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An aqueous solution of NaCl is 350 ppm. What is the mass of NaCl in 1.00 L of the solution? Assume the density of the solution is 1.00 g/mL.​

Sagot :

MakotoOrekiidn

Answer:

Hence, the Mass of NaCl is 0.35

Explanation:

Given that,

[tex] \cdot \ \ \rm{NaCl = 350 ppm} [/tex]

[tex] \cdot \ \ \rm{Volume \ of \ Solution = 1.00\cancel{L} \times \frac{1000mL}{1\cancel{L}} = 1000mL} [/tex]

[tex] \cdot \ \ \rm{Density \ of \ Solution = 1.00 \ g/mL} [/tex]

[tex] \cdot \ \ \rm{Mass \ of \ NaCl = ?}[/tex]

First step, we are going to find the mass of the solution, using the formula:

  • [tex] \boxed{\bold{D = \frac{M}{V}}}[/tex]

Substituting...

[tex] \rm{1.00 \ g/mL = \frac{M}{1000 \ mL} = 1000 \ g} [/tex]

Second step, we are going to find now the Mass of NaCl, using the formula:

  • [tex] \boxed{\bold{PPM = \frac{Mass \ of \ NaCl}{Mass \ of \ Solution} \times 10^6}}[/tex]

Substituting...

[tex] \rm{350 = \frac{Mass \ of \ NaCl}{1000} \times 10^6} \\ \rm{Mass \ of NaCl = \frac{1000 \times 350}{10^6}} \\ \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \rm{ = \frac{350000}{1000000}} \\ \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \: \rm{= 0.35} [/tex]

Hence, the Mass of NaCl is 0.35