GENERAL CHEMISTRY · SOLUTIONS STUDY MAP

Track the solvent.
Count the particles.

Fifteen focused outcomes connect polarity, solubility, particle-count effects, dissolution forces, and concentration units across the five official Solutions topics.

Start five lessons →Build a balanced set ↗See all objectives ↓
5official topics
15study objectives
5guided lessons
20original questions

Scope boundary

One solution can support several different comparisons.

The ADA names five Solutions topics but does not publish topic-level weights or question quotas. These outcomes organize study; they do not predict how many questions will appear.

Colligative effects follow effective particle concentration under a stated model. Solubility, conductivity, color, density, and other non-colligative behavior can depend on particle identity, forces, temperature, pressure, and measurement conditions.

Solution evidence sequence

Four questions before an equation.

  1. 01

    Name the components

    Which substance is solvent, which is solute, and which particles actually exist after mixing?

  2. 02

    Inventory attractions

    Compare solute–solute, solvent–solvent, and new solute–solvent interactions.

  3. 03

    Classify the property

    Does it depend mainly on dissolved-particle count or on identity and conditions?

  4. 04

    Fix the basis

    Molarity, molality, mole fraction, percent, and parts-based units use different denominators.

Official hierarchy → learning sequence

Five branches. Fifteen outcomes.

Open a topic to see its outcome, must-know relationships, model boundary, prerequisite sequence, misconception correction, and free references.

APolarity3 objectives
Objective 1

Solvent, solute, and molecular polarity

Identify solvent and solute roles and determine the relevant molecular or ionic polarity evidence before predicting solution behavior.

Must know
The solvent is the dissolving medium and is commonly, but not universally, the component present in greater amount; the solute is dispersed at the particle level. Molecular polarity follows the vector sum of bond dipoles in the three-dimensional geometry; ionic charge is not the same as a molecular dipole.
Model boundary
Use the component roles stated or supported by the preparation. Do not assign solvent solely from physical state or formula order when composition and context are ambiguous.
Misconception
The liquid component must always be the solvent. A solution can be gas, liquid, or solid, and component role follows the dissolving medium and preparation rather than physical state alone.
Earlier objectives in this map
None
Objective 2

Polarity matching and qualitative solubility

Use polar, nonpolar, or ionic character to make a bounded qualitative solubility or miscibility prediction from the attractions that can replace those in the separated components.

Must know
Polar and ionic solutes are often stabilized by polar solvents through dipole, hydrogen-bond, or ion–dipole attractions, while nonpolar solutes are often more compatible with nonpolar solvents. ‘Like dissolves like’ is a qualitative attraction comparison, not proof that every structurally similar pair is infinitely soluble.
Model boundary
Do not convert a polarity label into a quantitative solubility without supplied measurements. Size, shape, crystal energy, temperature, and competing interactions can change the result.
Misconception
Every polar substance is completely miscible with every polar solvent. Polarity can support favorable attraction, but total solution formation also depends on the interactions and structures of both separated components.
Earlier objectives in this map
Solvent, solute, and molecular polarity
Objective 3

Mixed functionality and evidence-controlled miscibility

Compare molecules containing both polar and nonpolar regions and decide which structural feature dominates a stated solvent interaction or measured partitioning result.

Must know
A molecule may contain both a polar functional region and a nonpolar carbon framework; increasing the relative nonpolar portion can reduce water compatibility within a controlled homologous series. Measured solubility, miscibility, or partition evidence outranks an unsupported judgment based on one functional group.
Model boundary
Amphiphile self-assembly, partition coefficients, and biological membrane transport are interpreted only when the needed model or data are supplied.
Misconception
One hydroxyl group guarantees high water solubility regardless of the rest of the molecule. The polar group contributes favorable interactions, but a sufficiently large nonpolar region can dominate the overall comparison.
Earlier objectives in this map
Polarity matching and qualitative solubility
B.1Properties — colligative3 objectives
Objective 1

Colligative particle-count principle

Distinguish colligative properties from identity-dependent properties and count dissolved solute particles using a supplied or idealized van ’t Hoff factor.

Must know
Colligative-property magnitude depends on the total concentration of dissolved solute particles under the stated model, not directly on their chemical identity or molar mass. For an idealized electrolyte, effective particle concentration is scaled by i; a nonelectrolyte that remains molecular has i = 1.
Model boundary
Use a supplied i or an explicitly ideal, complete-dissociation model. Real electrolyte solutions can show nonideal ion pairing, so formula subscripts do not guarantee an exact measured i.
Misconception
One mole of every solute produces the same colligative effect. The effect follows the number of dissolved particles, so ideal dissociation can make one mole of an electrolyte contribute more particles than one mole of a nonelectrolyte.
Earlier objectives in this map
None
Objective 2

Vapor-pressure, boiling-point, and freezing-point shifts

Predict and calculate vapor-pressure lowering, boiling-point elevation, or freezing-point depression for a stated ideal solution using supplied constants and particle concentration.

Must know
A nonvolatile solute lowers the solvent vapor pressure in an ideal solution; at fixed external pressure this raises the boiling point and lowers the freezing point. For the standard dilute model, ΔTb = iKbm and ΔTf = iKfm, where m is moles of solute per kilogram of solvent.
Model boundary
Raoult-law calculations require the stated ideal model and component volatility information. Kb, Kf, and any nonunity i must be supplied when numerical values are required.
Misconception
Dissolving a nonvolatile solute lowers both the boiling point and the freezing point. It lowers the freezing point but raises the boiling point because the solution reaches the external vapor pressure at a higher temperature.
Earlier objectives in this map
Colligative particle-count principle
Objective 3

Osmosis and osmotic pressure

Determine solvent movement across an ideal semipermeable membrane and calculate osmotic pressure from supplied concentration, temperature, and particle-factor data.

Must know
A membrane permeable to solvent but not solute supports net solvent movement toward the side with greater effective solute-particle concentration until opposed by pressure or equilibrium. For a dilute ideal solution, Π = iMRT uses absolute temperature and concentration of dissolved particles under the stated model.
Model boundary
Biological tonicity depends on membrane permeability and nonideal physiology; use only the membrane and solute behavior explicitly supplied. R and i must be supplied when calculation precision matters.
Misconception
Solute crosses the semipermeable membrane to dilute the concentrated side during ordinary osmosis. In the stated ideal model the membrane passes solvent, so net solvent movement—not solute passage—reduces the concentration difference.
Earlier objectives in this map
Colligative particle-count principle
B.2Properties — non-colligative3 objectives
Objective 1

Unsaturated, saturated, and supersaturated states

Classify a solution relative to its equilibrium solubility at stated conditions and interpret dissolution or precipitation after a controlled change.

Must know
An unsaturated solution can dissolve more solute under the stated conditions; a saturated solution is at equilibrium solubility; a supersaturated solution exceeds equilibrium solubility and is metastable. The words concentrated and dilute describe relative amount, not whether the solution is saturated.
Model boundary
Classify from supplied composition, solubility data, or particle evidence. Do not assume visible undissolved solid is required for a solution portion to have saturated concentration.
Misconception
Every concentrated solution is saturated. A solution can be concentrated yet still below its solubility limit, or dilute yet saturated when the solute has low solubility.
Earlier objectives in this map
None
Objective 2

Temperature, pressure, and solubility evidence

Read supplied solubility curves and apply bounded temperature or gas-pressure trends, including Henry’s law when its constant and conditions are provided.

Must know
Many solid solutes become more soluble as temperature rises, but exceptions exist; a supplied curve controls the answer. For many nonreacting gases at fixed temperature, dissolved concentration is proportional to gas partial pressure, while gas solubility in liquids typically decreases as temperature rises.
Model boundary
Henry’s-law constants depend on gas, solvent, temperature, and equation convention. Use the supplied form and units; do not apply the model when the prompt specifies substantial reaction with the solvent.
Misconception
Heating always increases the solubility of every solute. Gas solubility commonly decreases with temperature, and solid-solubility trends have exceptions that must be read from data.
Earlier objectives in this map
Unsaturated, saturated, and supersaturated states
Foundation review
Gas partial pressure ↗
Objective 3

Electrolytes, conductivity, and identity-dependent properties

Classify strong, weak, or nonelectrolyte particle models and connect solution conductivity to the concentration and mobility of dissolved ions.

Must know
Strong electrolytes produce mostly separated ions in the stated aqueous model, weak electrolytes ionize partially, and nonelectrolytes remain primarily as neutral molecules. Conductivity is non-colligative: it depends on particle charge, mobility, concentration, and identity rather than particle count alone.
Model boundary
A conductivity comparison must control concentration, temperature, and apparatus. Electrolyte strength describes extent of ion formation, not the numerical concentration of a particular sample.
Misconception
A strong electrolyte must be a highly concentrated solution. Strong refers to the extent of dissociation or ionization; a strong electrolyte solution can still be dilute.
Earlier objectives in this map
Unsaturated, saturated, and supersaturated states
CForces3 objectives
Objective 1

Three interaction sets in dissolution

Track solute–solute separation, solvent–solvent separation, and solute–solvent solvation as distinct energetic steps in solution formation.

Must know
Separating solute particles and separating solvent particles require energy, while forming solute–solvent attractions releases energy. For the stated step model, ΔHsolution is the sum of the two separation enthalpies and the solvation enthalpy, with signs preserved.
Model boundary
This ledger models interparticle changes during dissolution. Do not treat ordinary molecular dissolution as cleavage of the covalent bonds that define each solute or solvent molecule.
Misconception
Only solute–solvent attractions matter when deciding whether a solution can form. The new attractions must be evaluated against the energy needed to separate both original particle sets.
Earlier objectives in this map
None
Objective 2

Solvation-force inventory

Identify ion–dipole, hydrogen-bond, dipole–dipole, and dispersion attractions that can stabilize a specified solute–solvent pair.

Must know
Ions in a polar solvent can be stabilized by ion–dipole attractions; compatible donor and acceptor structures can form hydrogen bonds; polar molecules can add dipole–dipole attraction. London dispersion remains present for all atoms and molecules, including polar solute–solvent pairs.
Model boundary
Name every supported interaction but do not assign exact attraction energies or solubility from labels alone. A conventional hydrogen bond requires structural donor and acceptor evidence.
Misconception
An ionic solute dissolves in water because water breaks the ions into charged atoms. The ions already exist in the ionic lattice; polar water molecules stabilize separated ions through hydration interactions.
Earlier objectives in this map
Three interaction sets in dissolution
Objective 3

Energetic evidence and solution-formation limits

Use supplied attraction or enthalpy evidence to compare dissolution while recognizing that enthalpy alone does not determine spontaneity or equilibrium solubility.

Must know
A strongly exothermic solvation step can offset costly separation, but the sign of ΔHsolution alone does not establish how much solute dissolves. Some endothermic dissolutions occur because the full free-energy balance includes entropy as well as enthalpy.
Model boundary
Quantitative entropy, free-energy, lattice-energy, or Born–Haber calculations belong to their respective domains unless the prompt supplies the needed equation and data.
Misconception
Every exothermic dissolution is spontaneous and produces an infinitely soluble mixture. Heat direction is only one part of the thermodynamic balance and does not by itself determine the equilibrium solubility.
Earlier objectives in this map
Solvation-force inventory
DConcentration calculations3 objectives
Objective 1

Molarity from amount and solution volume

Calculate molarity, solute amount, or final solution volume with compatible amount and volume units.

Must know
Molarity M equals moles of solute divided by liters of total solution, not liters of solvent. Mass of solute must be converted to moles with molar mass before it enters a molarity calculation.
Model boundary
Use the stated final solution volume; do not assume solvent and solute volumes add exactly. Temperature dependence of volume is considered only when supplied.
Misconception
Molarity uses the volume of solvent before the solute is added. Its denominator is the final volume of the entire solution.
Earlier objectives in this map
None
Objective 2

Dilution and solution preparation

Use solute conservation to calculate a dilution or the aliquot needed to prepare a target solution from a stock solution.

Must know
For dilution of the same nonreacting solute, moles of solute are conserved, giving M1V1 = M2V2 when both concentrations use molarity and volumes share compatible units. The target volume is the final solution volume after dilution, not simply the amount of solvent added.
Model boundary
Do not use the dilution equation when solute reacts, precipitates, evaporates, or changes stoichiometric identity unless the prompt separately accounts for that process.
Misconception
To make 100 mL of diluted solution, add 100 mL of solvent to the stock aliquot. Transfer the aliquot and add solvent until the total solution volume reaches 100 mL.
Earlier objectives in this map
Molarity from amount and solution volume
Objective 3

Choosing and converting concentration units

Select and calculate molality, mole fraction, mass percent, volume percent, or parts-based concentration from the quantities actually supplied.

Must know
Molality is moles of solute per kilogram of solvent; mole fraction is component moles divided by total moles and all component fractions sum to one. Mass percent uses component mass divided by total solution mass; ppm and ppb are dimensionless part ratios under the stated basis, and density is required when converting between mass and volume descriptions.
Model boundary
Preserve the exact concentration basis named in the prompt. Do not interchange molarity and molality or assume dilute aqueous density is exactly 1.00 g/mL unless stated or justified by the required precision.
Misconception
A 1.0 M solution and a 1.0 m solution contain the same denominator quantity. Molarity uses liters of solution, whereas molality uses kilograms of solvent.
Earlier objectives in this map
Molarity from amount and solution volume

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Official 2026 DAT scopeDefines the five topic labels—not their weights. ↗OpenStax Dissolution ProcessSolution formation, solvation, forces, and energy steps. ↗OpenStax ElectrolytesStrong, weak, and nonelectrolyte particle and conductivity evidence. ↗OpenStax SolubilityPolarity, saturation, temperature, gas pressure, and Henry’s law. ↗OpenStax Colligative PropertiesParticle count, phase-property shifts, osmosis, and osmotic pressure. ↗OpenStax MolarityMolar concentration, dilution, and solution preparation. ↗OpenStax Concentration UnitsMass and volume percentages, parts-based units, and density bridges. ↗