic base that can accept two protons: 
(a) Consider the titration of 30.0 mL of 0.100 M ethylenediamine 
with 0.100 M HCl. Calculate the pH after 
the addition of the following volumes of acid, and construct 
a qualitative plot of pH versus milliliters of HCl 
added: 
(i) 0.0 mL (ii) 15.0 mL 
(iii) 30.0 mL (iv) 45.0 mL 
(v) 60.0 mL (vi) 75.0 mL

Weak Base Strong Acid Titration Example

Weak Base Strong Acid Titrations 2

A 25.0-mL sample of 0.125 M pyridine is titrated with
0.100 M HCl. Calculate the pH at each volume of added acid:
0 mL, 10 mL, 20 mL, equivalence point, one-half equivalence
point, 40 mL, 50 mL. Sketch the titration curve.<img src="https://lightcat-files.s3.amazonaws.com/problem_images/0ab6ec31496242d7-1682540014953.jpg" alt="" />

Weak Base Strong Acid Titrations 3

Consider the titration of a 25.0-mL sample of 0.175 M CH3NH2
with 0.150 M HBr. Determine each quantity.
e. the pH at the equivalence point

(a) Calculate the pH of a buffer that is 0.12 M in lactic acid
and 0.11 M in sodium lactate.

A 25.0-mL sample of 0.125 M pyridine is titrated with
0.100 M HCl. Calculate the pH at each volume of added acid:
40 mL.

A 1.0-L buffer solution is 0.125 M in HNO2 and 0.145 M in 
NaNO2. Determine the concentrations of HNO2 and NaNO2 
after the addition of each substance: 
a. 1.5 g HCl

A 25.0-mL sample of 0.125 M pyridine is titrated with
0.100 M HCl. Calculate the pH at each volume of added acid:
equivalence point.

Weak Base Strong Acid Titrations

16.6 Weak Base-Strong Acid Titrations

Weak Base Strong Acid Titrations 4

A 100.0-mL buffer solution is 0.100 M in NH3 and 0.125 M in
NH4Br. What mass of HCl can this buffer neutralize before the pH
falls below 9.00?

Neutralization reactions involving either a strong acid or a 
strong base go essentially to completion, and therefore we 
must take such neutralizations into account before calculating 
concentrations in mixtures of acids and bases. Consider 
a mixture of 3.28 g of Na3PO4 and 300.0 mL of 0.180 M 
HCl. Write balanced net ionic equations for the neutralization 
reactions and calculate the pH of the solution.

Find the pH: NH3 and HCl (Titration: Strong Acid/Weak Base)

Consider the titration of 30.0 mL of 0.050 M NH3 with 
0.025 M HCl. Calculate the pH after the following volumes 
of titrant have been added: (b) 20.0 mL.

A 25.0-mL sample of 0.125 M pyridine is titrated with
0.100 M HCl. Calculate the pH at each volume of added acid:
50 mL.

Calculate the pH at the equivalence point for titrating 
0.200 M solutions of each of the following bases with 0.200 
M HBr: (b) hydroxylamine 1NH2OH2.

A buffer contains 0.10 mol of acetic acid and 0.13 mol of
sodium acetate in 1.00 L. (c) What is the pH of the buffer after the addition of 0.02 mol of HNO3?

17.2 Titrations and Titration Curves | General Chemistry

Consider the titration of a 25.0-mL sample of 0.175 M CH3NH2
with 0.150 M HBr. Determine each quantity.
c. the pH at 5.0 mL of added acid

A 1.00 L buffer solution is 0.250 M in HF and 0.250 M in NaF. Calculate the pH of the solution after the addition of 100.0 mL of 1.00 M HCl. (Ka = 3.5 x 10^-4) 
(a) 4.11
(b) 3.82
(c) 3.46
(d) 3.09

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 (b) 0.0060 mol of HBr. Assume that the volume remains constant.

Consider the titration of 30.0 mL of 0.050 M NH3 with 
0.025 M HCl. Calculate the pH after the following volumes 
of titrant have been added: (e) 61.0 mL.

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.)
<img src="https://lightcat-files.s3.amazonaws.com/problem_images/946d693a9a94f2ab-1675353269514.jpg" alt="" />.
(a) To which of the following stages do solutions 1–4 correspond? 
(i) The initial solution before addition of any HCl 
(ii) Halfway to the equivalence point 
(iii) At the equivalence point 
(iv) Beyond the equivalence point

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).
a. What is the pH of blood plasma?

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

Use the formulas for the acid and base shown on the titration curve to determine the type of acid and base used.

Correct, NH3 is a weak base and HCl is a strong acid.

a strong acid titrated with a strong base

 The starting pH and the pH at the equivalence point indicate the two substances being used in the titration. 

The plot below illustrates which type of titration? <img src="https://media.pearsoncmg.com/ph/esm/esm_tro_chemistry_6/msa/content/practice-quiz/img/troama5_pq_c18q15.jpg" alt="Titration curve showing a graph of pH on the vertical acid and volume of HCl added in mL on the horizontal axis. The titration curve begins at pH 11.12 on the left of the graph and drops slowly to pH 8 at 25 mL of HCl added. At this point the curve drops rapidly to pH 3 when about 26 mL of HCl has been added. The graph then very slowly drops to pH of about 1.8 when 50 mL of HCl has been added." class="block">

A solution is made by mixing 1.5 g of LiOH and 23.5 mL of
1.000 M HNO3. (c) Is the resulting solution acidic or basic?

General Chemistry | Strong Acid & Weak Base Titration

Consider the titration of a 25.0-mL sample of 0.175 M CH3NH2 
with 0.150 M HBr. Determine each quantity. 
a. the initial pH

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/38a2077ac4cf2cb2-1673022516342.jpg" alt="" />.
(b) Draw a picture that represents the equilibrium state of solution (1) after the addition of two H3O+ ions.

A 25.0-mL sample of 0.125 M pyridine is titrated with
0.100 M HCl. Calculate the pH at each volume of added acid:
0 mL.

Weak Base Strong Acid Titration Calculations

A 25.0-mL sample of 0.125 M pyridine is titrated with
0.100 M HCl. Calculate the pH at each volume of added acid:
20 mL.

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

Weak Base Strong Acid Titration Practice

Use the initial concentration of NH3 and the Kb expression to calculate the concentration of OH&#215; and then convert to pH.

Correct, the solution is distinctly basic.

NH3 is a weak base; the equilibrium gives OH&#8722;.

What is the initial pH for the titration of 30.0 mL of 0.850 M NH3 with 0.100 M HCl. Kb for NH3 = 1.8 &#215; 10&#8722;5.

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? 
(c) CH3NH2 (methylamine) and HCl

Weak Base Strong Acid Titrations 1

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Weak Acid Strong Base Titrations

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

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;