Acids and bases MCQ 3

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Questions and Answers

What characteristic property distinguishes acids from bases when using litmus paper?

Acids turn blue litmus red. (correct)

Acids do not affect litmus paper.

Acids neutralize red litmus paper.

Acids maintain litmus paper color.

Which statement correctly describes a dibasic acid?

It has a pH less than 7.

It donates three H⁺ ions.

It donates two H⁺ ions. (correct)

It does not dissociate in solution.

What role does water play in the behavior of acids?

Water has no effect on acidic properties.

Water aids in the dissociation of acids into hydrogen ions. (correct)

Water neutralizes acids completely.

Water is essential for acids to form salts.

Which of the following best describes a strong acid according to the Arrhenius theory?

It dissociates completely to produce hydrogen ions Signup and view all the answers

According to the pH scale, which value indicates a basic solution?

9 Signup and view all the answers

What is one limitation of the Arrhenius theory?

It does not account for all amphoteric substances Signup and view all the answers

When an acid neutralizes a base, what are the products of this reaction?

Salt and water Signup and view all the answers

How does a monobasic acid differ from a dibasic acid in terms of hydrogen ion donation?

Monobasic acids donate one H⁺ ion. Signup and view all the answers

What occurs to red litmus paper when it is placed in an acidic solution?

It remains red. Signup and view all the answers

What is a common characteristic of both acids and bases?

Both can be corrosive. Signup and view all the answers

How do weak acids compare to strong acids in terms of their ability to donate protons?

Strong acids are better proton donors than weak acids. Signup and view all the answers

Which statement accurately describes the dissociation behavior of strong acids in water?

Strong acids completely dissociate into hydrogen ions and anions. Signup and view all the answers

What distinguishes a weak base from a strong base according to the Bronsted-Lowry theory?

Weak bases do not accept protons as effectively as strong bases. Signup and view all the answers

What is the role of hydrogen ions in the conductivity of acids in aqueous solutions?

Hydrogen ions enhance the conductivity by allowing better charge flow. Signup and view all the answers

Which of the following accurately defines a conjugate pair according to Bronsted-Lowry theory?

An acid and base pair that differ by a proton Signup and view all the answers

How does sodium hydroxide dissociate in water and why is this relevant to its classification as a strong base?

It completely dissociates in water to produce hydroxide ions. Signup and view all the answers

What is the conjugate base of CH₃COOH?

CH₃COO- Signup and view all the answers

Which factor primarily accounts for the electrical conductivity differences between weak and strong acids?

Weak acids have fewer hydrogen ions in the solution. Signup and view all the answers

Which of the following best describes a Bronsted-Lowry acid?

A compound that donates protons. Signup and view all the answers

Study Notes

Characteristic Properties of Acids and Bases

Acids turn blue litmus paper red and have a pH < 7.
Acids react with metals to produce hydrogen gas and are known for their corrosive nature.
Bases turn red litmus paper blue and have a pH > 7.
Bases neutralize acids and also exhibit corrosive properties.

Monobasic vs. Dibasic Acids

A monobasic acid can donate one H⁺ ion, while a dibasic acid can donate two H⁺ ions.

pH Value Significance

A pH value below 7 indicates acidity, while above 7 indicates basicity; a pH of 7 is considered neutral.

Role of Litmus

Litmus paper serves as an indicator, changing color to red in acidic solutions and blue in basic solutions.

Arrhenius Acid and Base Definitions

Arrhenius acid: Dissociates in water to form hydrogen ions (H⁺).
Arrhenius base: Dissociates in water to produce hydroxide ions (OH⁻).

Conductivity of Strong Acids

Strong acids dissociate in water to produce hydrogen ions and anions, allowing them to conduct electricity effectively.

Limitations of the Arrhenius Theory

The Arrhenius theory is limited to reactions in aqueous solutions and does not account for substances that show amphoteric behavior.

Water's Role in Acidity

Water is crucial for acids to exhibit acidic properties, enabling the dissociation of acids into hydrogen ions.

Products of Neutralization

Neutralization involves a reaction between an acid and a base, yielding salt and water.

Conductivity of Weak vs. Strong Acids/Bases

Weak acids and bases are poor electrical conductors, whereas strong acids and bases are good conductors.

Conductivity of Acids in Water

Acids conduct electricity in water by dissociating to form hydrogen ions, which facilitate conductivity.

Sodium Hydroxide as a Strong Base

Sodium hydroxide is considered a strong base because it fully dissociates in water, generating hydroxide ions.

Bronsted-Lowry Acid Definition

In the Bronsted-Lowry theory, an acid is defined as a proton donor.

Strong vs. Weak Acids in Bronsted-Lowry Terms

A strong acid is an effective proton donor, while a weak acid does not donate protons readily.

Bronsted-Lowry Base Definition

A base, according to Bronsted-Lowry, is a proton acceptor.

Strong vs. Weak Bronsted-Lowry Bases

A strong Bronsted-Lowry base is efficient in accepting protons, in contrast to a weak base which is not.

Conjugate Pairs Definition

A conjugate pair consists of an acid and its corresponding base that differ by a single proton.

Conjugate Acid and Base Examples

The conjugate base of acetic acid (CH₃COOH) is acetate (CH₃OO⁻).
The conjugate acid of the hydrogen phosphate ion (HPO₄²⁻) is the dihydrogen phosphate ion (H₂PO₄⁻).

Definitions of Conjugate Acid and Base

A conjugate acid is a species formed when a base gains a proton.
A conjugate base results from an acid donating a proton.

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Description

Test your knowledge on the properties of acids and bases, including their effects on litmus paper and their pH values. Learn the differences between monobasic and dibasic acids and understand the significance of pH in chemical reactions.