Question

What is the concentration in parts per million? Assume the density of the solution is the same as that for pure water (1.00 g/mL). ppm

Answer 1

6.6

Step-by-step explanation:

Answer 2

The question is incomplete, here is the complete question:

What is the concentration, in parts per million, of a solution prepared by dissolving 0.00040 mol HCl in 2.2 L
`H_2O` ? Assume that the volume of the solution does not change when the HCl is added. Assume the density of the solution is the same as that for pure water (1.00 g/mL)

Answer: The concentration of HCl in the solution is 6.64 ppm

Step-by-step explanation:

• To calculate the number of moles, we use the equation:

`\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}`

We are given:

Moles of HCl = 0.00040 moles

Molar mass of HCl = 36.5 g/mol

Putting values in above equation, we get:

`0.00040mol=\frac{\text{Mass of HCl}}{36.5g/mol}\\\\\text{Mass of HCl}=(0.00040mol* 36.5g/mol)=0.0146g`

• To calculate the mass of water, we use the equation:

`\text{Density of substance}=\frac{\text{Mass of substance}}{\text{Volume of substance}}`

Density of water = 1.00 g/mL

Volume of water = 2.2 L = 2200 mL (Conversion factor: 1 L = 1000 mL)

Putting values in above equation, we get:

`1.00g/mL=\frac{\text{Mass of water}}{2200mL}\\\\\text{Mass of water}=(1.00g/mL* 2200mL)=2200g`

ppm is the amount of solute (in milligrams) present in kilogram of a solvent. It is also known as parts-per million.

To calculate the ppm of HCl in the solution, we use the equation:

`\text{ppm}=\frac{\text{Mass of solute}}{\text{Mass of solution}}* 10^6`

Both the masses are in grams.

We are given:

Mass of HCl = 0.0146 g

Mass of solution = 2200 g

Putting values in above equation, we get:

`\text{ppm of HCl in solution}=(0.0146g)/(2200g)* 10^6\\\\\text{ppm of HCl in solution}=6.64`

Hence, the concentration of HCl in the solution is 6.64 ppm