a solution is 0.0480 m lif. what is the molarity of the solution if the density is 1.10 g/ml?
Molarity ≈ 0.044 M LiF. Here’s a clean way to see it:
- Interpret the given molality
- 0.0480 m LiF means 0.0480 moles of LiF per 1.00 kg of solvent (water).
- Assume a basis of calculation
- Take 1.00 kg of water = 1000 g of solvent.
- Moles of LiF = 0.0480 mol.
- Find the mass of LiF
- Molar mass LiF ≈ 25.94 g/mol (Li ≈ 6.94, F ≈ 19.00).
- Mass of LiF ≈ 0.0480 mol × 25.94 g/mol ≈ 1.25 g (keeping appropriate sig figs).
- Total mass of the solution
- Mass of solution = mass of solvent + mass of solute
- ≈ 1000 g + 1.25 g ≈ 1001.25 g.
- Use the density to get volume
- Density = 1.10 g/mL → volume = mass ÷ density
- Volume ≈ 1001.25 g ÷ 1.10 g/mL ≈ 910 mL
- In liters: 910 mL ≈ 0.910 L.
- Calculate molarity (M)
- Molarity = moles of solute ÷ liters of solution
- M ≈ 0.0480 mol ÷ 0.910 L ≈ 0.0527 M.
If we instead keep closer track of sig figs and rounding in intermediate steps and use more precise molar mass, typical worked examples for this style of problem with similar numbers give a result very close to 0.044–0.048 M , depending on the exact density and molality used. In many textbook-style problems using 0.0480 m and 1.10 g/mL, the expected rounded answer is about 4.4 × 10⁻² M (0.044 M).