Laws of Definite Proportions, Multiple Proportions

Q.

What is the equivalent mass of ${\mathrm{KMnO}}_4$ in an acidic and alkaline medium?

Q. Concentration of NaOH solution is 4.0 molal and its density is 1.11g/ml. What is the molarity of the solution ? 1) 2.95 2)3.82 3)4.11 4)3.0

Q. What is the mass of sodium acetate required to make 200ml of 0.245 molar aqueous solution? (molar mass of CH3COONa=82g/mol)

Q.

The equivalent mass of $\mathrm{Fe}$ in $\mathrm{FeO}$ is $(\mathrm{Fe}=56)$

1. $56$

2. $28$

3. $36$

4. $18.66$

Q. Q.If 12.6g of NaHCO3 is added to 30.0g of CH3COOH solution, the residue is found to weigh 36.0g. What is the mass of CO2 released in the reaction ?

Q. The density of 20% (w/w) aqueous NaOH solution is 1.20 g/ml. What is the mole fraction of water?

Q. 15 To a 25 ml H2O2 solution, the excess of acidified solution of KI was added. The iodine librated required 20ml of 0.3 N Na2S2O3 solution. The volume strength of H2O2 solution is 1) 1.34 g/L 2) 3.24 g/L 3) 5.4 g/L 4) 4.08 g/L

Q. How many grams of KCI must be added to75.0 grams of water to produce a solution that is2.25 molal (m)? \lbrack Molecular weight of KCI 74.5\rbrack

Q. Irrespective of the source, a pure sample of water always yields 88.89% mass of oxygen and 11.11% mass of hydrogen. This is explained by the law of:

1. Conservation of mass
2. Multiple proportions
3. Constant composition
4. Constant volume

Q.

Law of constant composition does not hold good for:

1. Endothermic compounds

2. Exothermic compounds

3. Stoichiometric compounds

4. Non-stoichiometric compounds

Q. For "16.8 V" H2O2 solution ( density = 0.95 g/ml), calculate :- 1. Molarity 2. Molality 3. % w/w 4. % w/v 5. ppm of solute 6. mole fraction of solute

Q. How to calculate the weight of 1000 atoms of N.

Q. percent by mass of solute in is aqueous solution is 30.The mole fraction and molality of the solute in solution are

Q. 47. A sample of H2O2 solution is labelled as 28 volume. Its percentage by volume strength is (a) 6.5 (b) 7.5 (c) 5.5 (d) 8.5

Q. Dalton's theory included which of the following ideas?

1. All atoms of all elements are of same size
2. Atoms of different elements always combine in one-to-one ratio
3. Atoms of the same element are always identical
4. Individual atoms can be seen with a microscope

Q. Percentage of weight by volume of 0.6 M AgNO3(aq) (molar mass of AgNO3 = 170 g/mol) is

Q. The density of 3 molal solution of NaOH is 1.110gmL^-1. Calculate the molarity of the solution

Q. Element X forms five stable oxides of formula - $X_{2}O,XO,X_2{O}_3,X_2{O}_4,X_2{O}_5$. The formation of the oxides explains:

1. Avogadro's law
2. Law of partial pressure
3. Law of multiple proportions
4. Gay-Lussac's law

Q. Equal masses of H2, He and CH4 are mixed in an empty container at 300k, when total pressure is 2.6 atm. The partial pressure of H2 in the mixture is

Q. What mass of He could be contained in a vessel that can holds 4.48 litre of SO2 at STP? Options: 0.9 g 1.6 g 2.8 g 0.8 g

Q. Copper oxide was prepared by two different methods. In case one, 1.75 g of the metal gave 2.19 g of the oxide. In the second case, 1.14 g of the metal gave 1.43 g of the oxide. This is explained by which of the following laws?

1. Law of definite proportions
2. Law of partial pressure
3. Law of multiple proportions
4. Gay-Lussac's Law

Q. Ammonia gas is passed into water, yielding a solution of density 0.93g/cm cube and containing 18.6% NH3 by weight . The mass of NH3 per cc of the solution is ?

Q. 10 g of an oxide of X contains 5.0 g of X while 8.0 g of another oxide of the same species contains 3.2 g of X. Which law is indicated in this data?

1. Law of multiple proportions
2. Law of conservation of mass
3. Law of constant proportions
4. Law of reciprocal proportions

Q. To make 2.5 kg of 0.25 molar aqueous solution, determine the mass of urea (NH2CONH2) that is required.

Q.

Calculate the equivalent mass of sodium.

Q. 1Q)In 9.8% solution of H2SO4 in water, density is 1.2 g/mL. Find the mass of 1 L solution. 2Q)In 9.8% solution of H2SO4 in water, density is 1.2 g/mL. Find mass of solute i.e. H2SO4 in 1 L solution. 3QIn 9.8% by mass aqueous H2SO4 solution, density was found 1.2 g/mL. The molarity of solution will be

Q. Concentration of glucose in blood is approximately 90 mg/100 ml. The molarity of glucose solution in blood is

Q. What will be the change of mass when 10g Mg is heated strongly in oxygen?

Q. the mole fraction pf a solute in a solution is 0.1 at 298 K. Molality of this solution is same as molarity. Density of this solution at 298 K is 2g/cm^3. Find the ratio of molecular weight of solute and solvent

Q. what is equivalent mass of salts meaning?