Chemistry Chapter: Electrolytes and Reactions

A substance that, when dissolved in water, forms a solution that can conduct electricity.

A substance that, when dissolved in water, forms a solution that does not conduct electricity.

A substance that dissolves completely into ions (100% dissociation) in water and conducts electricity very well

A substance that partially dissolves into ions in water (not completely dissociated) forms an incomplete solution that conducts electricity less effectively than a strong electrolyte

The process of water molecules surrounding and interacting with an ion in a solution.

A chemical reaction where an insoluble solid, called a precipitate, forms from a solution.

A chemical equation that shows only the species that participate in the reaction. Spectator ions are removed.

The reaction of an acid (H+) with a carbonate (CO3^2-) produces carbon dioxide gas (CO2), water (H2O), and a salt.

An Arrhenius acid is a substance that produces hydrogen ions (H+) when dissolved in water.

A Brønsted-Lowry acid is a proton donor.

An insoluble solid that forms and separates from a solution during a chemical reaction.

An ion that appears on both the reactant and product sides of a net ionic equation and does not participate in the reaction.

The maximum amount of a solute that can dissolve in a given amount of solvent at a particular temperature.

A chemical equation that represents strong electrolytes as their constituent ions.

A chemical equation showing the complete formulas of all reactants and products.

A list of metals ranked by their reactivity, with the most reactive metal at the top. Metals higher in the series can displace metals lower in the series from their compounds.

A reaction where a metal reacts with an acid to produce hydrogen gas and a salt. Metals above hydrogen in the activity series can displace hydrogen from acids.

A reaction where a more reactive metal displaces a less reactive metal from its salt solution.

A reaction where a more reactive halogen displaces a less reactive halogen from its compound.

A reaction where an element in one oxidation state is simultaneously oxidized and reduced, meaning it acts as both an oxidizing and reducing agent.

A reaction between an acid and a base, often forming salt and water.

A reaction involving the transfer of electrons between reactants, resulting in changes in oxidation states.

A reaction between an acid and a base that produces a salt and water. The H+ ions from the acid react with the OH- ions from the base to form water.

The molarity of an acid solution can be calculated if the volume and molarity of a base required to neutralize it are known.

When the number of moles of H+ ions from the acid equals the number of moles of OH- ions from the base.

In a neutralization reaction, the mole ratio between the acid and base determines the stoichiometry of the reaction.

The concentration of K+ ions in a 1M KCl solution is 1M. Since KCl is a strong electrolyte, it completely dissociates in water, producing one K+ ion and one Cl- ion for every mole of KCl.

The concentration of NO3- ions in a 1M Ba(NO3)2 solution is 2M. Ba(NO3)2 dissociates into one Ba2+ ion and two NO3- ions per formula unit.

Molarity is a measure of the concentration of a solution. It is defined as the number of moles of solute per liter of solution.

The number of moles of solute can be calculated using the formula: moles of solute = molarity x volume.

Dilution is the process of reducing the concentration of a solution by adding more solvent. This results in an increase in the volume of the solution while keeping the number of moles of solute constant.

The dilution formula states that the number of moles of solute before dilution is equal to the number of moles of solute after dilution. This can be expressed as: MiVi = MfVf.

The equivalence point in a titration is the point at which the acid and base have completely reacted with each other. At this point, the moles of acid are exactly equal to the moles of base.

An indicator is a substance that changes color at or near the equivalence point of a titration. This color change signals that the reaction is complete.

A homogeneous mixture of two or more substances, where one substance (the solute) is dissolved in another (the solvent).

A solution where the solvent is water.

A substance that, when dissolved in water, forms a solution that conducts electricity.

A substance that, when dissolved in water, forms a solution that does not conduct electricity.

The process of water molecules surrounding and interacting with ions in a solution.

A chemical reaction in an aqueous solution that produces an insoluble solid called a precipitate.

An insoluble solid that forms and separates from a solution during a chemical reaction.

Ag+(aq) + Cl-(aq) → AgCl(s)

1. Strong electrolytes in solution are written in their ionic form.
2. Weak electrolytes are written in their molecular (un-ionized) form.
3. Nonelectrolytes are written in their molecular form.
4. Insoluble substances, precipitates, and gases are written in their molecular forms.
5. The net ionic equation should include only substances that have undergone a chemical change. Spectator ions are omitted.
6. Equations must be balanced both in atoms and in electrical charge.

The mixture will contain a precipitate of AgCl (s) and spectator ions Na+(aq) and NO3-(aq) in solution.

A net ionic equation shows only the species that participate in the reaction. Spectator ions, which do not participate, are removed.

A Brønsted-Lowry base is a proton acceptor.

An acid that releases one hydrogen ion (H+) per molecule when dissolved in water.

An acid that releases two hydrogen ions (H+) per molecule when dissolved in water.

An acid that releases three hydrogen ions (H+) per molecule when dissolved in water.

A substance that donates a proton (H+) in a chemical reaction.

A substance that accepts a proton (H+) in a chemical reaction.

A substance that can act as both a Brønsted acid and a Brønsted base.

The loss of electrons by a substance.

The gain of electrons by a substance.

A substance that causes another substance to be oxidized by accepting electrons.

A chemical reaction where two or more substances combine to form a single product.

A chemical reaction where a single compound breaks down into two or more simpler substances.

A chemical reaction where a substance reacts with oxygen, usually releasing heat and light.

A chemical reaction where an ion or atom in a compound is replaced by an ion or atom of another element.

A type of displacement reaction where a metal reacts with an acid or water to produce hydrogen gas and a salt.

A type of displacement reaction where a more reactive metal displaces a less reactive metal from its salt solution.

A metal will displace another metal from its salt solution if it is higher in the activity series. The higher the metal in the activity series, the more reactive it is.

Zinc metal reacts with copper sulfate solution to produce zinc sulfate and copper.

Strong electrolytes fully break down into ions when dissolved in water. This means 100% of the substance forms ions, leading to high conductivity.

When a strong electrolyte dissolves, the concentration of each ion is determined by the number of moles of that ion produced per mole of the compound.

To find the mass of solute needed to make a specific solution, use the formula: Mass = (Moles x Molar Mass).

Diluting a solution means reducing its concentration by increasing its volume while keeping the number of moles of solute unchanged.

The equivalence point in titration is when the acid and base have completely reacted, meaning their moles are equal, neutralizing each other.

An indicator signals the equivalence point in a titration by changing color, indicating that the reaction has reached completion.

Titration involves carefully adding a solution of known concentration to a solution of unknown concentration to determine its concentration through complete reaction.