P&P notes Chapter 8 【Salts】
Wednesday, July 13, 2011
CHAPTER 8 : SALTS
7.1 SALTS
1. What is salt ?
It’s a ___________ compound which formed when the _______________ ________ from acid is replaced by a metal ion or ammonium ion.
Example: NaOH + HCl --> NaCl + H2O
2. Some of the salts are soluble and some are insoluble.
Salts Soluble √ Insoluble X
Sodium salts
Na+ • All soluble ------
Pottasium salts
K+ • All soluble ------
Ammonium salts
NH4+ • All soluble ------
Nitrate salts
NO3- • All soluble ------
Carbonate salts
CO32- • Sodium carbonate, Na2CO3
• Potassium carbonate,
K2CO3
• Ammonium carbonate,
(NH4)2CO3
• All other carbonate salts insoluble
Chloride salts
Cl- • All chloride salts • Lead(II) chloride, PbCl2
• Silver chloride, AgCl
Sulphates salts
SO42- • All chloride salts • Lead (II) sulphate, PbSO4
• Calcium sulphate, CaSO4
• Barium Sulphate, BaSO4
Ions Soluble √ Insoluble X
Oxide
O2- • Only Sodium oxide, Pottasium oxide,
Ammonium oxide soluble • All others insoluble
Hydroxide
OH- • Only Sodium hydroxide, Pottasium hydroxide,
Ammonium hydroxide soluble • All others insoluble
* try to determine the salts whether its soluble @ insoluble
1. Sodium hydroxide
2. Magnesium hydroxide
3. Barium nitrate
4. Copper (II) chloride
5. Ammonium sulphate
7. Lead (II) nitrate
8. Zinc sulphate
9. Copper (II) sulphate
10.Pottasium carbonate
11.Aluminium oxide
6. Lead (II) chloride 12.Silver sulphate
Group 1: Soluble salts of Na+ , K+ & NH4+
Group 2: Soluble salts which not Na+ , K+ & NH4+
Group 3: Insoluble salts
7.2 THE PREPARATION OF SOLUBLE SALTS OF GROUP 1
acid (aq) + alkali (aq) (neutralisation)
-recrystallisation can be done by repeating:
- recrystallisation repeated to get the ___________ salt.
7.3 THE PREPARATION OF SOLUBLE SALTS OF GROUP 2
1. acid (aq) + base (s)
2. acid (aq) + metal (s) ( x Cu & Ag)
3. acid (aq) + metal oxide (s)
4. acid (aq) + metal carbonate (s)
7.4 THE PREPARATION OF INSOLUBLE SALTS OF GROUP 3
1. soluble salt solution ( cation) + soluble salt solution ( anion)
7.5 NUMERICAL PROBLEM SOLVING
Step 1 : Write balance equation
Step 2 : Find No. of mole of substance which given info
Step 3 : Compare No. of mole
Step 4 : Get answer
* Exercises
7.6 QUALITATIVE ANALYSIS OF SALTS
Qualitative analysis – a chemical technique to determine what substances are present in a mixture but not their quantities.
Aim: To find out types of cation & anion which present.
Observation on the physical properties:
1. colour
2. solubility in water
3. test of produced gases
4. action of heat on salts
5. test for anions
6. test for cations
1.Colour
Cations in aq Colour Anion in aq Colour Solid salt Colour
Fe2+ Pale green NO3- colourless Fe2+ salts Green
Fe3+ Brown SO42- colourless Fe3+ salts Brown
Cu2+ Blue Cl- colourless Iron (III) Oxide Reddish Brown
Other colourless CO32- colourless Zinc Oxide Yellow –hot
White - cold
Lead (II) Oxide Brown – hot
Yellow - cold
Copper (II) Oxide Black
Cu2+ salts Blue
Other salts White
2. Solubility in Water
** refer to the table 7.1 (2)
3. Test of Produced Gases
Method of Tests Observation Acidic / Alkaline Gases
• tested by glowing splinter • • neutral O2
• tested by wooden splinter • • Little acidic H2
• gas bubbled through lime water • • Little acidic CO2
• Moist red litmus paper
• Tested by a drop of concentrated HCl • Red litmus paper turns blue
• Dense white fume formed • alkaline NH3
• Moist red / blue litmus paper • blue litmus paper turns red• • Little acidic Cl2
• Moist blue litmus paper
• Tested by a drop of concentrated NH3 • blue litmus paper turns red
• produce • acidic HCl
• Moist blue litmus paper
• Tested by a drop of acidified potassium manganate (VII) solution
• Tested by a drop of acidified potassium dichromate (VI) solution • blue litmus paper turns red
• decolourises the purple colour
• turns colour from orange to green • acidic SO2
• Moist blue litmus paper • Brown gas • acidic NO2
4. Action of Heat on Salts
Carbonate Salts Action of Heat Nitrate Salts Action of Heat
K2CO3
Na2CO3
Not decomposed by heat KNO3 NaNO3 2KNO3 2KNO2 + O2
CaCO3
MgCO3
Al2(CO3)3
ZnCO3
FeCO3
PbCO3
CuCO3 CaCO3 CaO + CO2 Ca(NO3)2
Mg(NO3)2
Al(NO3)3
Zn(NO3)2
Fe(NO3)2
Pb(NO3)2
Cu(NO3)2
Ag2CO3
AgNO3
(NH4)2CO3 NH4NO3
- most the sulphate salts are not decomposes by heat, only a few sulphate salts decompose when heated strongly
- all the chloride salts are not decomposes by heat, except ammonium chloride
NH4Cl (s) NH3 (g) + HCl (g)
5. Test of Anions ( -ve)
Anions Method
CO32- + 2 cm3 dilute HCl
Tested by lime water
-
SO42- + >>> dilute HCl
+ BaCl2 & shaked
-
Cl- + >>> dilute HNO3
+ AgNO3 & shaken well
-
+ NH3 & shaken well
-
NO3- + 2 cm3 dilute H2SO4
+ 2 cm3 FeSO4 & shaken well
+ Few drops of concentrated sulphuric acid dropped slowly along the side of a slanting test tube without shaking
-
7. Test of Cations
* refer to pg. 232 and complete the chart below
Add few drops of NaOH
7.1 SALTS
1. What is salt ?
It’s a ___________ compound which formed when the _______________ ________ from acid is replaced by a metal ion or ammonium ion.
Example: NaOH + HCl --> NaCl + H2O
2. Some of the salts are soluble and some are insoluble.
Salts Soluble √ Insoluble X
Sodium salts
Na+ • All soluble ------
Pottasium salts
K+ • All soluble ------
Ammonium salts
NH4+ • All soluble ------
Nitrate salts
NO3- • All soluble ------
Carbonate salts
CO32- • Sodium carbonate, Na2CO3
• Potassium carbonate,
K2CO3
• Ammonium carbonate,
(NH4)2CO3
• All other carbonate salts insoluble
Chloride salts
Cl- • All chloride salts • Lead(II) chloride, PbCl2
• Silver chloride, AgCl
Sulphates salts
SO42- • All chloride salts • Lead (II) sulphate, PbSO4
• Calcium sulphate, CaSO4
• Barium Sulphate, BaSO4
Ions Soluble √ Insoluble X
Oxide
O2- • Only Sodium oxide, Pottasium oxide,
Ammonium oxide soluble • All others insoluble
Hydroxide
OH- • Only Sodium hydroxide, Pottasium hydroxide,
Ammonium hydroxide soluble • All others insoluble
* try to determine the salts whether its soluble @ insoluble
1. Sodium hydroxide
2. Magnesium hydroxide
3. Barium nitrate
4. Copper (II) chloride
5. Ammonium sulphate
7. Lead (II) nitrate
8. Zinc sulphate
9. Copper (II) sulphate
10.Pottasium carbonate
11.Aluminium oxide
6. Lead (II) chloride 12.Silver sulphate
Group 1: Soluble salts of Na+ , K+ & NH4+
Group 2: Soluble salts which not Na+ , K+ & NH4+
Group 3: Insoluble salts
7.2 THE PREPARATION OF SOLUBLE SALTS OF GROUP 1
acid (aq) + alkali (aq) (neutralisation)
-recrystallisation can be done by repeating:
- recrystallisation repeated to get the ___________ salt.
7.3 THE PREPARATION OF SOLUBLE SALTS OF GROUP 2
1. acid (aq) + base (s)
2. acid (aq) + metal (s) ( x Cu & Ag)
3. acid (aq) + metal oxide (s)
4. acid (aq) + metal carbonate (s)
7.4 THE PREPARATION OF INSOLUBLE SALTS OF GROUP 3
1. soluble salt solution ( cation) + soluble salt solution ( anion)
7.5 NUMERICAL PROBLEM SOLVING
Step 1 : Write balance equation
Step 2 : Find No. of mole of substance which given info
Step 3 : Compare No. of mole
Step 4 : Get answer
* Exercises
7.6 QUALITATIVE ANALYSIS OF SALTS
Qualitative analysis – a chemical technique to determine what substances are present in a mixture but not their quantities.
Aim: To find out types of cation & anion which present.
Observation on the physical properties:
1. colour
2. solubility in water
3. test of produced gases
4. action of heat on salts
5. test for anions
6. test for cations
1.Colour
Cations in aq Colour Anion in aq Colour Solid salt Colour
Fe2+ Pale green NO3- colourless Fe2+ salts Green
Fe3+ Brown SO42- colourless Fe3+ salts Brown
Cu2+ Blue Cl- colourless Iron (III) Oxide Reddish Brown
Other colourless CO32- colourless Zinc Oxide Yellow –hot
White - cold
Lead (II) Oxide Brown – hot
Yellow - cold
Copper (II) Oxide Black
Cu2+ salts Blue
Other salts White
2. Solubility in Water
** refer to the table 7.1 (2)
3. Test of Produced Gases
Method of Tests Observation Acidic / Alkaline Gases
• tested by glowing splinter • • neutral O2
• tested by wooden splinter • • Little acidic H2
• gas bubbled through lime water • • Little acidic CO2
• Moist red litmus paper
• Tested by a drop of concentrated HCl • Red litmus paper turns blue
• Dense white fume formed • alkaline NH3
• Moist red / blue litmus paper • blue litmus paper turns red• • Little acidic Cl2
• Moist blue litmus paper
• Tested by a drop of concentrated NH3 • blue litmus paper turns red
• produce • acidic HCl
• Moist blue litmus paper
• Tested by a drop of acidified potassium manganate (VII) solution
• Tested by a drop of acidified potassium dichromate (VI) solution • blue litmus paper turns red
• decolourises the purple colour
• turns colour from orange to green • acidic SO2
• Moist blue litmus paper • Brown gas • acidic NO2
4. Action of Heat on Salts
Carbonate Salts Action of Heat Nitrate Salts Action of Heat
K2CO3
Na2CO3
Not decomposed by heat KNO3 NaNO3 2KNO3 2KNO2 + O2
CaCO3
MgCO3
Al2(CO3)3
ZnCO3
FeCO3
PbCO3
CuCO3 CaCO3 CaO + CO2 Ca(NO3)2
Mg(NO3)2
Al(NO3)3
Zn(NO3)2
Fe(NO3)2
Pb(NO3)2
Cu(NO3)2
Ag2CO3
AgNO3
(NH4)2CO3 NH4NO3
- most the sulphate salts are not decomposes by heat, only a few sulphate salts decompose when heated strongly
- all the chloride salts are not decomposes by heat, except ammonium chloride
NH4Cl (s) NH3 (g) + HCl (g)
5. Test of Anions ( -ve)
Anions Method
CO32- + 2 cm3 dilute HCl
Tested by lime water
-
SO42- + >>> dilute HCl
+ BaCl2 & shaked
-
Cl- + >>> dilute HNO3
+ AgNO3 & shaken well
-
+ NH3 & shaken well
-
NO3- + 2 cm3 dilute H2SO4
+ 2 cm3 FeSO4 & shaken well
+ Few drops of concentrated sulphuric acid dropped slowly along the side of a slanting test tube without shaking
-
7. Test of Cations
* refer to pg. 232 and complete the chart below
Add few drops of NaOH
P&P notes Chapter 7 【acids & bases】
CHAPTER 7 : ACID AND BASE
7.1 ACIDS & BASES
A. Acids
1. What is acids ?
A chemical substances which _______________ in water to produce __________________ _____ .
Example: HCl H+ + Cl-
2. The _________________ are responsible for acids to show their properties.
3. Acids classified as ____________ acid (produce I mole of H+) &
____________ acid (produce 2 mole of H+), base on its bacidity.
Example: HNO3 H+ + NO3- (monoprotic acid)
H2SO4 2 H+ + SO42- (diprotic acid)
4. Bacidity : The number of ______________ hydrogen atoms per molecule of an acid.
B. Bases
1. What is bases ?
A chemical substances which _______________ in water to produce__________________ _____ .
Example: NaOH Na+ + OH-
2. Base reacts with acid to form a _______ and _______ only.
Example: NaOH + HNO3 NaNO3 + H2O
3. The _________________ are responsible for alkalis to show their properties.
4. Difference of bases & alkalis :
- some bases can dissolves in water
- soluble bases are known as __________.
C. Role of Water
- acids & bases only show their properties when __________ in water
- because without water, acids & bases still exist as ___________ and no H+ @ OH- ions present.
- but in water, acids & bases __________ to form H+ @ OH- ions.
D. Indicators
- gives colour depend on the pH of the solution
- could be in solid form or liquid form
INDICATORS ACIDIC NEUTRAL ALKALINE
Litmus paper Red - Blue
Universal indicator Green Green Blue
Methyl orange Red Orange Yellow
Phenolphthalein Colorless Colorless pink
E. Physical Properties
ACIDS PROPERTIES ALKALIS
Taste
Turn moist litmus paper
Ph value
F. Chemical Properties
1. react with bases to form ___________ and ___________.
2. react with reactive metal to form ___________ and _______________.
3. react with carbonates to form ____________, _____________ and _____________________.
Examples:
1. HCl + KOH
2. HCl + Mg
H2SO4 + Pb
3. HCl + MgCO3
HNO3 + ZnCO3
1. react with acids to form ___________ and ___________.
2. mix with ammonium salt and heated, ____________ liberated.
3. adding to most of the metal ion solution, a to form _______________.
Reason: most of the metal hydroxide are insoluble in water.
Examples:
1. HCl + NaOH
2. NH4Cl + Ca(OH)2 ∆
7.2 THE STRENGTH OF ACIDS & BASES
Strong acids Strong alkalis
Acidic increasing Neutral Alkaline increasing
** Why strong acids has lower pH & strong alkalis has higher pH ??
Strong Acids Weak Acids
- Ionises completely in water - ionises partial in water
- Large numbers of H+ ions - few of numbers of H+
- [H+ ] high - [ H+ ] low
- pH value - pH value
**********************************************************************
Strong Alkalis Weak Alkalis
- ionises in water - ionises in water
- large numbers of H+ ions - few of numbers of H+
- [ OH- ] high - [ OH- ] low
- pH value - pH value
7.3 CONCENTRATION OF ACIDS AND ALKALIS
1. Molarity - the amount of dissolved substance in 1dm-3 of solvent to form a solution.
2. Unit - ________________ / _________¬¬¬¬¬¬¬¬¬¬________
1 dm-3 = 1000 cm-3
3. the molarity of a solution does not determine whether it is strong @ weak acid
4. No. of moles = M V ; M = molarity ; V = volume
1000
* exersicises
5. Preparation of Standard Solution
- a solution which has a _________________________________.
- prepared by ________________________.
* exersicises
6. Dilution
- prepare a less concentrated solution
M1V1 = M2V2 M1 = initial molarity ; V1 = initial volume
M2 = final molarity ; V2 = final volume
* exersicises
7. Molarity Vs pH value
Molarity / Concentration [ H+] in acids pH
[ OH-] in alkalis pH
7.4 NEUTRALISATIONS
1. the reaction between _________ and __________ to produce salt & water.
2. H+ from acids combine with OH- from alkalis to form water molecules.
H+ + OH- H2O
3. Acid – Bases Titration
- a quantitative analysis methode to determine the volume of an acid to neutralise an alkali
-
4. End Point – point which neutralization done completely.
5. End point can be determined by : indicators / electrical conductivity
7.1 ACIDS & BASES
A. Acids
1. What is acids ?
A chemical substances which _______________ in water to produce __________________ _____ .
Example: HCl H+ + Cl-
2. The _________________ are responsible for acids to show their properties.
3. Acids classified as ____________ acid (produce I mole of H+) &
____________ acid (produce 2 mole of H+), base on its bacidity.
Example: HNO3 H+ + NO3- (monoprotic acid)
H2SO4 2 H+ + SO42- (diprotic acid)
4. Bacidity : The number of ______________ hydrogen atoms per molecule of an acid.
B. Bases
1. What is bases ?
A chemical substances which _______________ in water to produce__________________ _____ .
Example: NaOH Na+ + OH-
2. Base reacts with acid to form a _______ and _______ only.
Example: NaOH + HNO3 NaNO3 + H2O
3. The _________________ are responsible for alkalis to show their properties.
4. Difference of bases & alkalis :
- some bases can dissolves in water
- soluble bases are known as __________.
C. Role of Water
- acids & bases only show their properties when __________ in water
- because without water, acids & bases still exist as ___________ and no H+ @ OH- ions present.
- but in water, acids & bases __________ to form H+ @ OH- ions.
D. Indicators
- gives colour depend on the pH of the solution
- could be in solid form or liquid form
INDICATORS ACIDIC NEUTRAL ALKALINE
Litmus paper Red - Blue
Universal indicator Green Green Blue
Methyl orange Red Orange Yellow
Phenolphthalein Colorless Colorless pink
E. Physical Properties
ACIDS PROPERTIES ALKALIS
Taste
Turn moist litmus paper
Ph value
F. Chemical Properties
1. react with bases to form ___________ and ___________.
2. react with reactive metal to form ___________ and _______________.
3. react with carbonates to form ____________, _____________ and _____________________.
Examples:
1. HCl + KOH
2. HCl + Mg
H2SO4 + Pb
3. HCl + MgCO3
HNO3 + ZnCO3
1. react with acids to form ___________ and ___________.
2. mix with ammonium salt and heated, ____________ liberated.
3. adding to most of the metal ion solution, a to form _______________.
Reason: most of the metal hydroxide are insoluble in water.
Examples:
1. HCl + NaOH
2. NH4Cl + Ca(OH)2 ∆
7.2 THE STRENGTH OF ACIDS & BASES
Strong acids Strong alkalis
Acidic increasing Neutral Alkaline increasing
** Why strong acids has lower pH & strong alkalis has higher pH ??
Strong Acids Weak Acids
- Ionises completely in water - ionises partial in water
- Large numbers of H+ ions - few of numbers of H+
- [H+ ] high - [ H+ ] low
- pH value - pH value
**********************************************************************
Strong Alkalis Weak Alkalis
- ionises in water - ionises in water
- large numbers of H+ ions - few of numbers of H+
- [ OH- ] high - [ OH- ] low
- pH value - pH value
7.3 CONCENTRATION OF ACIDS AND ALKALIS
1. Molarity - the amount of dissolved substance in 1dm-3 of solvent to form a solution.
2. Unit - ________________ / _________¬¬¬¬¬¬¬¬¬¬________
1 dm-3 = 1000 cm-3
3. the molarity of a solution does not determine whether it is strong @ weak acid
4. No. of moles = M V ; M = molarity ; V = volume
1000
* exersicises
5. Preparation of Standard Solution
- a solution which has a _________________________________.
- prepared by ________________________.
* exersicises
6. Dilution
- prepare a less concentrated solution
M1V1 = M2V2 M1 = initial molarity ; V1 = initial volume
M2 = final molarity ; V2 = final volume
* exersicises
7. Molarity Vs pH value
Molarity / Concentration [ H+] in acids pH
[ OH-] in alkalis pH
7.4 NEUTRALISATIONS
1. the reaction between _________ and __________ to produce salt & water.
2. H+ from acids combine with OH- from alkalis to form water molecules.
H+ + OH- H2O
3. Acid – Bases Titration
- a quantitative analysis methode to determine the volume of an acid to neutralise an alkali
-
4. End Point – point which neutralization done completely.
5. End point can be determined by : indicators / electrical conductivity
Exercise on calculation of number of moles
NUMBER OF MOLES
1. Hiow many times two titanium atoms heavier than three oxygen atoms?
2. P, Q, and R are three elements. Relative atomic mass for R is 210. One R atom is three times heavier than one Q atom and one Q atom is two times heavier than one P atom. Determine the relative atomic mass for element P.
3. Determine the relative molecular mass for the compounds below:
a) methane, CH4 b) ethanol, C2H5OH
c) glucose, C6H12O6 d) sodium sulphate, Na2SO4
e) sodium thiosulphate hydrated, Na2S2O3.5H2O
f) cobalt chloride hydrated, CoCl2.6H2O
g) ammonium carbonate, (NH4)CO3
h) aluminium sulphate, Al2 (SO4)3 i) oxygen gas
NUMBER OF MOLES Vs NO. OF PARTICLES
1. Calculate the number of particles:
a) 0.22 mole of nitrogen dioxide, NO2
b) 2.75 mole of zinc ions, Zn2+
c) 0.5 mole of ammonium chloride, NH4Cl
d) 0.2 mole of bromine gas
2. Calculate the number of mole for the following subtances:
a) 7.224 x 1022 carbon atoms, C
b) 1.204 x 1024 oxygen gas
c) 9.632 x 1023 sulfur dioxide, SO2
d) 4.515 x 1024 ammonia gas, NH3
NUMBER OF MOLES Vs MASS (g)
1. Find out the mass of:
a) 2/5 moles of zinc, Zn
b) 0.025 mole of sulfur dioxide, SO2
c) 1.75 moles of oxygen gas
d) 2 moles of chlorine gas
2. Calculate the number of mole of:
a) 1.4 g of Iron, Fe
b) 7.2 g of glucose, C6H12O6
c) 2.4 g of hydrogen gas
3. Calculate the number of particles of:
a) 1.3 g of zinc, Zn
b) 6.9 g nitrogen dioxide, NO2
c) 38.5 g carbon tetrachloride, CCl4
d) 132 g ozon, O3
e) 7.1 g chlorine
4. Determine the subtances mass:
a) 3.01 x 1023 iron atoms, Fe
b) 1.806 x 1024 hydrogen atoms
c) i) 1.505 x 1023 urene molecules, CO(NH2)2
ii) N dlm CO(NH2)2
iii)peratus N dlm sebatian CO(NH2)2
d) 2.709 x 1022 oxygen molecules
NUMBER OF MOLES Vs MOLAR VOLUME
1. Find out the volume of gas at S.T.P. condition:
a) 0.7 g of nitrogen gas
b) 5.4 x 1022 nitrogen dioxide molecules, NO2
c) 1.4 g of carbon monoxide, CO
2. Calculate the number of molecules of the following subtances at room condition:
a) 120 cm3 of methane gas, CH4
b) 4 dm3 of ammonia gas, NH3
c) 36 dm3 of sulfur trioxide, SO3
3. Determine the mass of gas at S.T.P. condition:
a) 3.36 dm3 of ozone gas,O3
b) 448 cm3 of fluorine gas, F2
c) 1.12 cm3 of ethane gas, C2H6
CHEMICAL FORMULAE
Combine the ions below to form the compound and write their names.
1. Ca2+ + SO42+
2. Al3+ + NO3-
3 Na+ + F-
4. Fe3+ + Cl-
5. Mg2+ + O2-
6. Cu2+ + CO32-
7. Pb2+ + Cl -
8. K+ + Cr2O42-
9. K+ + MnO4-
10. Zn2+ + SO42-
EMPIRICAL FORMULAE
1. 6.1 g of metal X combined with m gram of oxygen to form an oxide with formulaX2O5. Determine the value m.
2. 1.5 g of a hydrocarbon compound contains 0.3 g of hydrogen. If the relative molecular mass for the hydrocarbon compound is 30, calculate its:
i) empirical formulae
ii) molecular formulae for the hydrocarbon compound.
3. A hydrocarbon X contains 80% of caarbon and 20% of hydrogen. 1.5 g of the hydrocarbon occupies the volume of 1.12 dm3 at S.T.P. condition. i) Find the emperical formulae of hydrocarbon X.
ii) Find the relative molecular mass for hydrocarbon X.
iii) Determine the molecular formulae for hydrocarbon X.
Combustion of X in athe air produces carbon dioxide and water.
i) write the balance chemical equation.
ii) calculate the volume of carbon dioxide gas liberated.
v) Calculate the mass of water prodiced if 0.6 g of hydrocarbon X has burnt completely in air.
CHEMICAL EQUATIONS
1. Balance the following equation:
a) N2 + (g) H2 (g) NH3 (g)
b) C2H5OH (ce) + O2 CO2 (g) + H2O (ce)
c) MnO2 (p) + HCl (ak) MnCl (ak) + Cl2 (g) + H2O (ce)
d) Na2CO3 (ak) + HNO3 (ak) NaNO3 (ak) + CO2 (g) + H2O (ce)
e) C4H10 (g) + O2 (g) CO2 (g) + H2O (ce)
[NA= 6.02 x 1023 zarah]
[1 mol gas = 22.4 dm3] pd. s.t.p.
[1 mol gas = 24 dm3] pd. suhu / keadaan bilik
[H=1 ; C=12 ; N=14 ; O=16 ; F=19 ; Na=23 ; Al=27 ;
S=32 ; Cl=35.5 ; Ti=48 ; Fe=56 ; Co=59 ; Zn=65 ; Br=80]
1. Hiow many times two titanium atoms heavier than three oxygen atoms?
2. P, Q, and R are three elements. Relative atomic mass for R is 210. One R atom is three times heavier than one Q atom and one Q atom is two times heavier than one P atom. Determine the relative atomic mass for element P.
3. Determine the relative molecular mass for the compounds below:
a) methane, CH4 b) ethanol, C2H5OH
c) glucose, C6H12O6 d) sodium sulphate, Na2SO4
e) sodium thiosulphate hydrated, Na2S2O3.5H2O
f) cobalt chloride hydrated, CoCl2.6H2O
g) ammonium carbonate, (NH4)CO3
h) aluminium sulphate, Al2 (SO4)3 i) oxygen gas
NUMBER OF MOLES Vs NO. OF PARTICLES
1. Calculate the number of particles:
a) 0.22 mole of nitrogen dioxide, NO2
b) 2.75 mole of zinc ions, Zn2+
c) 0.5 mole of ammonium chloride, NH4Cl
d) 0.2 mole of bromine gas
2. Calculate the number of mole for the following subtances:
a) 7.224 x 1022 carbon atoms, C
b) 1.204 x 1024 oxygen gas
c) 9.632 x 1023 sulfur dioxide, SO2
d) 4.515 x 1024 ammonia gas, NH3
NUMBER OF MOLES Vs MASS (g)
1. Find out the mass of:
a) 2/5 moles of zinc, Zn
b) 0.025 mole of sulfur dioxide, SO2
c) 1.75 moles of oxygen gas
d) 2 moles of chlorine gas
2. Calculate the number of mole of:
a) 1.4 g of Iron, Fe
b) 7.2 g of glucose, C6H12O6
c) 2.4 g of hydrogen gas
3. Calculate the number of particles of:
a) 1.3 g of zinc, Zn
b) 6.9 g nitrogen dioxide, NO2
c) 38.5 g carbon tetrachloride, CCl4
d) 132 g ozon, O3
e) 7.1 g chlorine
4. Determine the subtances mass:
a) 3.01 x 1023 iron atoms, Fe
b) 1.806 x 1024 hydrogen atoms
c) i) 1.505 x 1023 urene molecules, CO(NH2)2
ii) N dlm CO(NH2)2
iii)peratus N dlm sebatian CO(NH2)2
d) 2.709 x 1022 oxygen molecules
NUMBER OF MOLES Vs MOLAR VOLUME
1. Find out the volume of gas at S.T.P. condition:
a) 0.7 g of nitrogen gas
b) 5.4 x 1022 nitrogen dioxide molecules, NO2
c) 1.4 g of carbon monoxide, CO
2. Calculate the number of molecules of the following subtances at room condition:
a) 120 cm3 of methane gas, CH4
b) 4 dm3 of ammonia gas, NH3
c) 36 dm3 of sulfur trioxide, SO3
3. Determine the mass of gas at S.T.P. condition:
a) 3.36 dm3 of ozone gas,O3
b) 448 cm3 of fluorine gas, F2
c) 1.12 cm3 of ethane gas, C2H6
CHEMICAL FORMULAE
Combine the ions below to form the compound and write their names.
1. Ca2+ + SO42+
2. Al3+ + NO3-
3 Na+ + F-
4. Fe3+ + Cl-
5. Mg2+ + O2-
6. Cu2+ + CO32-
7. Pb2+ + Cl -
8. K+ + Cr2O42-
9. K+ + MnO4-
10. Zn2+ + SO42-
EMPIRICAL FORMULAE
1. 6.1 g of metal X combined with m gram of oxygen to form an oxide with formulaX2O5. Determine the value m.
2. 1.5 g of a hydrocarbon compound contains 0.3 g of hydrogen. If the relative molecular mass for the hydrocarbon compound is 30, calculate its:
i) empirical formulae
ii) molecular formulae for the hydrocarbon compound.
3. A hydrocarbon X contains 80% of caarbon and 20% of hydrogen. 1.5 g of the hydrocarbon occupies the volume of 1.12 dm3 at S.T.P. condition. i) Find the emperical formulae of hydrocarbon X.
ii) Find the relative molecular mass for hydrocarbon X.
iii) Determine the molecular formulae for hydrocarbon X.
Combustion of X in athe air produces carbon dioxide and water.
i) write the balance chemical equation.
ii) calculate the volume of carbon dioxide gas liberated.
v) Calculate the mass of water prodiced if 0.6 g of hydrocarbon X has burnt completely in air.
CHEMICAL EQUATIONS
1. Balance the following equation:
a) N2 + (g) H2 (g) NH3 (g)
b) C2H5OH (ce) + O2 CO2 (g) + H2O (ce)
c) MnO2 (p) + HCl (ak) MnCl (ak) + Cl2 (g) + H2O (ce)
d) Na2CO3 (ak) + HNO3 (ak) NaNO3 (ak) + CO2 (g) + H2O (ce)
e) C4H10 (g) + O2 (g) CO2 (g) + H2O (ce)
[NA= 6.02 x 1023 zarah]
[1 mol gas = 22.4 dm3] pd. s.t.p.
[1 mol gas = 24 dm3] pd. suhu / keadaan bilik
[H=1 ; C=12 ; N=14 ; O=16 ; F=19 ; Na=23 ; Al=27 ;
S=32 ; Cl=35.5 ; Ti=48 ; Fe=56 ; Co=59 ; Zn=65 ; Br=80]
Notes :F4 Chem Chapter 1 [INTRODUCTION TO CHEMISTRY]
What is chemistry ?
CHEMISTRY is the study of the composition, structure, properties and interactions of matter.
What career related with chemistry ?
• Biochemist
• Chemical engineer
• Cosmetic scientist
• Doctor
• Food technology
• Pharmacist
• Etc.
Scientific Method
- a systematic method used to solve problems in science
- observation - inference (smart guess) - identify problem
- hypothesis - identify variables - controlling variables
- planning an experiment
- collecting data (measurements in table or observation in sentence) - interpreting data (calculation / graphs or chart) - conclusion - write report
Laboratory experiment report
• Problem : occurring question
• Hypothesis : make a general statement
• Manipulated variable : which changes in experiment but determined by yourself
• Responding variable : which changes in experiment and it’s data or observation of experiment
• Constant variables : which constant and no changes during experiment
• Apparatus : instrument used
• Materials : chemical used (quantity)
• Procedure : passive sentences
• Data : table @ sentences
• Interpreting data / Discussion : why I get such a data ? chemistry equation, explanations
• Conclusion : hypothesis accepted rejected
CHEMISTRY is the study of the composition, structure, properties and interactions of matter.
What career related with chemistry ?
• Biochemist
• Chemical engineer
• Cosmetic scientist
• Doctor
• Food technology
• Pharmacist
• Etc.
Scientific Method
- a systematic method used to solve problems in science
- observation - inference (smart guess) - identify problem
- hypothesis - identify variables - controlling variables
- planning an experiment
- collecting data (measurements in table or observation in sentence) - interpreting data (calculation / graphs or chart) - conclusion - write report
Laboratory experiment report
• Problem : occurring question
• Hypothesis : make a general statement
• Manipulated variable : which changes in experiment but determined by yourself
• Responding variable : which changes in experiment and it’s data or observation of experiment
• Constant variables : which constant and no changes during experiment
• Apparatus : instrument used
• Materials : chemical used (quantity)
• Procedure : passive sentences
• Data : table @ sentences
• Interpreting data / Discussion : why I get such a data ? chemistry equation, explanations
• Conclusion : hypothesis accepted rejected
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