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.
Advertisements
Solution
300 g of 25% solution contains solute = 75 g
400 g of 40% solution contains solute = 160 g
Total solute = 160 + 75 = 235 g
Total solution = 300 + 400 = 700 g
% of solute in the final solution = `235/700 xx 100`
= 33.5%
% of water in the final solution = 100 − 33.5
= 66.5%
APPEARS IN
RELATED QUESTIONS
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?
If the solubility product of CuS is 6 × 10−16, calculate the maximum molarity of CuS in aqueous solution.
Calculate the mass percentage of aspirin (C9H8O4) in acetonitrile (CH3CN) when 6.5 g of C9H8O4 is dissolved in 450 g of CH3CN.
What is molal depression constant? Does it depend on nature of the solute?
Molarity of the solution is ____________.
Which of the following is a quantitative description of the solution?
The volume of 4 N HCl and 10 N HCl required to make 1 litre of 6 N HCl are ____________.
200 ml of water is added to 500 ml of 0.2 M solution. What is the molarity of this diluted solution?
For preparing 0.1 N solution of a compound from its impure sample of which the percentage purity is known, the weight of the substance required will be:
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:
Define the following modes of expressing the concentration of a solution. Which of these modes are independent of temperature and why?
V/V (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)
A solution has been prepared by dissolving 5 g of urea in 95 g of water. What is the mass percentage of urea in the solution?
3.36 M sulphuric acid solution is 29% H2SO4 calculate the density of the solution.
Calculated the mole fraction of benzene in a solution containing 30% by mass of its is carbon tetrachloride
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 ______.
4 ml of pure A (d = 2.45 gm/ml) was added to 46 ml of B (d = `25.1/23` gm/ml), the molarity of a solution of A in B will be ______, if the density of the final solution is 1.8 gm/ml.
Given: Molar mass of A = 98, Molar mass of B = 46
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.
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.
