Easily convert percentage concentration to molarity for your solutions. Ideal for students and professionals in chemistry.

In the field of chemistry, a comprehensive grasp of solution concentrations is indispensable for a multitude of applications, ranging from laboratory experiments to industrial procedures. Two widely employed metrics, percentage concentration and molarity, often necessitate conversion between them, akin to unraveling an age-old enigma.

Thankfully, the Percentage Concentration to Molarity Calculator comes to the aid, streamlining this conversion process and facilitating your forays into the realm of chemistry.

This practical tool serves as a conduit between two distinct modes of expressing solute concentration in a solution:

**Percentage concentration**: This signifies the weight/volume (w/v) or weight/weight (w/w) percentage of the solute within the solution. For instance, a 10% w/v sodium chloride solution implies that 10 grams of NaCl are dissolved in every 100 milliliters of the solution.

**Molarity (M)**: This denotes the moles of solute per liter of solution. A 1 M NaCl solution contains 1 mole of NaCl (58.44 grams) for every liter of the solution.

The calculator processes the percentage concentration, along with pertinent details like molar mass and density, yielding the corresponding molarity. This obviates the need for manual calculations, saving valuable time and effort.

While utilizing the calculator is straightforward, comprehending the underlying equation empowers you to perform calculations even without the tool.

The key lies in this formula:

$Molarity\left(M\right)=\frac{(Percentageconcentration\times Density)}{(Molarmass\times 10)}$

Where:

Simply input the known values, solve for M, and there you have the molarity of your solution at your disposal.

Let's apply the theory with some examples:

**Example 1**: Determine the molarity of a 20% w/v sulfuric acid (${H}_{2}S{O}_{4}$) solution with a density of 1.84 g/mL.

Solution -

Molar mass of ${H}_{2}S{O}_{4}$ = 98.08 g/mol

Density = 1.84 g/mL = 1840 g/L

$Molarity=\frac{(0.2\times 1840)}{(98.08\times 10)}=3.76M$

**Example 2**: Find the percentage concentration of a solution containing 0.5 moles of glucose (${C}_{6}{H}_{12}{O}_{6}$) in 2 liters of water.

Solution -

Molar mass of ${C}_{6}{H}_{12}{O}_{6}$ = 180.16 g/mol

$Percentageconcentration$

$=\frac{(0.5mol\times 180.16g/mol\times 100)}{(2L\times 1000g/L)}=4.5\%$

Here are some additional examples of converting percentage concentration to molarity:

**70% (w/w) sulfuric acid (H2SO4) in water:** Molarity ≈ 11.7 M

**15% (w/v) ethanol (C2H5OH) in water:** Molarity ≈ 2.5 M

**5% (w/w) glucose (C6H12O6) in water:** Molarity ≈ 0.28 M

Some calculators allow you to choose the solute, and they may provide an estimated density for that specific solution. Otherwise, you may need to look up the density in a reference book or online database.

Yes, the same equation can be used to convert molarity to percentage concentration by rearranging the terms.

The equation applies to solutions with one solute. For multi-component solutions, individual solute concentrations need to be determined separately.

You can still use the same equation, but the density needs to be adjusted based on the specific solution and its components.