chemistry lecture 2
TRANSCRIPT
Chemistry Lecture-2
Topics
1) Laws of chemical combinations
2) The Gas Laws
3) Ideal Gas Equation
4) Avogadro’s Hypothesis
5) Vapour density
6) Mole concept
7) What is a Solution?
1) Laws of chemical combinations
Questions
1. If water sample are taken from sea, rivers or lake, they will be found to contain hydrogen
and oxygen in the approximate ratio of 1 : 8. This indicates the law of:
(a) Multiple proportion (b) Definite proportion
(c) Reciprocal proportions (d) None of these
2. Hydrogen and oxygen combine to form H2O2 and H2O containing 5.93% and 11.2%
hydrogen respectively. The data illustrates :
(a) law of conservation of mass (b) law of constant proportion
(c) law of reciprocal proportion (d) law of multiple proportion
Mole concept
1) Strength of the solution (gm/ml)
2) Mass Percentage (%w/w)
3) Molarity (M)
4) Normality (N)
5) Relation between Molarity and Normality
6) Molality (m)
7) Mole Fraction (X)
Que: 6 grams of a solute are present in 500 ml of solution.
What is the strength and the density of the solution?
Que: A solution is prepared by adding 10 gm of a
substance S to 50 gm of water. Calculate the %w/w of
the solute.
Que: 49 grams of H2SO4 are present in 100 ml aqueous solution.
What is the molarity of H2SO4. Molar mass of H2SO4 = 98gm/mol
Que: Calculate the normality (N) of the solution containing 5 g
NaOH dissolved in 250 mL aqueous solution.
Que: 214.2 g of an aqueous solution of sugar contains 34.2
grams sugar. If molecular mass of sugar is 342, calculate the
molality of the solution.