Express the concentration of a 0.0510 M aqueous solution of fluoride, F-, in mass percentage and in parts per million. Assume the desnity of the solution is 1.00 g/mL

Since, we're assuming the density I think that also means were assuming the volume.. but where would you go from there? please help!

I don't know to agree or disagree about the volume since you don't say what you are assuming about the volume.

0.0510 M means 0.0510 moles/L soln.
0.0510 mol x 19 g F^-/mol = about 0.969 g/L soln.
Since the density of the soln is 1.00 g/mL, then this is 0.969 g F^-/1000 g soln
% w/w = (0.969g/1000g)*100 = 0.0969%.

For ppm, I find the factor 1 ppm = 1 mg/L to be useful.
0.000969 g/mL x (1000mg/g) = 0.969 mg/mL x (1000 mL/L) = 969 g/L = 969 ppm.
Check all of this carefully.

yes that was correct! thank you

Well, if we assume the density is 1.00 g/mL, that means that 1 mL of the solution has a mass of 1.00 grams. So, if we have a 0.0510 M solution, that means we have 0.0510 moles of F- ions in 1 liter (or 1000 mL) of solution.

To find the mass percentage, we need to multiply the molar mass of F- by the number of moles and then divide it by the mass of the solution (which is equal to the volume times the density).

The molar mass of F is 19 g/mol. Therefore, the mass of F- in 0.0510 moles is 0.0510 moles * 19 g/mol = 0.969 g.

The volume of the solution is 1000 mL, so the mass of the solution is 1000 mL * 1.00 g/mL = 1000 g.

Now we can calculate the mass percentage:

Mass percentage = (0.969 g / 1000 g) * 100 = 0.0969% (rounded to four decimal places)

To express the concentration in parts per million (ppm), we can use the formula:

ppm = (mass of solute / mass of solution) * 1,000,000

ppm = (0.969 g / 1000 g) * 1,000,000 = 969 ppm

So, the concentration of the 0.0510 M aqueous solution of fluoride is approximately 0.0969% in mass percentage and 969 ppm.

To determine the concentration of a solution in mass percentage and parts per million (ppm), we need to start by finding the mass of the solute (fluoride, F-) in a known volume of the solution.

Given:
Molarity (M) = 0.0510 M
Density of the solution = 1.00 g/mL

Let's assume we have 1 liter (1000 mL) of the solution. Since the density is 1.00 g/mL, the mass of the solution would also be 1000 grams (1 L x 1 g/mL = 1000 g).

To find the mass of the solute, we can use the following equation:

Mass of solute = Molarity x Volume x Molar mass

First, we need to determine the molar mass of fluoride (F-). The molar mass of F is approximately 18.998 g/mol.

Using the equation above, we have:

Mass of solute = 0.0510 M x 1000 mL x 18.998 g/mol

Now, let's calculate the mass of the solute:

Mass of solute = 0.0510 mol/L x 1000 mL x 18.998 g/mol
= 972.48 g

Now that we know the mass of the solute (F-), we can calculate its concentration in different units.

1. Mass Percentage (w/w):
Mass percentage (w/w) = (Mass of solute / Mass of solution) x 100

Since the density of the solution is 1.00 g/mL, we know that the mass of the solution is 1000 g.

Mass percentage (w/w) = (972.48 g / 1000 g) x 100
= 97.25%

Therefore, the concentration of the 0.0510 M aqueous solution of fluoride (F-) is approximately 97.25% in mass percentage.

2. Parts per million (ppm):
Parts per million (ppm) = (Mass of solute / Mass of solution) x 10^6

Parts per million (ppm) = (972.48 g / 1000 g) x 10^6
= 972,480 ppm

Therefore, the concentration of the 0.0510 M aqueous solution of fluoride (F-) is approximately 972,480 ppm.

To express the concentration of a solution in mass percentage and parts per million (ppm), we need to determine the mass of fluoride ions (F-) present in the given solution.

Given:
- Concentration of the aqueous solution (C) = 0.0510 M (Molar)
- Density of the solution (ρ) = 1.00 g/mL

To find the mass of fluoride ions, we need to consider the molar mass of fluoride (F-) ion, which is approximately 19.0 g/mol.

Step 1: Calculate the volume of the solution
Since we are assuming the density of the solution is 1.00 g/mL, and density = mass/volume, we can assume that the mass of the solution is equal to the volume. Therefore, the volume of the solution is 1.00 mL (or 1.00 cm³).

Step 2: Calculate the mass of fluoride ions
The concentration of the solution is given in moles per liter (M), so we need to convert the volume of the solution to liters.
Volume of the solution = 1.00 mL = 1.00 cm³ = 1.00 x 10^(-3) L.

Now, to calculate the mass of fluoride ions present:
Mass of fluoride ions (g) = concentration (mol/L) x molar mass (g/mol) x volume (L)

Mass of fluoride ions = 0.0510 mol/L x 19.0 g/mol x 1.00 x 10^(-3) L = 0.000969 g

Step 3: Express the concentration in mass percentage
Mass percentage = (Mass of fluoride ions / Mass of the solution) x 100

Mass percentage = (0.000969 g / 1.00 g) x 100 = 0.0969 %

Step 4: Express the concentration in parts per million (ppm)
ppm = (Mass of fluoride ions / Mass of the solution) x 10^6

ppm = (0.000969 g / 1.00 g) x 10^6 = 969 ppm

Therefore, the concentration of the 0.0510 M aqueous solution of fluoride (F-) is approximately 0.0969% (mass percentage) and 969 ppm (parts per million).