Advertisements
Advertisements
Question
A solution is obtained by mixing 300 g of 25% solution and 400 g of 40% solution by mass. Calculate the mass percentage of the resulting solution.
Solution
The total amount of solute present in the mixture is given by,
= `300 xx 25/100+400xx40/100`
= 75 + 160
= 235 g
Total amount of solution = 300 + 400 = 700 g
Therefore, mass percentage (w/w) of the solute in the resulting solution = `(235 xx 100)/700`
= 33.57%
And, mass percentage (w/w) of the solvent in the resulting solution,
= (100 − 33.57)%
= 66.43%
APPEARS IN
RELATED QUESTIONS
Define Molarity (M).
If the density of some lake water is 1.25 g mL−1 and contains 92 g of Na+ ions per kg of water, calculate the molality of Na+ ions in the lake.
Define Normality.
Which of the following is a quantitative description of the solution?
Molarity of liquid HCl will be if the density of the solution is 1.17 gm/cc.
An X molal solution of a compound in benzene has mole fraction of solute equal to 0.2. The value of X is ____________.
10 g of NaCl is dissolved in 106 g of the solution. Its concentration is ____________.
200 ml of water is added to 500 ml of 0.2 M solution. What is the molarity of this diluted solution?
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:
Which of the following units is useful in relating concentration of solution with its vapour pressure?
Out of molality (m), molarity (M), formality (F) and mole fraction (x), those which are independent of temperature are:
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 (Molality)
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?
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)
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]
A 5% solution of \[\ce{Na2SO4.10H2O}\] (MW = 3 22) is isotonic with 2% solution of non- electrolytic, non volatile substance X. Find out the molecular weight of X.
Calculate the molarity of the following solution:
30 mL of 0.5 M \[\ce{H2SO4}\] diluted to 500 mL.
