Introduction to Acids and Bases IB Chemistry Power Points Topic 08 Acids and Bases .

Introduction to

Acids and Bases

IB Chemistry Power Points

Topic 08

Acids and Bases

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In aqueous solutions, a proportion of the water molecules dissociate;

The ions formed are H+ or positively charged hydrogen ions and negatively charged hydroxide ions (OH-)

Technically

2 H2O(l) H

3O+

(aq) + OH-

(aq)

Kw = [H + ][OH − ] = 1 x 10-14

Some chemical compounds contribute additional H+ to make the solution more acidic. Other compounds remove H+ ions.

A compound that increases H+ is called an acid

Examples: HCl, H2SO4, HNO3, CH3COOH

A compound that removes H+ ions from an aqueous solution is called a base. This reaction is called a neutralization.

Often this is done by adding OH- ions for example NaOH, KOH, Ca(OH)2. Soluble bases are called alkalis.

Neutralization Reactions hydroxides

acid + base water + saltHCl + NaOH H2O + NaCl (aq)

• metal oxidesacid + base water + salt2 HCl + Cu2O H2O + CuCl2 (aq)

• ammoniaacid + base salt HCl + NH3 NH4Cl (aq)

Three theories of acidsArrhenius (most common)

Bronsted-LowryLewis

Arrhenius (most common): an acid dissociates to yield H+ and a base dissociates to yield

OH-

Hydrochloric acid H+ + Cl-

Sodium hydroxide Na+ + OH-

Bronsted-Lowry:

an acid is a proton (H+) donor

and a base is a proton acceptor

amphiprotic

Lewis: An acid is an electron pair

acceptor

and a base is an electron pair donor

A dative covalent bond is formed

Example of Lewis Acid

Lewis Acid Lewis

Base

This is a common example that is not an obvious acid/base rxn

Boron trifluoride acts as a Lewis Acid. The boron has only 6 electron in valence shell so the lone pair of electrons forms a dative bond and fills up the valence shell of the boron

IndicatorsAcids and bases are substances with specific physical and chemical properties.

We can determine if substances are acidic or basic by testing their reaction with indicators.

Indicators are organic substances that change color in the presence of an acid or a base.

Some common indicatorsin acid in base

Litmus red bluePhenolphthalein colorless pinkMethyl orange red yellow

Reactions of acidsReact with active metals (above copper in

reactivity series)2 HCl + Ca CaCl2 + H2

Reaction with carbonatesH2SO4 + Na2CO3 Na2SO4 + CO2 + H2O

Reaction with bicarbonatesHNO3 + NaHCO3 NaNO3 + CO2 + H2O

Acid/base properties of Period 3 oxides (topic 3)

Metal oxides Na2O and MgO react with water to form hydroxides (basic solutions)

Na2O + H2O 2 NaOH (aq)

Aluminum oxide is amphoteric (will react as a base with an acid or vice versa)

Al2O3 + 6 HCl 2 AlCl3 + 3 H2O

Other period 3 oxides (non-metal S, P, Cl oxides) react with water to form acidic solutions

SO3 + H2O H2SO4 (aq)

see page 15 in study guide

Acid/base properties of Period 3 chlorides (topic 13)

Chlorides across Period 3 become more acidic across the period

NaCl (aq) is neutral

MgCl2 (aq) is weakly acidic

Chlorides of Al, Si, P, S and Cl2 react with

water to produce HCl (aq) solutions

see Study guide page 16

Strong Acids vs Weak Acids

The strength of an acid or base depends on how easily it dissociates in water.

The dissociation of an acid or base is an equilibrium.

HA(aq) H+(aq) + A-

(aq)

BOH(aq) B+(aq) + OH-

(aq)Strong acids or bases dissociate (ionize) easily – the equilibrium favors the ionic products : kc >> 1

Strong vs Weak

When the strength of an acid or base is discussed, it is very important NOT to confuse “strength” with “concentration”

A 5M acid solution contains 5 mol of acid per dm3 but its strength is determined by how much of that acid is ionized.

Strong acids : HCl, H2SO

4, HNO

3 (mono vs

diprotic)Strong bases : NaOH, KOH, Ba(OH)

2

Weak acids: CH3COOH, H

2CO

3, carbonic acid

CO2(aq)

Weak bases: NH3, ethylamine CH

3CH

2NH

2

Strong vs Weak

How to tellStrong acids and bases are mostly ionized and therefore solutions are good electrolytes (high conductivity). The pH of the solution can also be measured.

What is the pH scale?pH is a measurement of hydrogen ion

concentration

It tells you how acids or basic (or alkaline) something is

Ranges from 0 (most acidic) to 14 (most basic

log[ ]pH H

How does scale work?

The scale is logarithmic. As you go up or down, the concentration is changed by a power of ten

Example pH 3 is 100 times more concentrated than pH 5

neutral

pH 10 is 100 times less concentrated than pH 8

Strong Acid

example HCl

HCl(aq) H+(aq) + Cl-(aq)

+ -[H ][Cl ]k = >> 1

[HCl]

• completely dissociated

• pH of 0.1 M soln = 1• strong electrolyte• reacts vigorously • note simplified “net

ionic” equation

Weak Acid

example CH3COOH

CH3COOH (aq) H+

(aq) + CH3COO-

(aq)

+ -3

3

[H ][CH COO ]k = << 1

[CH COOH]

• partially dissociated• pH of 0.1 M soln = 2.9• weak electrolyte• reacts slowly