Advertisements
Advertisements
Question
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
Solution
Given, m = 1.5 × 10−3
The molar mass of nalorphene (C19H21NO3) is given as
= 19 × 12 + 21 × 1 + 1 × 14 + 3 × 16
= 311 g mol−1
In 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
Therefore, total mass of the solution = (1000 + 0.467) g
= 1000.467 g
Thus, for 467 mg of nalorphene, the solution required = 1000.467 g
Therefore, 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.
APPEARS IN
RELATED QUESTIONS
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.
Calculate the mass of urea (NH2CONH2) required in making 2.5 kg of 0.25 molal aqueous 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?
An antifreeze solution is prepared from 222.6 g of ethylene glycol (C2H6O2) and 200 g of water. Calculate the molality of the solution. If the density of the solution is 1.072 g mL−1, then what shall be the molarity of the solution?
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: a Molar mass of urea = 60 gram mol-1)
Molarity of the solution is ____________.
The molarity of the solution containing 7.1 g of Na2SO4 in 100 ml of aqueous solution is ____________.
The mole fraction of the solute in one molal aqueous solution is ____________.
25 ml of a solution of barium hydroxide on titration with a 0.1 molar solution of hydrochloric acid gave a titre value of 35 ml. The molarity of barium hydroxide solution was ______.
Mole fraction of the solute in a 1.00 molal aqueous solution is ____________.
How many grams of concentrated nitric acid solution should be used to prepare 250 mL of 2.0M HNO3? The concentrated acid is 70% HNO3:
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)
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:
The number of electrons involved in the reduction of one nitrate ion to hydrazine is
What is the normality of 0.3 m H3Pcl solution?
138 g ethyl alcohol is mixed with 72 g of water. The ratio of mole fraction of alcohol to water is ______.
250 mL of 0.5 M NaOH was added to 500 mL of 1 M HCl. The number of unreacted HCl molecules in the solution after complete reaction is ______ × 1021. (Nearest integer) (NA = 6.022 × 1023).
The molarity of the solution prepared by dissolving 6.3 g of oxalic acid (H2C2O4 · 2 H2O) in 250 mL of water in mol L-1 is x × 10-2. The value of x is ______. (Nearest integer)
[Atomic mass: H : 1.0, C : 12.0, O : 16.0]
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.
