academic chemistry acids & bases - pbworks - acid... · academic chemistry ids & bases...

Name

AcAcademic Chemistry

ids & BasesNotes

H+ IonConcentration

Examples ofSolulions

100pH Value

0 "+--+ Hydrochloric acid

10++

102 2 ÿ Stomach acidLemon juice

!0ÿ3 3 Vinegar, cola, beer

!04 -- 4 --- Tomatoes

10-s -- -- 5 ÿ Black coffeeNormal rainwater

IO-6 ÿ -- 6 ÿ UrineSaliva

10 7 ÿ -- 7 ÿ Pu+ÿ} water - --

Blood108 ÿ 8 ÿ Seawater

10,9 +++ 9 ÿ Baking soda/

10+40 -- ":- 10 -- Grea! Salÿ Lake+ Milk of magneskÿ

10'+++ ÿ -- 11 -- Household ammonia

!2 ÿ Household bleach

-- 13 -- Overÿ cleaner

14 Sodium hydroxide

Unit # 14 Test Date :q!ÿors ÿ,rch z'ÿm

Jÿ cincochem, pbworks.com

Notes Unit 14

fBrackets, [ ], mean concentration or...

MOLARITY (M)

So, "[H+] = 1M" means...

The concentration of hydrogen ions is 1 M.

J

2 ÿ% cincochem.pbworks.com Acid Base

Unit 14

Acid - a compound that producesdissolved in water.

ions when

Acids

@

@

Vinegar- ACCÿ __

Lemon juice- Cÿ(-

taste

Reacts with (corrodes)

turns blue litmus paper

¢ÿJFd{/3 to form /qT_ gas

Rcasolutions of acids are

Sour candy -

erties of Acids

® ÿO U if

acid

acid

acid

FX,

clcctrolv sI

react with BASES to form

(must be mixed with water!)

Sÿ!ÿL and %/qÿ

Naminq Acids

Binary acids - H bonded to one nonmetal (HF)

® Begin with ÿqxÿlJiW , use the 00ÿL

of the element name, add the suffix - I 6

/

2, HBr i'3VClÿ P(Oÿ/ÿIC acid/

Ternary Acids - H bonded to a polyatomic ion (H2S04)

c ion without

Acid Base ÿ cincochem.pbworks.com 3

Acids

Add suffix - iCÿ if there was an

Unit 14

Add suffix --QU5 if there was an

1. HNO3 H ÿ-6ÿ-jL AQ8

2. HClO C lo c}us Ac 4

Strength of Acids

STRONG acids - completely __J_O/11 Z,P_,3

dissociate, in water. All the acid breaks into ions., or

HCI + H20 -ÿ H30+ + Cl-1 way arrow ALL IONS AFTER MIXING/

WEAK acids - do rqoÿ ionize completely in solution.Some acid stays intact instead of ionizing.

H2SO3 + H20 ÿ H30+ + SO34SOME ACID 2 head arrow SOME IONS

Binary Acid Strength

There are 3 STRONG Binary acidso ÿ+Clo ÿ1ÿ<o ÿ

® ALL other Binary acids are weak: H2S, H2Se, HF

Ternary Acid Strength

There are 4 STRONG Ternary acids (that we will use!)o iqÿ50ÿo HHOso 14 CÿOÿo HelOt

o All other Ternary acids are weak: H3PO4, H2SO3, HNO2 etc...

A quick way to determine if a ternary acid is strong:SUBTRACT #H from #O's in the acid. If the difference is>_ 2, the acid is strong. Less than 2, the acid is weak.

4 "ÿ cincochem.pbworks.com Acid Base

Unit 14

Base - a compound that produces ÿ (__

ions when dissolved in water.

Bases

)

Examples"

Milk of Magnesia -

Drain cleaner -

vlnO.q FIC5 t Oÿq]

hydroxide

hydroxide

Window cleaner - __ÿ vÿ Yvq o 'mict

[ Red litmus paper with a drop of base here

/]

[4

Blue litmus paper with a drop of acid here )P perties of Bases

o 15,+ÿ tastet

Feels S ÿ ÿpC,r y to the touch

® Does k!OT react with metal

® turns red litmus paper ÿ

o .a%v.eoÿ

e l ec-ÿo i vÿ sI

o reacts with ACIDS to form

solutions of bases are

(must be mixed with water!)

,ÿSÿ Iÿ and WoIÿ'O4f


Bases Unit 14

Narninq Bases

Use the same rules as for ÿhvv\ic /O V t5

ions (name the cation, then name the anion)

1. aaOH 50(ÿiOÿ,q kVdro'ÿ ioÿ

2. Ca(OH)2

3. KOH

4. Mg(OH)2

Strength of Bases

STRONG bases - completely

water. All base breaks into ions.

All hydroxides with groups

m

and

metals (except iÿ_ÿ ) are STRONG bases.

LiOH, NaOH, KOH, RbOH, CsOH

Mg(OH)2, Ca(OH)2, Sr(OH)2, Ba(OH)2, Ra(OH)2

2

in

WEAK bases - I(ÿÿ only

Some of the base stays intact instead of ionizing.

® All bases NOT LISTED ABOVE AS STRONG.

6 ÿ cincochem.pbworks.com Acid Base

Unit 14

An Arrhenius acid must contain a

(ionizes) in water to produce

HArrhenius Theory

and dissociates

,0+]

An Arrhenius base must contain a (3ÿ

(ionizes) in water to produce _ÿ V Ctro ÿ {dÿ!

Practice:

and dissociates

Classify each of the following as an Arrhenius acid orArrhenius base.

Ca(OH)2 ->

HBr -> Arrkÿvlius

H2S04 -> A W'/'ÿqCPÿit)3

LiOH -> A rÿheÿi ÿs

Act o;

]ÿ)CtS-gJ

Disadvantages of Arrhenius Theor_E

Only compounds with

What about ammonia,

Can only be applied to reactions that occur in

wou,d Incorr cf/y

some compounds as acids, such as ÿ ÿ

H can be classified as a base.

classify


Br0nsted Lowry The0ry 0f Acids and Bases

B Zÿnsted-Lowry Theorÿ of Acids and Bases

In an acid-base reaction, substances are defined by theirACTIONS in Brÿnsted - Lowry theory!

Unit 14

The Br0nsted - Lowry acid is the reactant that

The Brÿnsted - Lowry base is the reactant that \6Yÿ

o LI40.I

® The Brensted - Lowry Conjugate acid is the product that

forms after a B-L ÿ0ÿ,ÿ© accepts an H+.

The Brensted - Lowry Conjugate base is the product that

forms after a B-L ÿclcÿ has donated an H+.

To identify the B acid, base, and conjugates in an acidbase reaction, we wiWm use the folJowing process andbuild 2 toni#gate pairs between reactants and products

• Ask yourself "Which reactant loses an H+?"This is the

.ÿQ'¢'] Its partner in the products (missing an H+)

is the conjugate ÿ-ÿ • Connect with an arrow•

• Ask yourself, "Which reactant gains an H+?"This is the

_ÿ6C fts partner in the products (with its new H+)

is the conjugate ACÿ___ Connect with an arrow.

8 "f0 cincochem.pbworks.com Acid Base

Unit 14 BronstedoLowryTTheor,z of Acids and Bases

3. Remember' Conjugates are always ÿC[ÿCÿ J[3 I

[ %HCI H2LO ÷ HÿO+ CI-

Acÿa ÿ

Practice: Identify the B-L acid, B-L base, conjugate acid, andconjugate base.

r q.HNO3 + H20 H30+ + NO3-

Given an acid or base, to predict the conjugate acid andconjugate base we will use the foRIowing rules,

.

.

Given a B-L acid, to find its conjugate base, take

away one /-4 and lower (subtract -) the charge

by )

Given a B-L base, to find its conjugate acid, add

one ÿ and raise (add to +) the charge by /

+2+l

0-i

-2

Practice:

HI ÷

Give the formula of the conjugate base of thefollowing B-L acids. (doÿqÿ q H4)

-2.

HCO3-1 -ÿ> __ÿ03 ___ H2PO4-*


Bronsted Lowry, Hvdronium, Protons

Practice: Give the formula of: the conjugate acid of thefollowing B-L basesÿ¢ts H.ÿ )

Unit 14

H2P04-'÷ Iqs FOL __ F-l÷ ÿ/ F

Then droniurnion H30+

Hydrogen ions are not always "free" in an acidic solution.

+ The ÿqÿ/ÿFÿqiÿ]ÿqÿq ion forms when an acidI

is dissolved in H20. H20 and H+ can combine to form H30+.

The hydronium ion functions the same as an H+ ion.

}{Cl + }{20 ÿ H30+ + CF

qen ion ÿ'H+) is a pROTON.ÿ

A hydrogen atom contains a single proton and an electron, soafter it loses an electron all that remains is a PROTON.

SO, hydrogen ions (H+) are often referred to as PROTONS.

-A-Acids can be defined by how many H+ they can donate.

Type # of H+ to give Example

onoprohc

TriFohc

qbi froSo 2


Unit 14

Semf-IonJzation of Water

Water can act asa B-L ÿdiÿ era B-L ÿ6ÿ .

In any sample of water, a very small amount of H+ and OH-

ions will form. Thus, equal amounts ofhydronium and

hydroxide ions form, creating conjugate pairs. This is called

the self- I OÿiZQÿLI'ÿ of water:

Self-Ionization of water

H20 H20 -') H30+ OH-

In ÿU r-Pÿ, water, equal concentrations of [H+]

and [OH-] are present at 1 x 10-7 M (0.0000001 M).

NEUTRAL is where [H+] = [OH-] with at molarity of 1 x 10-7 Iv]

Therefore, for any aqueous solution,

[H+] x [OH-] = 1 x 10-14 M

AND...

As [H+] ÿb, [OH-] must 4,

As [OH-] ÿb, [H+] must 4,

This is an }ÿtÿf-3 ¢ relationship

between hydrogen and hydroxide ions. With greater

[H+] you have and acid, with greater [OH-], a base.


H Unit 14

0 1 3 4

I pH Scale5 6 7 8

/ I9 10 11 12 13I I I I I

14

[

Concentration of Ions in Solutions

Aod,o ["+1 ?

pH Scale

[OH-]

[OH-]

[OH-]

basicity.

pH range is from

[H+] are in very_ Iÿbÿ) concentration, so the

pH scale is easier to use to represent acidity and

6 to

Using a calculator, we use the "

JH/ 01 " key to

generate a value for pH we can easily work with.

Remember, [H30÷] = [H÷]


Unit 14

fTo find pH using a TI calculator

Example [H30+] = 3.23 x 10.5 find the -iog[3.23 x 10-5]

key in' E2]I-C0-ÿ[]ÿ][ÿ[ÿIÿ[2-ÿIIÿEÿIÿEÿ thenThis yields a pH of 4.49.

Remember, in a F5ÿ4ÿ/ aqueous solution,

J

[H+] = [OH-] = lx 10-7 M

So... pH = -7

If [H3O+] = 1.0 x 10 -12 M, what is the pH? i2_

Is the solution ÿ NEUTRAL, or ACIDIC?

#4-- -Io9 (,I,0 ÿ10-'ÿ)

If [HsO+] = 1.0 x 10-7 M, what is the pH? 3

Is the solution BASIC,ÿ or ACIDIC?

Practice: 5If [HBO+] = 1.0 X 10-s M, what is the pH?

Is the solution BASIC, NEUTRAL, or

?ÿ -Ioÿ (I,o,,, ÿoÿ-ÿ)

pH is < ÿ7 Solution is AÿOl-cÿio

pH is : -1 Solution is iqCtÿ¢l

pH is } ] Solution is )ÿ.tSIC.


pOH

@ like H÷ ions, OH- ions exist in very

Unit 14

concentrations in aqueous solutions. However, we can find

)0 ÿ to make the numbers easier to work with.

pOH range is also from O to ) Lÿ

pOH is the OPPOSITE of PHr so if..

poll is 4 =7

pOH is - -7

pOH is "ÿ -ÿ

Solution is

Solution is

Solution is

nÿ½/Aciollc

pH and pOH are ALSO i ÿ Cerÿc/v_J

relatedy so..,

pH + pOH = ;#


Unit 14

FindinqjLHÿÿ

Given pH, we can determine

[H+]

£1430ÿ by using the inverse of

the log ofpH! To find [H+], set 10 to the power of the-pH.

fTo convert FROH pH to [H+] using a TI calculator

Example: pH = 9.51. [H30+]=10-9'sl

Key in 2ÿ] LILILÿGÿFZ][ÿ]IÿI-5]IÿIÿThis yields a [H+] of 3.09 x 10 -10

Practice: ÿ1430qj= }O"ÿ'fl

If the pH of a solution is 4.4, what is the [H30+]?

If the pH of a solution is 9.8, what is the [H+]? i

J

pH

4.9

11.2

[H30+]

1,3 xlO"ÿ M

b. 3 x IO°'ZM

Acid/BaseNeutral

¢pOH

q,ÿ

Eÿ4q- l oq'ÿ

q,0ÿ10"5>

, tp ÿ10 °J°i4

Acid Base ÿ0 cincochem,pbworks.com 15

pH and [H+]

pH = -ÿiO3ÿ,ÿ'3 [H+] = I0

pH + pOH = Iff

.o fu/

Unit 14

ZDetermine the pH of a 0.01 H HCI solution

-Io z

Determine the pH of a 0.0010 N H2SO4 solution5

Find [H30+] for a solution that has a pH of 3.1 ___

Find [H30+] for a solution that has a pH of 9.5 3, 2 :x )O-ÿ°fvl

Find [H+] for a solution that has a pH of 8.2 Mÿ ÿ/ÿ)-ÿ//k4

[Hu#ÿ /0 " ÿ,z .-_ 6, ÿaÿx10-ÿ

Find [H30+] for a solution that has a pH of 4.85.


Unit 14

Q; What happens mayou mix an acid with a base?

Neutralization

A: A reaction!

HCI + NaOHLsalÿ

Products are ALWAYS a salt and water (H20)

also known as an

+ mon-mÿ+q /

0R ÿ compound

@

This is called a ÿ CtAÿYa/iÿq'olÿ

When writing the products, write __Xÿ'ÿ(-

reaction.

first, then criss-cross the charges of the metal and

nonmetal to find the formula of the ÿ(4/ÿ

Practice: Write the balanced chemical equation for theneutralization reaction between"

1) nitric acid (HNO3) and potassium hydroxide (KOH) /

HN03 ÿ KoH ÿ 14ÿO # KNO:ÿ

2) sulfuric acid (H2SO4) and magnesium hydroxide(Mg(OH)2)

HÿoI t Iqqo(0t4'ÿ ÿ 2_ S4ÿo/

Neutralization reaction"


Titration

Titration - a process in which a

reaction is used to determine the

Unit 14

of a

solution. ÿconcentration is molarity (IVl)

[ÿAIÿ; Ceÿc. ÿ Acid

x/k: ,4& ÿRc(¢ff4 rUr

n, qolAm

To solve:1; b la ceA chemical equation

2) use acid/base coefficients for "mOIAczD" and "mOIBAsE" values

Example ¢ÿ ÿ ? ÿ jÿ V6How many m L of 0.45 ! HCI must be added to 25.0 mL of1.00 IVl KOH to make a neutral solution?

(ÿ) ÿvÿ

Practice : ? lee xlA ,What is the molarity o]: nitric acid (HNO3ÿ,if 15.0 mL or thesolution is cÿ neutralized by 38.ÿJ mÿC6f6::150 IVlNaOH?. HJÿ0ÿ +ÿ4aON -ÿ ÿ4ÿ.O+ ÿaÿO5 ,

,TA

A 25.0 mL solution of sulfuÿc acid (H2SO4) is completelyneutralized by 18 ÿL of 1.CI R LiOn. What is theconcentration of the H2SO4 solution?


Unit 14

Find pH

To go from [H30+] to pH

EXAMPLE: [H30÷] = 3.23 x 10-s

Take the -log of the [H30÷] concentration

Key in [ÿ[E-O-ÿ[ÿ[ÿ[ÿ][ÿ[ÿ[ÿ[ÿ[ÿ[]. This yields a pH of 4.49.

Using the TI Calculator for p H

Find concentration

To go from pH to [H+]

EXAMPLE: pH = 9.51.

Set 10 to the power of the -pHo

Key in [2ÿ[-Co-ÿD[ÿ[ÿ[ÿ[ÿ[ÿ This yields [H+] of 3.09 x 10-lo

OH

To go from pH to pOH (and vice versa)

EXAMPLE: pH = 4.49

Subtract pH from 14.

This yields a pOH of 9.51.


Periodic Table Unit 14

L ....Lÿ) L

'- °° lÿ? -i:'ÿo ¢D ÿ!t b

oÿ ÿ

nÿ, csÿ r]G

a

i

m

xf

oÿ<ÿ

/}; tH2ÿ

o

o

a)ÿ ÿ

O*] LL it; 2

6,

>

tco :ÿ

¢)E

gÿ. E

<

-rÿ N;!Lÿ

[

b

0 ÿ

J L"tZ oi.ÿ

8 oo r<ÿ i

<o ÿ 9ÿ1<1o 1",1 ,tÿ

...................... 4

oO

8

r-ÿ,ÿ,ÿ <<4 '-I

i

(o 69 (N r! d)

o (lJ c! {: ÿ2

........ ?:: .......I

r) Is,kS) dÿ <

(O

-- {!ÿ

Le

co '<,,<ÿ

t:i

c;ÿ.tlÿ <w e

- !i

bÿ

it) Eu ÿJ a,?'

COl._ ,ÿjJ ÿ ÿ,ÿ

<+o LIJ -:ÿ r>ÿ/7:

. ,ÿ ÿ-" %

t,, {il' O

I0 t=

E

?T [: ÿi

6;7 7,S:ÿ %

L-* { ?'J Lz

Ocxl l--

tO (f)¢0 O)

(ÿoo coC0 (9j TD

20 ÿ-0 cincochem.pbworks.com Acid Base

academic chemistry acids & bases - pbworks - acid... · academic chemistry ids & bases...

Documents