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Brønsted-Lowry Acid-Base Concepts

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Questions and Answers

What distinguishes a strong acid from a weak acid according to the Bronsted-Lowry definition?

Strong acids can only react with bases, while weak acids can react with both bases and other acids.

Strong acids only donate protons, while weak acids accept protons.

Strong acids completely dissociate in solution while weak acids do not. (correct)

Strong acids have higher molecular weights than weak acids.

In the acid-dissociation equation HA ⇌ H⁺ + A⁻, which species is considered the conjugate base?

Both A⁻ and H⁺

A⁻ (correct)

H⁺

How does the equilibrium constant (Ka) relate to the strength of an acid?

Ka is related solely to the molecular structure of the acid.

Stronger acids have higher Ka values. (correct)

Ka values do not affect acid strength.

Higher Ka values indicate weaker acids.

At what point on the titration curve does the pKa of an acid correspond?

<p>At the half-equivalence point.</p> Signup and view all the answers

How does the ratio of [HA] to [A⁻] change with increasing pH?

<p>The ratio of [HA] decreases and [A⁻] increases.</p> Signup and view all the answers

Study Notes

Brønsted-Lowry Acid-Base Definitions

A Brønsted-Lowry acid is a proton (H+) donor.
A Brønsted-Lowry base is a proton acceptor.

Acid Strength

Strong acids completely dissociate in water.
Weak acids only partially dissociate in water.

Acid-Dissociation Equations

Acid-dissociation equations show the equilibrium between an acid and its conjugate base in water.
Example: HA + H₂O ⇌ H₃O⁺ + A⁻
HA is the acid.
A⁻ is the conjugate base.

Equilibrium Constant (Ka) and pKa

Ka is the acid dissociation constant, quantifying the strength of an acid.
Larger Ka values indicate stronger acids.
pKa = -log₁₀Ka; lower pKa values correspond to stronger acids.

Titration Curves and pKa

pKa is found at the midpoint of the titration curve's buffer region.
This is where the concentrations of the acid (HA) and conjugate base (A⁻) are equal.

[HA]:[A⁻] and pH

The ratio of [HA] to [A⁻] changes with pH.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation relates pKa, pH, and the ratio of [HA] to [A⁻].
It allows calculation of the ratio of [HA] to [A⁻] at a given pH.

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Description

This quiz covers the Brønsted-Lowry definitions of acids and bases, the concept of acid strength, and the importance of acid-dissociation equations. Additionally, it explores the equilibrium constant (Ka), the Henderson-Hasselbalch equation, and the significance of titration curves in understanding acidity.