Chemistry Chapter on Electrolytes and Solutions

A strong electrolyte dissociates completely into ions in solution, while a nonelectrolyte does not dissociate and consists of intact molecules.

Weak acids only partially ionize in solution, leaving a majority of the acid molecules non-ionized, unlike strong acids which completely ionize.

Silver chloride remains as a solid precipitate in water and does not dissolve, indicating it is insoluble.

<p>Molecular equations show reactants and products as intact, undissociated compounds, not reflecting the ions that are actually present in solution.</p> Signup and view all the answers

<p>Water's polar molecular shape allows it to effectively surround and interact with ionic and some covalent compounds, dissolving them.</p> Signup and view all the answers

<p>Chemists rely on a set of observed empirical rules based on solubility trends of various ionic compounds to predict their solubility in water.</p> Signup and view all the answers

<p>Hydrochloric acid completely ionizes into H+ and Cl- ions when dissolved in water, categorizing it as a strong electrolyte.</p> Signup and view all the answers

<p>Knowing a compound's solubility impacts predictions regarding chemical reactions, associated products, and their formation in aqueous environments.</p> Signup and view all the answers

<p>Spectator ions appear unchanged on both sides of a total ionic equation and do not participate in the actual chemical change.</p> Signup and view all the answers

<p>The reactants are butane (C4H10) and oxygen (O2), while the products are carbon dioxide (CO2) and water (H2O).</p> Signup and view all the answers

<p>A net ionic equation eliminates spectator ions and only shows the species that undergo a chemical change, providing a clearer picture of the reaction.</p> Signup and view all the answers

<p>The solute-solute interactions hold the solid together, while solvent-solute interactions occur when the solvent molecules interact with the solute particles, potentially leading to dissolution.</p> Signup and view all the answers

<p>The polar nature of water allows it to effectively surround and stabilize the separated Na+ and Cl- ions, facilitating their dissolution.</p> Signup and view all the answers

<p>A precipitate is an insoluble solid compound formed when two soluble ionic compounds react in solution to produce an insoluble product.</p> Signup and view all the answers

<p>The key event is the formation of an insoluble product through the net removal of ions from solution.</p> Signup and view all the answers

<p>The balanced equation is: $SiO_2 (s) + 3C (s) \rightarrow SiC (s) + 2CO (g)$</p> Signup and view all the answers

<p>A precipitation reaction occurs when soluble ionic compounds are mixed and at least one product is insoluble in the solution.</p> Signup and view all the answers

<p>Hydrogen bonds between water molecules contribute to their ability to solvate and separate solute particles, allowing them to dissolve.</p> Signup and view all the answers

<ol> <li>Note the ions in the reactants. 2. Consider all possible cation-anion combinations. 3. Decide whether any combination is insoluble.</li> </ol> Signup and view all the answers

<p>Solvation refers to the interaction of solvent molecules with solute ions, which is relevant because it determines whether ions remain in solution or form a precipitate.</p> Signup and view all the answers

<p>The balanced equation is: $2C_2H_6 (g) + 7O_2 (g) \rightarrow 4CO_2 (g) + 6H_2O (g)$</p> Signup and view all the answers

<p>All common compounds of Group 1A (1) ions and ammonium ion (NH4+) are always soluble.</p> Signup and view all the answers

<p>The charges of the ions must balance on both sides of the equation to ensure that the overall charge remains zero.</p> Signup and view all the answers

<p>Potassium chromate and silver acetate contain different cations (K+ and Ag+) and anions (CrO4^2- and C2H3O2-) that serve as spectator ions in respective reactions.</p> Signup and view all the answers

<p>Sugar dissolves in water due to the strong attractions between sugar molecules and water molecules, which overcome the intramolecular forces within sugar.</p> Signup and view all the answers

<p>Yes, most common sulfates are soluble, except for those of Ca2+, Sr2+, Ba2+, Ag+, and Pb2+.</p> Signup and view all the answers

<p>The formation of solid products is driven by the stronger electrostatic attractions between certain ions compared to their solvation, leading to an insoluble compound.</p> Signup and view all the answers

<p>All common carbonates (CO32-) are insoluble except those of Group 1A(1) and NH4+.</p> Signup and view all the answers

<p>The products are solid cobalt and carbon dioxide gas.</p> Signup and view all the answers

<p>They are generally soluble except for those of Ag+, Pb2+, Cu+, and Hg22+.</p> Signup and view all the answers

<p>All common metal hydroxides are insoluble except those of Group 1A(1) and larger members of Group 2A(2), starting with Ca2+.</p> Signup and view all the answers

<p>Most common sulfides are insoluble except those of Group 1A(1), Group 2A(2), and NH4+.</p> Signup and view all the answers

A representation of a chemical reaction using symbols and formulas.

Substances present before a chemical reaction occurs.

Substances formed as a result of a chemical reaction.

A type of chemical reaction where a substance combines with oxygen to produce energy.

Attractive forces between solvent molecules and solute particles.

Water molecules have a partial negative charge on oxygen and partial positive on hydrogens.

The process where ionic compounds dissolve in water, breaking into separate ions.

Sugar dissolves in water due to attraction between sugar and water molecules.

Substances that completely dissociate into ions when dissolved in water.

Substances that do not dissociate into ions in solution.

Molecular compounds that completely ionize in water, like HCl.

Acids that do not fully ionize in solution, such as acetic acid.

Soluble compounds dissolve in water; insoluble do not.

Reactions occurring in water.

Equations showing all reactants and products intact, not as ions.

The process where ionic compounds separate into ions in water.

An equation showing all soluble ionic compounds as separate, solvated ions.

Ions that appear unchanged on both sides of a chemical equation.

An equation that shows only the ions involved in the actual chemical change.

An insoluble solid compound formed during a chemical reaction in solution.

A reaction where two soluble ionic compounds react to form an insoluble product.

A process where ionic compounds exchange ions in solution.

The force between oppositely charged ions that can lead to the formation of precipitates.

Ions that are surrounded by water molecules in a solution.

Atoms or molecules with a net electrical charge due to loss or gain of electrons.

The ability of a substance to dissolve in a solvent.

Guidelines to predict whether a compound will dissolve in water.

Ionic compounds that dissolve in water, such as Group 1A ions.

Ionic compounds that do not dissolve well in water, like metal hydroxides.

Ionic compounds containing CO3^2- that are generally insoluble except with Group 1A and NH4+.