75. Mole Concept and Stoichiometry-2
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Transcript of 75. Mole Concept and Stoichiometry-2
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Chemistry
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Session Opener
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Session Objectives
Problems related to
1. Mole concept
2. Stoichiometry
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Simple Titrations
Find out the concentration of a solution
with the help of a solution of knownconcentration.
1 1 2 2N V N V
For mixture of two or more substances
N1V1 + N2V2+ = NVWhere V=(V1 + V2+ ..)
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Normality of mixing two acids
1 1 2 2
1 2
N V +N VN=
V +V
Normality of mixing acid and bases
1 1 2 2
1 2
N V -N VN=
V +V
2 2 1 1
1 2
N V -N V
or N= V +V
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Questions
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Illustrative example 1
Find the molality of H2SO4 solution
whose specific gravity(density) is1.98 g/ml and 95% mass by volume H2SO4.
100 ml solution contains 95 g H2SO4.
95
98Moles of H2SO4 =
Mass of solution = 100 1.98 = 198 g
Mass of water = 198 95 = 103 g
Molality =
95 1000
98 103= 9.412 m
Solution:
Molality =moles of solute
mass of solvent in kg
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Illustrative example 2
A sample of H2SO4 (density 1.787 g/ml)is 86% by mass. What is molarity of acid?
What volume of this acid has to beused to make 1 L of 0.2 M H2SO4?
d10%
M= Molecular mass
1.7871086
= =15.68 molar98
Let V1 ml of this H2SO4 are used to prepare 1 L of 0.2 M
H2SO4.M1V1 = M2V2
15.68 V1 = 0.2 1000
10.21000
V = =12.75 ml15.68
Solution:
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Illustrative example 3A mixture is obtained by mixing 500ml0.1M H2SO4 and 200ml 0.2M HCl at 25
0C.
Find the normality of the mixture.
2 2 1 1
1 2
N V +N VWe know, N =
V + V
For the mixture, 500 0.1 2 200 0.2 1N 0.2700
Solution:
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Illustrative example 4
500 ml 0.2 N HCl is neutralized with250 ml 0.2 N NaOH. What is thestrength of the resulting solution?
Equivalents of HCl
3
500 0.2 10 eqv
Equivalents of NaOH -3=2500.210 eqv
Equivalence of excess HCl
3 3(500 0.2 10 250 0.2 10 eqv)
Normality of HCl (excess)-3 3
50010 10= =0.067 N750
Strength of HCl = .067 36.5 g/litre
= 2.44 g/litre
Solution:
2HCl NaOH NaCl H O
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Solution
1 1 2 2
1 2
N V -N VN=
V +V
0.2 1 500 - 0.2 1 250N =
500 + 250
N = 2.44 NStrength of HCl = .067 36.5 grams/litre
= 2.44 grams/litre
Normality of HCl (excess),
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Illustrative example 5
Calculate the empirical formula of a mineral
having the following compositionCaO=48.0% ;P2O5=41.3% ; CaCl210.7%
9
3
1
48.0/56=0.857
41.3/142=0.291
10.7/111=0.096
56
142
111
48.0
41.3
10.7
CaO
P2O5
CaCl2
Simple
ratio
Mol.
Mass
%tageConstituents Relative no. of const.
%=Mol. mass
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Illustrative example 6
1.5 g of an impure sample of sodiumsulpate dissolved in water was treatedwith excess of barium chloride solutionwhen 1.74 g of BaSO4 were obtained asdry precipitate. Calculate the percentagepurity of the sample.
2 4 2 42 23 32 16 4 137 32 4 16
142gm 233gm
Na SO BaCl BaSO 2NaCl
4 2 4
4
233 gm of BaSO is produced from 142 gmNa SO
1421.74 gm of BaSO is produced from 1.74 1.06gm233
2 4
2 4
The mass of pure Na SO in 1.5gm of impure sample is 1.06gm
1.06%tage purity of Na SO 100 70.67%
1.5
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Solution
3 2 22(23 14 32) 138gm2[23 14 48]170gm
2NaNO 2NaNO O
3
3
170gm of NaNO gives residue 138gm
138(5 x) gm of NaNO gives residue (5 x)gm
1700.812(5 x)gm
28Actual residue obtained (5 ) 100 3.6 gm
100
3 2
3
0.674x 0.812(5 x) 3.6
or 0.318x 0.46
or x 3.33 gm
Pb(NO ) in mixture 3.33gm
and NaNO in mixture 5 3.33 1.67 gm
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Illustrative example 8
What volume of oxygen isrequired to effect complete combustion of
200 cm3 of acetylene and what would bethe volume of CO2 formed?
2 2 2 2 22 volume 5 volume 4 volume
2C H 5O 4CO 2H O
2 2 2
According to Gay lussac's law of gaseous volumes
2 volume of C H require 5 volume of O for complete combustion
3 3
2 2
5
200 cm of C H require 200 500 cm at STP2
2
3 32 2 2
2 volume of produce CO 4volume
4200cm of C H produce CO 200 400 cm at STP
2
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Illustrative example 9
The formula weight of an acid is 82.0in a titration.100 cm3 of a solution of
this acid containing 39.0 g of the acidper litre were completely neutralisedby 95.0 cm3 of aqueous NaOH containing40.0 g of NaOH per litre. What is the basicity of the acid?
Let requirement wt. of acid =E
Normality of acid 39/EEquivalent wt. of NaOH 40 /1
Normality of NaOH 40 /40 1
Solution:
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Solution
1 1 2 2
(acid) (NaOH)
N V N V 39 100 1 95
EE 41.0
Formula wt. 82.0Basicity of acid 2
Eq. wt 41.0
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Illustrative example 10
Calculate approximate molecular mass
of dry air containing 78% N2 and 22% O2.Solution:
78 22Molecular mass 28 32 28.88
100 100
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Illustrative example 11
Calculate atomic mass of elementX and Y given thatComposition of X=9.76%Relative no. of atoms of X=0.406Composition of Y=26.01Relative no. of atoms of Y=1.625
Solution:
%tage of element 9.76Atomic mass of X 24
Relative no. of Atoms of X 0.406
%tage of element 26.01Atomic mass of Y 16Relative no. of Atoms in Y 1.625
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Illustrative example 12
The molality of a solution of ethyl alcohol(C2H5OH) in water is 1.55m.How many
grams of ethyl alcohol are dissolved in 2kgof water?
Solution:
2
2
1000gm of H O contain 1.55mol of ethyl alcohol
1.55 20002000gmof H O contain 3.10 mol
1000
Mass of ethyl alcohol 3.10 46 142.6gm
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Illustrative example 13
You are given 1 litre of 0.15 M HCl and1 litre of 0.40 M HCl. What is the maximumvolume of 0.25 M HCl which you can makefrom these solutions without adding any water?
Solution:
Volume of 0.25 M HCl cant be more than 2 litresbecause no water is added
X litre of 0.40M HCl be added to 1L 0.15 M HCl
1 1 2 2 3 3M V M V M V 0.15 1 0.40 X 0.25 (1 X)
0.15X 0.100.10
X 0.667litre0.15
Total volume of 0.25M solution 1 X
1 0.667 1.667
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Illustrative example 14
How many ml of H2SO4 of density
1.8 g/ml containing 92.5% by volumeof H2SO4 should be added to 1 litre of40% solution of H2SO4 ( density 1.30 g/ml)in order to prepare 50% solution of H2SO4(density 1.4 g/ml).
Molarity(M ) of solution containing 92.5% of H SO1 2 4
vol. of H SO Density 1000 92.5 1.8 10002 4 16.99M98 100 98 100
2 2 4Molarity(M ) of solution containing 40% of H SO
40 1.3 10005.31M
98 100
2 4Molarity(M) of solution containing 50% of H SO
50 1.4 10007.14M
98 100
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Solution
1 1 2 2M V M V MV
16.99 V 5.31 1 7.14(1 V)
9.85V 1.83
1.83V 0.186L
9.85
V 0.186L or 186 ml
1
2
Let VL of solution with molarity(M ) is added to 1L of solution
with molarity(M ) to prepare(1 V)L of solution with molarityM,
then
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Illustrative example 15
Gastric juice contains about 3.0 gof HCl per litre. If a person produces
about 2.5 litre of gastric juice per day,how many antacid tablets each containing400 mg of Al(OH)3 are needed to neutralizeall the HCl produced in one day?
3 3 23(35.1 1) 27 3(16 1)109.5 78g
3HCl Al(OH) AlCl 3H O
Amount of HCl produced ina day 2.5 3 7.5g
3Now 109.5g of HCl require Al(OH) 78g
378
7.5 g of HCl will require Al(OH) 7.5 5.34g109.5
5.34Number of tablets required 13.35 14 tablets
0.4
Solution:
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Illustrative example 16
Calculate the number of Cl ions in
100 ml of 0.001 M HCl solution.
Solution:
HCl is a strong acid, it ionises completely
1000ml of 0.001M HCl solution contains Cl 0.001 mole
4
0.001 100100 ml of 0.001M HCl solution contains Cl
1000
1 10 mole
Conc. of HCl is equal to that of Cl
ions
23 4
19
No. of Cl ions 6.023 10 1.0 10
6.023 10
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Helena kabr se farar
Group 1 elements (Alkalimetals)
He
Li
Na
K
Rb
Cs
Fr
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Be
Mg
Ca
Sr
Ba
Ra
Bear mugs can serve bar rats
Group 2 elements(Alkaline earth metals)
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B
Al
Ga
In
Tl
Bob Allen Gave Indians Tennis Lessons
Group 13 elements (Boronfamily)
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C
Si
Ge
Sn
Pb
Can sily or Genius snatch lead
Group 14 elements (Carbon family)
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N
P
As
Sb
Bi
Never put arsenic in silver bullet bear
Group 15 elements (Nitrogen family)
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O
S
Se
Te
Po
Oh, she sells tie Poles
Group-16 elements (Oxygen family)
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F
Cl
Br
I
At
Fat Clyde bribed Innocent Atul
Group-17 elements (Halogen family)
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Group-18 elements (The NobleGas)
He
Ne
Ar
Kr
Xe
Rn
He needs our crazy Xerox repairman
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Thank you