Understanding Acid-Base Equilibria

Understanding Acid-Base Equilibria

12th Grade

10 Qs

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Understanding Acid-Base Equilibria

Understanding Acid-Base Equilibria

Assessment

Quiz

Others

12th Grade

Practice Problem

Easy

Created by

Fikadu Mulugeta

Used 2+ times

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10 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the definition of an acid according to the Brønsted-Lowry theory?

A Brønsted-Lowry acid is a substance that increases pH.

A Brønsted-Lowry acid is a proton donor.

A Brønsted-Lowry acid is a molecule that donates electrons.

A Brønsted-Lowry acid is a proton acceptor.

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Explain the concept of pH and how it relates to hydrogen ion concentration.

pH is inversely related to hydrogen ion concentration; as [H+] increases, pH decreases.

pH is directly proportional to hydrogen ion concentration.

pH increases as hydrogen ion concentration increases.

pH has no relation to hydrogen ion concentration.

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the difference between a strong acid and a weak acid?

Strong acids are always more concentrated than weak acids.

Weak acids have a higher pH than strong acids.

Strong acids are less corrosive than weak acids.

Strong acids fully dissociate in solution; weak acids partially dissociate.

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

Describe the role of a conjugate base in acid-base reactions.

A conjugate base accepts protons and can participate in reverse reactions.

A conjugate base has no role in chemical reactions.

A conjugate base is always a strong acid.

A conjugate base donates protons to acids.

5.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How does Le Chatelier's principle apply to acid-base equilibria?

Le Chatelier's principle applies to acid-base equilibria by predicting how the equilibrium will shift in response to changes in concentration, temperature, or pressure.

Le Chatelier's principle states that equilibrium cannot be shifted.

Le Chatelier's principle only applies to gas reactions.

Acid-base equilibria are unaffected by temperature changes.

6.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the significance of the acid dissociation constant (Ka)?

It measures the temperature of an acid solution.

It determines the solubility of an acid in water.

The significance of the acid dissociation constant (Ka) is that it indicates the strength of an acid in solution.

It indicates the color change of an acid in a pH indicator.

7.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

How do buffers work to maintain pH in a solution?

Buffers work by increasing the concentration of hydrogen ions.

Buffers maintain pH by neutralizing added acids or bases through equilibrium reactions.

Buffers change the temperature of a solution to affect pH.

Buffers only absorb excess water in a solution.

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