5
% w/v
5
% v/v
5
% w/w
50
g/L
50,000
mg/L
50,000
ppm
50
g
5
% w/v
5
% v/v
5
% w/w
50
g/L
50,000
mg/L
50,000
ppm
50
g
The Percent Solution Calculator computes the concentration of a solution expressed as a percentage. Three types of percent concentration are supported: % w/v (weight/volume, grams of solute per 100 mL of solution), % v/v (volume/volume, mL of solute per 100 mL of solution), and % w/w (weight/weight, grams of solute per 100 grams of solution). Percent solutions are among the most common ways to express concentration in laboratory chemistry, clinical settings, pharmacy, and industrial manufacturing. A 5% w/v NaCl solution, for example, contains 5 grams of sodium chloride in every 100 mL of solution. This calculator also converts your result to amount per liter and parts per million (ppm), enabling easy cross-referencing with environmental, food safety, and industrial standards that often use ppm notation.
The percent concentration formula is straightforward:
% Concentration = (Amount of Solute / Amount of Solution) × 100
For % w/v: the solute is measured in grams and the solution in milliliters. A result of 5% w/v means 5 g of solute per 100 mL of solution. This is the most common expression in medical and pharmaceutical contexts.
For % v/v: both solute and solution are measured in volume units (mL). Ethanol concentration in beverages is often expressed this way — 40% v/v means 40 mL of ethanol per 100 mL of beverage.
For % w/w: both are measured in mass units (grams). This is preferred when density varies with concentration or when working with solid mixtures.
The calculator also converts to per-liter amounts (multiply by 10 for w/v to get g/L) and ppm (1% = 10,000 ppm). These conversions are critical for regulatory compliance, where limits are often specified in ppm. Note that ppm conversions assume dilute aqueous solutions where 1 mL ≈ 1 g for the solvent. For non-aqueous or concentrated solutions, density corrections may be needed.
The percent concentration directly tells you how much solute is present in a given amount of solution. Higher percentages mean more concentrated solutions. The ppm conversion is useful for trace-level analysis: 1% equals 10,000 ppm. When comparing concentrations across different systems, pay attention to whether the percentage is w/v, v/v, or w/w, as these are not interchangeable unless the density of the solute equals that of the solvent. For dilute aqueous solutions, the three types give approximately equal values.
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Normal saline is 0.9% w/v NaCl — 9 grams of sodium chloride dissolved in 1000 mL of solution. This equals 9 g/L or 9,000 ppm.
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50 mL of ethanol in 500 mL of beverage gives 10% v/v alcohol content, equivalent to 100 mL per liter.
% w/v uses mass of solute (grams) per volume of solution (mL). % v/v uses volume of solute per volume of solution. % w/w uses mass of solute per mass of solution. The choice depends on whether the solute is a solid, liquid, or gas, and the convention in your field.
Molarity = (% × 10 × density) / molecular weight. For example, 37% w/w HCl with density 1.19 g/mL and MW 36.46: M = (37 × 10 × 1.19) / 36.46 ≈ 12.1 M. The density factor is essential for this conversion.
Yes, for weight-based or dilute aqueous solutions: 1% = 1/100 = 10,000/1,000,000 = 10,000 ppm. This conversion assumes the denominator units are equivalent, which holds for dilute aqueous solutions where solution density ≈ 1 g/mL.
Medical solutions are typically administered by volume (mL), so expressing concentration as grams per 100 mL allows clinicians to quickly calculate the mass of drug a patient receives from a given volume. For example, D5W (5% w/v dextrose) delivers 5 g of glucose per 100 mL infused.
Dissolve 2 grams of solute in enough solvent to make 100 mL of total solution. Do not simply add 2 g to 100 mL of solvent — the final volume must be 100 mL. Use a volumetric flask for precision: add solute, partially fill with solvent, dissolve, then fill to the mark.
For % w/w, no — the solute cannot weigh more than the total solution. For % w/v, it is theoretically possible if the solute is very dense and soluble (e.g., a very concentrated heavy metal salt solution could exceed 100 g per 100 mL), though this is uncommon in practice.
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