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Chemistry Solver

Use this chemistry solver to explore school and introductory college problems with balanced equations, mole ratios and explicit solution assumptions. Type a question or upload a clear photo or PDF, then use worked steps or gradual hints to check your understanding.

Tip: drag a photo here or paste a screenshot (Ctrl+V)
How are solve allowances used?

Math, physics, chemistry and all AI tools share your plan allowance.

Each successful standard AI submission uses one standard solve. Deep reasoning uses one deep solve instead. Both count toward the daily solve limit.

Photos and selected PDF pages also use one daily photo solve per submission. Uploading a file or selecting a page does not start a solve. PDF upload requires Plus or Pro.

Local calculations, worked examples, hints, copying answers and cached answers use no solves.

Technical failures return the reserved solve. An automatic retry is included in the same submission. A new successful AI submission counts again, even if it follows an earlier answer.

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Topic tools

Worked example

Step-by-step solution

Balance Fe + O2 -> Fe2O3.

Step 1 / 3

Count atoms in the unbalanced equation

Iron and oxygen counts do not initially match.

Fe+O2→Fe2O3\mathrm{Fe}+\mathrm{O_2}\rightarrow\mathrm{Fe_2O_3}

How to work through a problem

  1. Enter formulas with correct capitalization, charges and subscripts.
  2. Supply concentrations, amounts, temperature and any required atomic weights or equilibrium constants.
  3. Balance atoms and charge, convert quantities to consistent units and follow the steps.
  4. Check limiting reactants, rounding and the assumptions behind any equilibrium approximation.

Scope and assumptions

Keep formulas and assumptions explicit

Balancing changes coefficients, not chemical subscripts. Stoichiometric coefficients give mole ratios, while mass calculations also require molar masses from a stated atomic-weight table.

A pH calculation needs the identity and strength of the acid or base, concentration and temperature. Ideal dilute behavior and complete dissociation are conditional approximations. These tools do not establish reaction feasibility or provide experimental safety instructions.

Using the Chemistry Solver to preserve formulas and calculation bases

Chemistry solver inputs: substances and quantities

Inputs to this chemistry solver often connect a chemical identity with an amount, composition or condition. Start by writing the supplied formula with correct capitalization, subscripts and electric charges, then name the requested quantity. Molar mass, mass of a sample, moles, concentration and theoretical yield are different quantities with different units. If atomic weights or equilibrium constants are supplied, use those values throughout. A clear photograph or PDF should preserve formula details and table labels. Describe unreadable notation in text rather than replacing it with a chemically different guess.

For reaction questions in this chemistry solver, a balanced reaction conserves atoms and, where relevant, electric charge. Its coefficients establish mole ratios between the specified species, not direct ratios of sample masses. Balancing also does not predict a missing product or establish that a reaction occurs under arbitrary conditions. For a yield question, the amounts of all potentially limiting reactants or an explicit excess assumption are needed. For a concentration question, identify the specified solute and whether the denominator is total solution volume, solvent mass or another stated basis. Selecting that basis comes before performing arithmetic.

Chemistry solver example: limiting reactants and yield

Consider the supplied reaction N2 + 3 H2 -> 2 NH3 with 2 mol nitrogen and 3 mol hydrogen. The nitrogen amount could support 4 mol ammonia, but the hydrogen amount supports only 2 mol ammonia. Hydrogen is therefore limiting, and theoretical product is 2 mol ammonia under complete conversion by this reaction. One mole of nitrogen is consumed and one remains in excess. The limiting conclusion follows from comparing coefficient ratios; it cannot be found by simply choosing the reactant with the smaller mass or displayed number.

Using N = 14.007 and H = 1.008 g/mol gives ammonia molar mass 17.031 g/mol. The theoretical ammonia mass is therefore 34.062 g before final significant-figure rounding. If a reported product amount on that same basis is 25.5465 g, its apparent percent yield is 75%. Actual yield and theoretical yield must describe the same product and matching units. An apparent result above 100% requires checking measurement, purity and calculation bases; report the computed value without silently capping it or claiming an unstated cause.

Chemistry solver units: concentration and dilution

For a concentration example, a solution contains 2.922 g NaCl in a total final volume of 250 mL. With the supplied NaCl molar mass 58.44 g/mol, its amount is 0.0500 mol. The solution volume is 0.250 L, so formal molarity is 0.200 mol/L. This calculation uses solution volume, not solvent mass or an unspecified volume of water. Ion concentrations require a dissociation model as well: under an ideal complete-dissociation approximation, each NaCl formula unit contributes one sodium ion and one chloride ion.

A hypothetical 25 mL portion of that 0.200 mol/L solution contains 0.005 mol NaCl. If that same amount is described in a total final solution volume of 100 mL with no solute loss or reaction, the new concentration is 0.050 mol/L. Initial and final concentration–volume products both represent 0.005 mol. This is a numerical conservation example, not a laboratory preparation procedure. Added solvent volume is a different quantity from final solution volume, and the simple dilution relation should not be used when a reaction consumes the tracked solute.

Chemistry solver review: equilibrium and assumptions

The pH shortcut using the negative base-ten logarithm of acid concentration has a limited scope. For ideal dilute 0.001 mol/L HCl at 25 °C with complete dissociation, hydrogen-ion activity is approximated by concentration relative to 1 mol/L, giving pH 3. A tenfold dilution under the same assumptions gives approximately pH 4. The same shortcut cannot be applied to every weak acid or buffer. Those problems need the relevant equilibrium constants and amounts, and sufficiently dilute solutions can require including water’s contribution to the ion balance.

Review the chemistry solver explanation’s formulas and units alongside the calculation. Recount atoms in a balanced equation, expand parentheses in a molar-mass calculation and confirm that a concentration denominator matches its definition. Use supplied temperature and significant-figure requirements rather than presenting every decimal as a measured certainty. The educational tools explain common school and introductory college relationships; they do not provide experimental procedures or establish product purity or reaction feasibility. Read the displayed assumptions and request clarification when the input does not support a unique result. AI tools share your existing account allowance; a new standard or deep solve counts against its corresponding solve limit.

Common questions

What chemistry topics are covered?

The starter tools cover common equation balancing, molar mass, mole-ratio stoichiometry and introductory pH calculations.

Can I upload a chemical equation or table?

Use a readable photo or PDF and type any unclear formulas, charges or table values. Ambiguous labels should be clarified before calculating.

Why do atomic weights or pH answers vary?

Atomic-weight tables use different rounding, and pH depends on temperature and activity assumptions. Include the values required by your course.

Does a balanced equation prove a reaction occurs?

No. Balancing checks conservation. Reaction feasibility, products and experimental conditions require separate chemical evidence.