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What is Concentration of Solution?
Methods of Expressing Concentration of Solutions
Percentage by Weight
Percentage by Volume
Weight by Volume
Mole Fraction
Parts Per Million
Molarity
Molality
Normality
Formality
Demal
The Concentration of a Solution is defined as the relative amount of solute present in a solution.
It basically talks about how to find the amount of solute present in solvent which together forms solution.There are various methods used to find this,
Percentage by weight (w / w %)
Percentage by volume (V / V%)
Weight by volume (w / v%)
Mole fraction (x)
Parts per million (ppm)
Molarity (M)
Molality (m)
Normality (N)
Formality (F)
Demal (D)
All of them are briefed below:
Symbol: (w / w %)
Definition: It is defined as the amount of solute present in 100 g of solution.
Unit: No unit
Symbol: (V / V %)
Definition: It is defined as the volume of solute present in 100 mL of solution.
Symbol: (W / V %)
Definition: It is defined as the amount of solute present in 100 mL of solution.
Unit: mg/L
Formula:
Percent Concentration
Example:
As an example consider 5 g sugar dissolved in 20 g of water. What is the w/w% concentration of sugar in this solution?
Symbol : X ( lower-case Greek letter chi, χ)
Definition: It is the ratio of the number of moles of solute and the total number of moles of solute and solvent.
Mole Fraction (X): This is the number of moles of a compound divided by the total number of moles of all chemical species in the solution.
What are the mole fraction of the components of the solution formed when 92 g glycerol is mixed with 90 g water? (molecular of weight water = 18; molecular weight of glycerol = 92)
Solution:
90 g water = 90 g x 1 mol / 18 g = 5 mol water
92 g glycerol = 92 g x 1 mol / 92 g = 1 mol glycerol
Total mol = 5 + 1 = 6 mol
X water = 5 mol / 6 mol = 0.833
X glycerol = 1 mol / 6 mol = 0.167
It’s a good idea to check your math by making sure the mole fractions add up to 1:
xwater + xglycerol = .833 + 0.167 = 1.000
Symbol: ppm
Definition: It is defined as the parts of a component per million parts (106) of the solution. It is widely used when a solute is present in trace quantities.
Unit: ppm
Calculate the molar concentration of 2000 ppm of Pb2 + (A. M. = 207 g/mol)?
PPM = M x M. M.x1000
Symbol : M
Definition: Molarity of any solution is number of moles of solute per liter of solution
Unit: mol/litre
Molarity = Number of moles of solute / Volume of solution in liter.
What is the molarity of a solution containing 0.32 moles of NaCl in 3.4 liters?
= 0.94 M NaCl
Symbol: m
Definition: Molality of any solution is represented as the number of moles of solute present per kg of solvent
Unit: mol/kg
Molality(m) = Number of moles of solute / Mass of solvent in Kg
Note: Why m is not affected by change in temperature?
Since it is dependent on mass of solute and mass do not change to small shift in temperature due to close packing of solid atoms therefore it is independent of temperature change.
What is the molarity of a solution containing 0.46 mole of solute in 2.0 kg water?
Given:
Moles of Solute = 0.46 mole
Kilogram of Solvent = 2.0 kg
= 0.23 m
Symbol : N
Definition: It is defined as the gram equivalent weight per liter of solution.
Unit: equivalent/L
Normality = Number of grams – Equivalent of solute / Volume of solution in L
Number of gram-equivalents of solute = Mass of solute in gram / Equivalent weight
Calculate the normality of 0.53 g/100 mL solution of Na2 CO3 (M.M. = 106 g/mol) as the following reaction:
Na2CO3 + 2H+ → H2CO3 + 2Na
Eq. wt. of Na2 CO3 = 106/2 = 53 g/eq
Symbol : F
Definition: It is the number of formula weights of solute present per liter of the solution.
Unit: mol/L
It is applicable in case of ionic solids like NaCI.
Calculate the formality of solution in which 948 gram potash alum is dissolved in 5 litre solution.
The formula mass of potash alum is 474 gram (formula mass)-1.
Symbol: D
Definition: It represents one mole of solute present in 1L of solution at O°C.
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