If 11 g of oxalic acid is dissolved in 500 mL of solution (density $=$ 1.1 g mL $^{- 1}$ ), what is the mass % of oxalic acid in solution?

Open in App

Solution

11 g of oxalic acid is present in 500 mL of solution.

Density of solution $= 1.1 g m L^{- 1}$

Mass of solution $= (500 m L) \times (1.1 g m L^{- 1})$

$= 550 g$

Mass of oxalic acid $=$ 11 g

Mass % of oxalic acid $= \frac{11}{550} \times 100 = 2$ %

Suggest Corrections

Similar questions

Calculate the mass percentage of solution if 11 g of oxalic acid are dissolved in 500 mL.

Q. If

1.26 g

of oxalic acid is dissolved in

250 m L

of solution, find its normality. The equivalent mass of oxalic acid is

63

Q. Solution of oxalic acid is prepared by dissolving 0.63g of acid in 250ml of solution .calculate molarity

Q. Find the normality of oxalic and solution containing

63 g

of crystalline oxalic acid in

500 m l

of solution.

A known mass of oxalic acid dihydrate is dissolved in water to make 100 ml solution. 10 ml of this solution is diluted to 100 ml. 20 mL of the solution requires 20 mL of 0.1 N NaOH for complete neutralisation. (eq. mass of oxalic acid dihydrate = 63). The mass of oxalic acid in gram in the original solution is

Join BYJU'S Learning Program

If 11 g of oxalic acid is dissolved in 500 mL of solution (density = 1.1 g mL−1), what is the mass % of oxalic acid in solution?

11 g of oxalic acid is present in 500 mL of solution.Density of solution =1.1gmL−1Mass of solution =(500mL)×(1.1gmL−1) =550gMass of oxalic acid = 11 gMass % of oxalic acid =11550×100=2%

If 11 g of oxalic acid is dissolved in 500 mL of solution (density $=$ 1.1 g mL $^{- 1}$ ), what is the mass % of oxalic acid in solution?

11 g of oxalic acid is present in 500 mL of solution.

Density of solution $= 1.1 g m L^{- 1}$

Mass of solution $= (500 m L) \times (1.1 g m L^{- 1})$

$= 550 g$

Mass of oxalic acid $=$ 11 g

Mass % of oxalic acid $= \frac{11}{550} \times 100 = 2$ %