What is the dilution formula?

The dilution formula is C1×V1 = C2×V2, where C1 is initial concentration, V1 is volume of stock needed, C2 is final concentration, V2 is final volume. Example: To make 1L of 5% solution from 20% stock: V1 = (5% × 1000mL) ÷ 20% = 250mL stock + 750mL water.

How do I convert between concentration units?

Common conversions: % w/v to g/L = multiply by 10 (5% = 50 g/L). Molarity to g/L = Molarity × Molecular Weight. ppm to g/L = divide by 1000. For % w/w, you also need density to convert to volume-based concentrations.

What is the difference between % w/v, % w/w, and % v/v?

% w/v = grams per 100 mL of solution (most common for solids in liquids). % w/w = grams per 100 grams (mass basis, used for solids). % v/v = mL per 100 mL (for liquid-liquid mixtures like alcohol solutions).

How do I make a molar solution?

Mass needed = Molarity × Volume(L) × Molecular Weight. For 1L of 0.1M NaCl: 0.1 × 1 × 58.44 = 5.844g NaCl. Dissolve in ~800mL water, then add water to make exactly 1L (volumetric flask).

Chemical Formulation Calculator - Dilution & Concentration

What is Chemical Formulation?

Chemical formulation involves calculating exact quantities of ingredients needed to create solutions, mixtures, or products at specific concentrations. Whether you're in a research lab, manufacturing facility, or industrial setting, accurate formulation ensures product quality, safety, and regulatory compliance.

Our calculator handles dilutions from stock solutions, concentration conversions, and multi-ingredient formulations with percentage-based recipes.

Key Formulation Formulas

Dilution Equation (C1V1 = C2V2)

C1 × V1 = C2 × V2
V1 (stock volume) = (C2 × V2) ÷ C1

Mass for Molar Solution

Mass (g) = Molarity (M) × Volume (L) × Molecular Weight (g/mol)

Percentage Concentration

% w/v = (Mass of solute in g ÷ Volume of solution in mL) × 100
% w/w = (Mass of solute ÷ Total mass) × 100
% v/v = (Volume of solute ÷ Total volume) × 100

Dilution Calculation Examples

Example 1: Simple Dilution

Stock concentration (C1)	50%
Target concentration (C2)	10%
Final volume needed (V2)	500 mL
Calculation
V1 = (10 × 500) ÷ 50	100 mL stock
Water to add	400 mL

Example 2: Molar Solution

Chemical	Sodium Chloride (NaCl)
Molecular weight	58.44 g/mol
Target concentration	0.5 M
Volume needed	250 mL (0.25 L)
Calculation
Mass = 0.5 × 0.25 × 58.44	7.305 g NaCl

Concentration Unit Conversions

From	To	Formula
% w/v	g/L	× 10
g/L	% w/v	÷ 10
ppm	g/L	÷ 1000
Molarity (M)	g/L	× Molecular Weight
g/L	Molarity (M)	÷ Molecular Weight
Molarity (M)	mg/mL	× MW ÷ 1000

Common Stock Solutions

Chemical	Typical Stock	Use
Hydrochloric Acid	37% (12M)	pH adjustment, cleaning
Sulfuric Acid	98% (18M)	Strong acid applications
Sodium Hydroxide	50% (12.5M)	pH adjustment, saponification
Ethanol	95-100%	Solvent, disinfection
Hydrogen Peroxide	30-35%	Bleaching, oxidation
Ammonia	25-28%	Cleaning, pH adjustment

Formulation Safety Guidelines

Always add acid to water - Never add water to concentrated acid (exothermic)
Use PPE - Gloves, goggles, lab coat for chemical handling
Work in ventilated area - Fume hood for volatile chemicals
Check compatibility - Some chemicals react dangerously
Label everything - Concentration, date, preparer name
Dispose properly - Follow hazardous waste protocols

Serial Dilution

For creating a range of concentrations (e.g., calibration standards):

Start with highest concentration
Dilute by fixed factor (commonly 1:2 or 1:10)
Each step: Take fixed volume, add diluent

Example 1:10 serial dilution from 1000 ppm:

Step	Concentration	Preparation
Stock	1000 ppm	Original solution
1	100 ppm	1 mL stock + 9 mL diluent
2	10 ppm	1 mL from step 1 + 9 mL diluent
3	1 ppm	1 mL from step 2 + 9 mL diluent

Quality Control in Formulation

Weigh accurately - Use calibrated analytical balance (±0.1 mg for small quantities)
Volumetric glassware - Use volumetric flasks for final volume, not beakers
Temperature control - Solutions expand with heat, affecting concentration
Mixing order - Some formulations are order-sensitive
Verify concentration - Test samples against standards

Frequently Asked Questions

How do I make a buffer solution?

Buffers require weak acid + conjugate base (or weak base + conjugate acid) at specific ratios. Use Henderson-Hasselbalch equation: pH = pKa + log([A⁻]/[HA]). For common buffers (PBS, Tris, acetate), refer to published recipes and adjust pH with acid or base.

What if my chemical has different purity?

Adjust mass for purity: Required mass = Theoretical mass × (100 ÷ Purity%). If you need 10g of 95% pure chemical: 10 × (100/95) = 10.53g of the impure material.

How do I account for water of crystallization?

Use the hydrated molecular weight. CuSO₄·5H₂O (MW 249.7) vs anhydrous CuSO₄ (MW 159.6). To get equivalent copper ions, you need 1.56× more hydrated salt by mass.

Can I mix concentrated acids?

Some acid mixtures are dangerous or useful: HCl + HNO₃ = Aqua Regia (dissolves gold). Never mix without understanding the reaction. Chlorine gas can be released from bleach + acid mixtures. Always consult SDS and trained personnel.