Question

How do you find the mass of a solution if you know the volume and identity of the solute added, the density of the solvent, and the concentration of the solution?

Answer 1

You're leaving us a bit in the dark with this question.......

Explanation:

If `rho=1.12*g*mL^-1`, then a `1*L` volume of solution has a mass of:

`1*cancelLxx10^3*cancel(mL)*cancel(L^-1)xx1.12*g*cancel(mL^-1)=1.12xx10^3*g`

`-=1.12xxcancel(10^3)*cancelgxxcancel(10^-3)*kg*cancel(g^-1)`

`-=1.12*kg`.

Note that this is a measurement SOLELY of `"density"`. This is likely an aqueous solution, but you have not specified this.

You have not quoted units of concentration, i.e.

`"Moles of solute"/"Volume of solution"`, and thus we are in the dark.

Answer 2

I think it's possible to find the density of the aqueous solution without knowing its total mass, but I think we need the volume of the solution in addition to the volume of the solute. With this information we can find the total mass of the solution by knowing the density of water at given temperature.

Suppose we are at `20^@ "C"`. Then, the density of water is `"998.2071 g/L"`. By assuming that volumes are additive, as they are for ideal solutions, we have:

`V_"solvent" = V_"solution" - V_"solute"`

We can assume we have `"1 L"` of solution, and thus we have the volume of solvent that is in that. From there, we can use the density of water to get its mass:

`m_"solvent" = rho_"solvent"V_"solvent"`

And we can use the molar mass of the solute to get its mass. Therefore:

`"mol solute"/"L solution" = "mol solute"/"L solute + L solvent"`

`= (("mol/g solute") xx ("g solute"))/("L solute" + ("g solvent")/"g/L solvent"`

Once we have the mass of the solvent and solute, we can add them together (and masses are surely additive always) to get the mass of the solution.

Therefore, knowing the mass and volume of the solution, we can get its density.

EXAMPLE

Let's say we are given that a certain mass percent solution of `"HCl"` in water is `"12.06 M"` in molar concentration. The molar mass of `"HCl"` is `"36.4609 g/mol"`, and let's say that the volume of `"HCl"` dissolved to form a `"1.00 L"` aqueous solution is `"0.25 L"`.

It's probably not a useful calculation to do, but let's see how this works out because this is something we can easily look up the answer to.

`V_"water" = "1.00 L soln" - "0.25 L solute"`

`~~` `"0.75 L"`

`m_"water" = "998.2071 g/L water" xx "0.75 L water"`

`=` `"748.6553 g water"`

From the concentration, we'd find the mass of the solute:

`(12.06 cancel"mol HCl")/cancel"L soln" xx "36.4609 g HCl"/cancel"mol HCl" xx cancel"1 L soln"`

`=` `"439.7185 g HCl"`

And from these masses we'd get the mass of the solution:

`"439.7185 g HCl"` `+` `"748.6553 g water"`

`=` `"1188.3738 g solution"`

Knowing its assumed volume then, we'd have:

`"1188.3738 g soln"/cancel"1 L soln" xx cancel"1 L"/"1000 mL soln"`

`~~` `color(blue)("1.19 g/mL soln")`

So I think we can do it, but we would still need the total volume of the solution.