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Acids and bases irp notes, Lecture notes of Applied Chemistry

Monash University, Malaysia CampusApplied Chemistry

Chemistry notes about acid and bases

Typology: Lecture notes

2015/2016

Uploaded on 10/19/2016

farah.zaini
farah.zaini 🇲🇾

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ACIDS AND BASES
Bronsted-Lowry
Acid = H+ donor
Base = H+
acceptor
Eg : HCl + NH3 Cl- +NH4+
Lewis
ACid = e- pair ACceptor
Base = e- pair donor
A dative covalent bond is formed in Lewis acid-
base reaction.
*Conjugate acid-base pairs differ by one proton
AMPHIPROTIC
Substances which can act as Bronsted-Lowry
acids and bases (both a proton donor and a proton
acceptor)
Must have possessed both a lone pair of e- and
hydrogen that can be released as H+
PROPERTIES OF ACIDS AND BASES
- reactions of acids and bases
1. Acids + metals (more reactive than H)
Metal + acid → salt + hydrogen
2. Acids + carbonates/hydrogencarbonates
Acid + CO32-
/HCO3 → salt + CO2 + H2O
3. Acids + bases/alkalis
Base + acid → salt + H2O
pH scale
Measuring pH
Def: pH is the –ve logarithm to base 10 of the
hydrogen ion concentration in an aqueous
solution.
pH= -log10[H+(aq)] // pOH= -log10 [OH-]
[H+]= 10-pH
Kw= [H+] [OH-]
Kw= 1.0 x 10-14 at 298k (std temp in K)
Kw= H2O(l) H+(aq)+OH-(aq)
STRONG AND WEAK ACIDS AND BASES
STRONG
WEAK
Kw= ionic
product
constant for
WATER !!
• Conduct electricity better
than weaker acids.
• React more violently with
metals/ carbonates.
• Have LOWER pH than weak
acids
Acids = dissociate completely to form H+
Bases = ionize completely to form OH-
Acids = dissociate partially to form H+
STRONGER acid, WEAKER conjugate base
STRONGER base, WEAKER conjugate acid
Bases = ionize partially to form OH-
pf3
pf4

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ACIDS AND BASES

Bronsted-Lowry

Acid = H +^ donor

Base = H+ acceptor

Eg : HCl + NH 3 Cl-^ +NH 4 +

Lewis

ACid = e- pair ACceptor

Base = e- pair donor

A dative covalent bond is formed in Lewis acid- base reaction.

  • Conjugate acid-base pairs differ by one proton

AMPHIPROTIC

Substances which can act as Bronsted-Lowry acids and bases (both a proton donor and a proton acceptor)

Must have possessed both a lone pair of e- and hydrogen that can be released as H+

PROPERTIES OF ACIDS AND BASES

- reactions of acids and bases 1. Acids + metals (more reactive than H)

Metal + acid → salt + hydrogen

  1. Acids + carbonates/hydrogencarbonates

Acid + CO 3 2-/HCO 3 → salt + CO 2 + H 2 O

  1. Acids + bases/alkalis

Base + acid → salt + H 2 O

pH scale

Measuring pH

Def: pH is the –ve logarithm to base 10 of the hydrogen ion concentration in an aqueous solution.

pH= -log10[H+^ (aq)] // pOH= -log 10 [OH - ]

[H +^ ]= 10 -pH

Kw= [H+^ ] [OH - ]

Kw= 1.0 x 10-14^ at 298k (std temp in K)

Kw= H 2 O(l)^ H^ +^ (aq)+OH^ - (aq)

STRONG AND WEAK ACIDS AND BASES

STRONG

WEAK

Kw= ionic product constant for WATER !!

  • Conduct electricity better than weaker acids.
  • React more violently with metals/ carbonates.
  • Have LOWER pH than weak acids

Acids = dissociate completely to form HBases = ionize completely to form OHAcids = dissociate partially to form HSTRONGER acid, WEAKER conjugate base+ - +

STRONGER base, WEAKER conjugate acid

Bases = ionize partially to form OH -

_________________

_________________

_____

ACID DEPOSITION

Def : The process where acidic particles, gases and precipitation leave the atmosphere.

  • Rain water is acidic, pH 5.6 because of it is the product of CO 2 and H 2 O.

Forming the weak acid, carbonic acid and can be ionized to form H+ and HCO 3 - :

  • Acid rain = below pH 5.
  • Acid deposition contains oxides of sulfur and nitrogen.
  • Two types of acid deposition :

SULFUR OXIDES

  • Produced from burning of fossil fuels/ coal/heavy oil in power plants used to generate electricity.

_______________________________________

a colorless gas with a sharp smell dissolves in H2O to form H2SO3:

SO2 then oxidized to SO3 and dissolves in water to form H2SO4:

NITROGEN OXIDES

NO produced from internal combustion engines, where the burning of the fuel releases heat energy that causes N and O from air to combine.

  • NO2 forms from:

• N 2 (g) + 2O 2 (g) → 2NO 2 (g)

• 2NO(g) + O 2 (g) → 2NO 2 (g)

  • NO2 dissolves in H2O to form HNO2 and HNO3:
  • NO2 can also be oxidized to form nitric acid:

2H 2O(l) + 4NO2(g) + O 2(g) → 4HNO3(aq)

  • Main components of acid rain :-

Wet deposition – rain, snow, hail, fog, etc.

Dry deposition – acidic gas, particles