Chemistry Acids and Bases Overview

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Questions and Answers

What type of reaction is an acid-base reaction?

A proton (H+) transfer reaction

What is an amphoteric substance?

A substance that can act as either an acid or a base

What produces OH- ions when placed in water?

Base

What is a Bronstead Lowry acid?

A proton (H+) donor Signup and view all the answers

What is a Bronstead Lowry base?

A proton (H+) acceptor Signup and view all the answers

What is a buffer solution?

A solution that resists a change in pH when limited amounts of acid or base are added Signup and view all the answers

What is buffer capacity?

The maximum amount of acid or base that can be added before the buffer stops working Signup and view all the answers

What is formed when you add a proton (H+) to a base?

Conjugate acid Signup and view all the answers

What is the conjugate base?

What you get when you remove a proton (H+) from an acid Signup and view all the answers

What is a conjugate acid-base pair?

Any pair of molecules or ions that can be interconverted by transfer of a proton (H+) Signup and view all the answers

What are diprotic acids?

Acids that can give up two protons (H+) Signup and view all the answers

What is the hydronium ion?

H3O+ Signup and view all the answers

What is an indicator?

A substance that changes color at a certain pH Signup and view all the answers

What is the ion product of water (Kw) at room temperature?

1.0 x 10-14 Signup and view all the answers

What are monoprotic acids?

Acids that can give up only one proton (H+) Signup and view all the answers

How is pH calculated?

-log[H3O+] Signup and view all the answers

What defines a strong acid or strong base?

Dissociates completely (100%) when put in water Signup and view all the answers

What are triprotic acids?

Acids that can give up three protons (H+) Signup and view all the answers

What defines weak acids and weak bases?

Dissociates partially (less than 100%) when put in water Signup and view all the answers

Study Notes

Acids and Bases

Acids produce hydronium ions (H3O+) when dissolved in water.
Bases produce hydroxide ions (OH-) when dissolved in water.
Acid-base reactions involve the transfer of protons (H+).
Amphoteric substances can act as both acids and bases.

Brønsted-Lowry Theory

A Brønsted-Lowry acid is a proton (H+) donor.
A Brønsted-Lowry base is a proton (H+) acceptor.
A conjugate acid-base pair is formed when an acid donates a proton to a base.
The conjugate acid is formed by adding a proton to the base.
The conjugate base is formed by removing a proton from the acid.

pH and pOH

pH is a measure of the acidity of a solution.
pH is calculated as the negative logarithm of the hydronium ion concentration: pH = -log[H3O+].
pOH is a measure of the basicity of a solution.
pOH is calculated as the negative logarithm of the hydroxide ion concentration: pOH = -log[OH-].

Strength of Acids and Bases

Strong acids and strong bases dissociate completely in water.
Weak acids and weak bases dissociate partially in water.

Buffer Solutions

Buffer solutions resist changes in pH when small amounts of acid or base are added.
Buffer solutions consist of a weak acid and its conjugate base.
Buffer capacity is the maximum amount of acid or base that can be added before the buffer stops working.

Ion Product of Water (Kw)

Kw is the equilibrium constant for the autoionization of water.
At room temperature, Kw has a value of 1.0 x 10^-14.
Kw = [H3O+][OH-] = 1.0 x 10^-14.

Polyprotic Acids

Diprotic acids can donate two protons (H+).
Triprotic acids can donate three protons (H+).
Monoprotic acids can donate only one proton (H+).

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Description

Test your knowledge on the properties of acids and bases, including the Brønsted-Lowry theory and calculations of pH and pOH. This quiz covers essential concepts such as hydronium and hydroxide ions, proton transfer, and the strength of acids and bases. Perfect for chemistry students looking to reinforce their understanding!