Advertisements
Advertisements
प्रश्न
Nalorphene (C19H21NO3), similar to morphine, is used to combat withdrawal symptoms in narcotic users. Dose of nalorphene generally given is 1.5 mg. Calculate the mass of 1.5 × 10−3 m aqueous solution required for the above dose.
Advertisements
उत्तर
Given: m = 1.5 × 10−3
The molar mass of nalorphene (C19H21NO3) = 19 × 12 + 21 × 1 + 1 × 14 + 3 × 16
= 311 g mol−1
In a 1.5 × 10−3 m aqueous solution of nalorphene,
1 kg (1000 g) of water contains 1.5 × 10−3 mol.
= 1.5 × 10−3 × 311 g
= 0.467 g
= 467 mg
∴ Total mass of the solution = (1000 + 0.467) g
= 1000.467 g
Thus, for 467 mg of nalorphene, the solution required is 1000.467 g.
∴ The mass of the solution containing 1.5 mg of nalorphene = `1000.467/467 xx 1.5`
= 3.21 g
Hence, the mass of the aqueous solution required is 3.21 g.
संबंधित प्रश्न
Define mass percentage.
Concentrated nitric acid used in laboratory work is 68% nitric acid by mass in aqueous solution. What should be the molarity of such a sample of the acid if the density of the solution is 1.504 g mL−1?
A solution of glucose in water is labelled as 10% w/w, what would be the molality and mole fraction of each component in the solution? If the density of solution is 1.2 g mL−1, then what shall be the molarity of the solution?
How many mL of 0.1 M HCl are required to react completely with 1 g mixture of Na2CO3 and NaHCO3 containing equimolar amounts of both?
22.22 gram of urea was dissolved in 300 grams of water. Calculate the number of moles of urea and molality of the urea solution.
(Given: Molar mass of urea = 60 gram mol−1)
An X molal solution of a compound in benzene has mole fraction of solute equal to 0.2. The value of X is ____________.
An aqueous solution of glucose is 10% in strength. The volume in which 1 g mole of it is dissolved, will be:
Which of the following concentration terms is/are independent of temperature?
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:
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"` |
Define the following modes of expressing the concentration of a solution. Which of these modes are independent of temperature and why?
w/w (mass percentage)
Define the following modes of expressing the concentration of a solution. Which of these modes are independent of temperature and why?
(iii) w/V (mass by volume percentage)
Define the following modes of expressing the concentration of a solution. Which of these modes are independent of temperature and why?
M (Molarity)
What is the ratio of mass of an electron to the mass of a proton?
The number of electrons involved in the reduction of one nitrate ion to hydrazine is
The de Broglie wavelength of a car of mass 1000 kg and velocity 36 km/hr is :
What is molarity of resulting solution obtained by mixing 8.5 L of 0.5 m urea solution and 500 ml of 2 m urea solution?
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 mole fraction of a solute in a 100 molal aqueous solution is ______ × 10-2. (Round off to the Nearest Integer).
[Given :Atomic masses : H : 1.0 u, O : 16.0 u]
