Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

10. Acids and Bases

Strong Acid Strong Base Titrations (Simplified)

GOB Chemistry

10. Acids and Bases

Strong Acid Strong Base Titrations (Simplified)

Previous problemNext problem

2:30 minutes

Problem 108d

Textbook Question

Determine each of the following for a 0.100 M HBr solution:
d. milliliters of the HBr solution required to neutralize 36.0 mL of a 0.250 M LiOH solution

Verified step by step guidance

Step 1: Write the balanced chemical equation for the neutralization reaction. HBr (a strong acid) reacts with LiOH (a strong base) in a 1:1 molar ratio to form water and lithium bromide:

{HBr}_{} + {LiOH}_{} \to {H 2 O}_{} + {LiBr}_{}

Step 2: Calculate the moles of LiOH in the given solution. Use the formula

moles = molarity \times volume

, where the molarity is 0.250 M and the volume is 36.0 mL (convert to liters by dividing by 1000).

Step 3: Since the reaction is a 1:1 molar ratio, the moles of HBr required to neutralize the LiOH will be equal to the moles of LiOH calculated in Step 2.

Step 4: Use the formula

volume = \frac{moles}{molarity}

to calculate the volume of the HBr solution required. The moles of HBr are from Step 3, and the molarity of the HBr solution is 0.100 M.

Step 5: Convert the volume of HBr solution from liters to milliliters by multiplying by 1000. This will give the final volume of HBr solution required to neutralize the LiOH solution.

Verified video answer for a similar problem:

This video solution was recommended by our tutors as helpful for the problem above

Video duration:

Play a video:

Was this helpful?

Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Neutralization Reaction

A neutralization reaction occurs when an acid reacts with a base to produce water and a salt. In this case, HBr (hydrobromic acid) reacts with LiOH (lithium hydroxide) to form water and lithium bromide. Understanding this reaction is crucial for determining the stoichiometry involved in the neutralization process.

Molarity (M)

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (M). In this problem, the molarity of HBr and LiOH solutions is essential for calculating the volume of HBr needed to neutralize the given volume of LiOH.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. For the neutralization of HBr and LiOH, the stoichiometric coefficients indicate the ratio in which the reactants react, allowing us to determine the required volume of HBr solution to completely neutralize the LiOH solution.

Watch next

Master Strong Acid Strong Base Titrations (Simplified) Concept 1 with a bite sized video explanation from Jules

Start learning

Related Videos

Related Practice

Textbook Question

If 32.8 mL of a 0.162 M NaOH solution is required to titrate 25.0 mL of a solution of H₂SO₄, what is the molarity of the H₂SO₄ solution?

H₂SO₄(aq) + 2 KOH(aq) → 2 H₂O(l) + K₂SO₄(aq)

1357

views

Textbook Question

How many grams of Al(OH)₃ are required to neutralize 150. mL of stomach acid with a pH of 1.5?

686

views

Textbook Question

A 0.205 M NaOH solution is used to titrate 20.0 mL of a solution of H₂SO₄. If 45.6 mL of the NaOH solution is required to reach the endpoint, what is the molarity of the H₂SO₄ solution?

H₂SO₄(aq) + 2NaOH(aq) → 2H₂O(l) + Na₂SO₄

1409

views

Textbook Question

Calculate the volume, in milliliters, of a 0.150 M NaOH solution that will completely neutralize each of the following:

a. 25.0 mL of a 0.288 M HCl solution

707

views

Textbook Question

One of the most acidic lakes in the United States is Little Echo Pond in the Adirondacks in New York. Recently, this lake had a pH of 4.2, well below the recommended pH of 6.5.

c. One way to raise the pH (and restore aquatic life) is to add limestone (CaCO₃). How many grams of CaCO₃ are needed to neutralize 1.0 kL of the acidic water from Little Echo Pond if the acid is sulfuric acid?

H₂SO₄(aq) + CaCO₃(s) → CO₂(g) + H₂O(l) + CaSO₄(aq)

836

views

Textbook Question

The daily output of stomach acid (gastric juice) is 1000 mL to 2000 mL. Prior to a meal, stomach acid (HCl) typically has a pH of 1.42.

c. The antacid milk of magnesia contains 400. mg of Mg(OH)₂ per teaspoon. Write the neutralization equation, and calculate the number of milliliters of stomach acid neutralized by 1 tablespoon of milk of magnesia (1tablespoon = 3teaspoons).

631

views

Multiple Choice

How many grams of HNO₃ are required to completely neutralize 110.0 mL of 0.770 M LiOH?

788

views

Multiple Choice

What is the molar mass of a 0.350 g sample of a HA acid if it requires 50.0 mL of 0.440 M Sr(OH)₂ to completely neutralize it? A is used as a place holder for the unknown nonmetal of the acid.