Discussion OF Group A units - % by volume/% wt by volume/Strength/Molarity

Discussion OF Group B units- % by weight/Mole Fraction/Molality

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. The normality of 0.3N H_(3) BO_(3) is:

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. Number of oxalate ions in 100 mL of 0.1N oxalic acis is:

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. Molecular weight of O_(3) in the reaction, 2O_(3)hArr3O_(2) is:

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. Which is not a molecular formula?

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. Two litre of NH_(3) at 30^(@)C and 0.20 atm is neutralised by 134 mL of acid (H_(2)SO_(4)) . The molarity of H_(2)SO_(4) is:

Volume Percentage

The concentration of solutions can be expressed in number of ways such that Normality, Molarity, Molality, Mole fractions, Strength, % by weight, % by volume and % by strength. The molarity of ionic compound is usually expressed as formality beacuse we use formula weight of ionic compound. Addition of water to a solution changes all these terms, however increase in temperature does not change molality, mole fraction and % by weight terms. Volume of water required to convert 100 mL 0.5M NaOH solutions to 0.2M NaOH solution is:

Relationship between volume strength of H_2O_2 aqueous solution and molarity depeds on pressre and temperature of O_2 (g) collected Example : "At1 atm ,273K," "Volume strength =11.2xxM" "At STP, " "Volume strength =11.35 x M" [Note : By default STP is taken for volume strength and calculationl. Find the relationship between volume strength and molarity at 300 K and 1 atm.