Advertisements
Advertisements
Question
Match the terms given in Column I with expressions given in Column II.
| Column I | Column II |
| (i) Mass percentage | (a) `"Number of moles of the solute component"/"Volume of solution in litres"` |
| (ii) Volume percentage | (b) `"Number of moles of a component"/"Total number of moles of all the components"` |
| (iii) Mole fraction | (c) `"Volume of the solute component in solution"/"Total volume of solution" xx 100` |
| (iv) Molality | (d) `"Mass of the solute component in solution"/"Total mass of the solution" xx 100` |
| (v) Molarity | (e) `"Number of moles of the solute components"/"Mass of solvent in kilograms"` |
Advertisements
Solution
| Column I | Column II |
| (i) Mass percentage | (d) `"Mass of the solute component in solution"/"Total mass of the solution" xx 100` |
| (ii) Volume percentage | (c) `"Volume of the solute component in solution"/"Total volume of solution" xx 100` |
| (iii) Mole fraction | (b) `"Number of moles of a component"/"Total number of moles of all the components"` |
| (iv) Molality | (e) `"Number of moles of the solute components"/"Mass of solvent in kilograms"` |
| (v) Molarity | (a) `"Number of moles of the solute component"/"Volume of solution in litres"` |
APPEARS IN
RELATED QUESTIONS
Why is molality of a solution independent of temperature?
Calculate the mass percentage of benzene (C6H6) and carbon tetrachloride (CCl4) if 22 g of benzene is dissolved in 122 g of carbon tetrachloride.
Calculate the mole fraction of benzene in solution containing 30% by mass in carbon tetrachloride.
Define Mass percentage.
A sample of drinking water was found to be severely contaminated with chloroform (CHCl3) supposed to be a carcinogen. The level of contamination was 15 ppm (by mass):
- express this in percent by mass.
- determine the molality of chloroform in the water sample.
The sum of all mole fraction for a mixture is always equal to ____________.
The molarity of pure water is ____________.
10 g of NaCl is dissolved in 106 g of the solution. Its concentration is ____________.
If N/10 50 ml H2SO4, N/3 30 ml HNO3, N/2 10 ml HCl is mixed and solution is made to 1 L. Then normality of the resultant solution is:
A solution is prepared by dissolving 10 g NaOH in 1250 mL of a solvent of density 0.8 mL/g. The molality of the solution in mol kg–1 is:
Out of molality (m), molarity (M), formality (F) and mole fraction (x), those which are independent of temperature are:
Cone. H2SO4 is 98% H2SO4 by mass has d = 1.84 g cm−3. Volume of acid required to make one litre of 0.1 M H2SO4 is:
Which of the following is a correct statement for C2H5Br?
Match List-I with List-II:
| List-I | List-II |
| A. ppm | I. molL-¹ |
| B. Molarity | II. No units |
| C. Molality | III. Independent of temperature |
| D. Mole fraction | IV. Very dilute solutions |
Choose the correct answer from the options given below:
What is the ratio of mass of an electron to the mass of a proton?
Calculated the mole fraction of benzene in a solution containing 30% by mass of its is carbon tetrachloride
4.5 g of compound A (MW = 90) was used to make 250 mL of its aqueous solution. The molarity of the solution in M is x × 10−1. The value of x is ______. (Rounded-off to the nearest integer)
A sample of Ferrous sulphide reacts with dil. H2SO4 to from H2S which contains 9% hydrogen by volume. The percentage of fee in the sample, is ______.
The depression in freezing point of water observed for the same amount of acetic acid, trichloroacetic acid and trifluoroacetic acid increases in the order given above. Explain briefly.
