Mass Percent of a Solution
Worked example: 25 g salt in 250 g solution → c = 10% — press Try an example to run it live, then adjust anything.
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Mass percent →
Grade 11Grade 11 Chemistry
Three ways to say how much →
Grade 12Grade 12 Chemistry
The dilution line →
UniversityProcess & Water Chemistry
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Mass Percent of a Solution explained
Mass percent is the concentration measure that needs nothing but a balance: the solute's mass divided by the mass of the whole solution — solute plus solvent — times 100. Dissolve 25 g of salt in 225 g of water and the solution is 25/250 × 100 = 10% salt by mass. The classic mistake is dividing by the solvent mass alone, which would wrongly give 11.1%.
Because it is temperature-proof and instrument-free, mass percent dominates industrial and household labels: household vinegar is about 5% acetic acid, physiological saline 0.9% NaCl, seawater roughly 3.5% dissolved salts, and concentrated sulfuric acid ships at 98%. Converting to molarity requires the solution's density, which is why bottle labels for concentrated acids list both figures side by side.
Mass Percent of a Solution formula
- = Mass percent (%)
- = Mass of solute (kg)
- = Mass of solution (kg)
Missing one of these? Work it out first, then come back
- Mass percent — Percent Composition of an Element, Empirical Formula Mole Ratio from Percent Composition
- Mass of solute — Density, Sensible Heat (Q = mcΔT)
- Mass of solution — Density, Sensible Heat (Q = mcΔT)