In a water sample,the concentration of F^- io | vedclass

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(A) The concentration in $ppm$ (parts per million) is defined as the mass of solute in $mg$ per liter of solution.Given,concentration = $10 \ ppm = 10

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$10^{-3}$

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(A) The concentration in $ppm$ (parts per million) is defined as the mass of solute in $mg$ per liter of solution.Given,concentration = $10 \ ppm = 10 \ mg/L$.We know that $1 \ mg = 10^{-3} \ g$.So,$10 \ mg = 10 	imes 10^{-3} \ g = 10^{-2} \ g$.Thus,the concentration is $10^{-2} \ g/L$.To convert this to $\% W/V$ (grams per $100 \ mL$):Concentration in $\% W/V = \frac{	ext{mass of solute in } g}{	ext{volume of solution in } mL} 	imes 100$.Concentration = $\frac{10^{-2} \ g}{1000 \ mL} 	imes 100 = \frac{10^{-2}}{10} = 10^{-3} \% W/V$.

In a water sample,the concentration of $F^-$ ions is $10 \ ppm$ by weight-volume. What is the concentration of $F^-$ in $\% W/V$ in that solution?

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