Macroscopic evidence
Colour, temperature, mass, pressure, precipitates, gas evolution, and other observations you can record.
Free, self-paced Foundations of Chemistry
Matter, arranged. Change, explained.
A complete self-paced course that keeps three views of every chemical event in sync — what you observe, what particles are doing, and what the symbols and equations say.
- Format
- Self-paced
- Level
- College algebra
- Workload
- 9–12 hrs / week
- Cost
- Free & open
Think like a chemist
See the same event at three scales.
A strong chemical explanation connects evidence, particles, and symbols instead of treating chemistry as memorisation.
Particle-level models
Atoms, ions, molecules, collisions, attractions, and the distribution of energy among them.
Symbolic representations
Formulas, balanced equations, graphs, units, and the calculations that make relationships quantitative.
The learning path
From measurement to molecular forces.
Each module adds a layer while reusing four ideas on repeat: conservation, proportional reasoning, structure, and energy.
A worked example
What a course problem actually looks like.
Every module works problems in full — the substitution, the units, the reasoning — not just the final number.
This is stoichiometry from Module 5: convert a mass to moles, use the balanced equation as a ratio, convert back to mass. The three scales are all here — a measurable mass of fuel, a particle-level ratio of molecules, and the symbolic equation that links them.
- macro4.00 g of methane is a quantity you could weigh out.
- particleOne CH₄ molecule reacts with two O₂ to give one CO₂ and two H₂O.
- symbolCH₄ + 2 O₂ → CO₂ + 2 H₂O carries the ratio 1 : 1 for CH₄ : CO₂.
Complete combustion of methane
How many grams of carbon dioxide form when 4.00 g of methane (CH₄) burns completely in oxygen?
1
Balance the equation.
CH₄ + 2 O₂ → CO₂ + 2 H₂O
2
Mass of CH₄ → moles of CH₄ (M = 16.04 g/mol).
4.00 g ÷ 16.04 g/mol = 0.2494 mol CH₄
3
Mole ratio from the equation, CH₄ : CO₂ = 1 : 1.
0.2494 mol CH₄ × (1 mol CO₂ / 1 mol CH₄) = 0.2494 mol CO₂
4
Moles of CO₂ → mass (M = 44.01 g/mol).
0.2494 mol × 44.01 g/mol = 10.98 g
Answer: 11.0 g CO₂ — three significant figures, matching the 4.00 g given. Check it with the molar-mass calculator.
Built for this site
Interactive tools, not just reading.
Things a printed textbook cannot do: a periodic table you can interrogate, and calculators that show every step of the arithmetic.
118 elementsTwenty calculatorsOne page100+ terms
Interactive periodic table
Filter by category, search by name or number, and read structure, common uses, and history for every element.
Chemistry toolkit
Molar mass, empirical formulas, stoichiometry, equation balancing, dilutions, the ideal gas law, calorimetry, pH, percent yield, unit conversions, significant figures, and scientific notation for this course's own material — plus eight calculators marked "beyond this course's own scope" covering equilibrium, buffers, kinetics, electrochemistry, nuclear decay, thermodynamics, and a titration curve grapher. Each one worked step by step.
Quick reference
Constants, vapor pressure and specific heat data, heats of fusion and vaporization, SI prefixes, polyatomic ions, solubility rules, strong acids and bases, and the activity series, ready to copy.
Filterable glossary
The essential vocabulary of first-semester chemistry, defined plainly and searchable as you type.
Course desk
Everything has a place.
Work through the site as a linear course, or jump straight to what today needs.
Course rulesRecommended paceTwelve investigationsReference desk
Read the syllabus
Outcomes, materials, grading, policies, office hours, and the weekly rhythm in one place.
Follow the pacing guide
A week-by-week pace for lessons, labs, and practice — self-paced, so slower or faster is fine.
Enter the laboratory
RAMP safety, notebook standards, report guidance, experiments, virtual options, and five at-home investigations for learners with no institution at all.
Use the study toolkit
Formulas, constants, conversions, problem templates, retrieval plans, and an error log.
A recommended week
One suggested rhythm.
Day 1
Concept pass
New model introduced with demonstrations and worked reasoning.
Day 2
Reading & practice
Assigned OpenStax reading plus a short retrieval set on the prior session.
Day 3
Problem practice
Guided practice on the week's calculations; misconceptions surfaced early.
Day 4
Laboratory
One investigation with a pre-lab check, notebook record, and analysis.
Day 5
Quiz & review
Ten-minute quiz, then problem-set review and revision.
Questions
Before you start.
What is Solute?
A free, self-paced chemistry course: fifteen learning modules with worked examples and practice, a twelve-investigation laboratory program, assessments, an interactive periodic table, a growing glossary that goes past the modules into equilibrium, kinetics, electrochemistry, and more, and step-by-step calculators.
Who is the course for and what background is needed?
First-year college students or independent learners comfortable with college algebra. No prior chemistry is assumed; Module 0 covers the math, units, and study methods used throughout.
What topics does General Chemistry I cover here?
Measurement and matter, atomic structure, the periodic table, chemical nomenclature, the mole and stoichiometry, aqueous reactions, solution concentration, thermochemistry, electronic structure and periodic trends, bonding, molecular geometry, gases, and intermolecular forces.
How much time does it take?
About 9 to 12 hours per week at the recommended pace: reading, worked practice, problem sets, one laboratory investigation per unit, and review. It's self-paced, so slower or faster is fine.
Is it really free to use?
Yes. All course materials are open and free to read, and the primary reading maps to the free OpenStax Chemistry text. Physical laboratory work still requires qualified supervision.
More detail lives in the about page and the syllabus.
By the end
Predict, calculate, explain, and investigate.
The course builds practical fluency across chemical language, quantitative reasoning, molecular structure, energy, and safe evidence-based investigation.
See all learning outcomes- Translate among names, formulas, particles, moles, mass, and concentration without losing the thread.
- Plan, document, analyse, and communicate a safe chemical investigation.
- Connect bonding and intermolecular attractions to measurable physical properties.
Laboratory work requires approved supervision.
Read the safety framework
Do not reproduce course experiments outside an approved laboratory. Follow the instructor, local procedures, safety data sheets, and emergency instructions.