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Standard XII

Chemistry

Concentration Terms - An Introduction (w/w etc)

The concentra...

Question

The concentration of $B r^{-}$ ion in a sample of $H_{2} O$ is 36 ppm. What is the mass of $B r^{-}$ ion is present in 250.0 mL of water ? (given density of water is 1.00 g/ $c m^{3}$ )

2.0 mg

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9.0 mg

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12.0 mg

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5.0 mg

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Solution

The correct option is B 9.0 mg
As density of water = 1 g/mL , using
$D e n s i t y = \frac{m a s s}{v o l u m e}$
We get mass of water = $1 g / m L \times 250 m L$
$= 250 g$
Now, Using
$p p m = \frac{mass of solute (g)}{m a s s o f s o l u t i o n (g)} \times 10^{6} 36 = \frac{mass of solute}{250} \times 10^{6}$
Mass of solute $= \frac{250 \times 36}{10^{6}} g = \frac{9000}{10^{6}} g$
$= \frac{9000}{10^{6}} \times 10^{3}$ mg = 9 mg

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Concentration Terms - An Introduction (w/w etc)

Standard XII Chemistry

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The concentration of Br− ion in a sample of H2O is 36 ppm. What is the mass of Br− ion is present in 250.0 mL of water ? (given density of water is 1.00 g/cm3)

The correct option is B 9.0 mgAs density of water = 1 g/mL , using Density=massvolume We get mass of water = 1 g/mL×250 mL =250 g Now, Using ppm=mass of solute (g)mass of solution(g)×10636=mass of solute 250×106 Mass of solute =250×36106 g=9000106 g =9000106×103 mg = 9 mg

The concentration of $B r^{-}$ ion in a sample of $H_{2} O$ is 36 ppm. What is the mass of $B r^{-}$ ion is present in 250.0 mL of water ? (given density of water is 1.00 g/ $c m^{3}$ )