Acids and Bases Quiz

A neutral solution has a pH of 7.

A substance that releases hydrogen ions (H⁺) when in a solution and its formulas often starts with hydrogen.

A substance that releases hydroxide ions (OH⁻) when in a solution. or accepts hydrogen ions to form water.

A reaction between an acid and a base that produces salt and water.

Examples include NaOH and KOH.

Acids donate H⁺ ions (hydrogen ions) when dissolved in water.

Bases accept H⁺ ions or release OH⁻ ions (hydroxide ions) in water.

Water can act as both an acid by donating H⁺ and a base by accepting H⁺ (forming OH⁻).

Ammonia (NH₃) is an exception, acting as a base by accepting H⁺ and forming ammonium (NH₄⁺). Ammonium can then act as an acid by donating H⁺.

Ammonia ($NH_3$) acts as a weak base in water by accepting hydrogen ions ($H^+$), indirectly releasing hydroxide ions ($OH^-$). This indirectly increases the concentration of $OH^-$ in the solution, making it slightly alkaline.

A weak base releases hydroxide ions ($OH^-$) indirectly in a solution, while a strong base releases $OH^-$ directly. Weak bases have a lower pH than strong bases, though both are still considered alkaline.

Metal carbonates are basic compounds, but their pH is lower than metal oxides. This means they are less alkaline.

A reaction where a solid, called a precipitate, forms and settles at the bottom of a solution.

Both reactants must be soluble in the solution to form an insoluble product. The precipitate can also be an aqueous solution.

Soluble + Soluble = Insoluble + Other Products. One of the products MUST be insoluble.

In a precipitation reaction, the insoluble product is the one that forms a solid and settles at the bottom.

A chemical reaction where a compound breaks down into simpler substances using heat.

The primary products of complete combustion are carbon dioxide ($CO_2$) and water ($H_2O$)

A chemical reaction that releases heat and light, typically involving the rapid reaction of a substance with oxygen.

Combustion where there's not enough oxygen, resulting in carbon monoxide ($CO$) production instead of carbon dioxide ($CO_2$)

Oxygen is essential for complete combustion, leading to the formation of carbon dioxide ($CO_2$) from carbon oxidation.

A chemical reaction where a more reactive element replaces a less reactive element in a compound.

A list of elements arranged in order of their reactivity, with the most reactive at the top.

Elements that easily gain or lose electrons are more reactive. The fewer electrons needed to be gained or lost, the more reactive the element.

A type of displacement reaction where one element replaces another element in a compound.

Mg(s) + FeSO₄(aq) → MgSO₄(aq) + Fe(s)

The number of neutrons in an atom's nucleus. It is calculated by subtracting the atomic number from the mass number.

Atoms of the same element that have the same number of protons but different numbers of neutrons, resulting in different mass numbers.

The mass of one mole of a substance. It is calculated by dividing the mass of a sample by the number of moles in the sample.

The amount of solute dissolved per unit volume of solution. It is calculated by dividing the number of moles of solute by the volume of the solution.

Q represents the amount of heat energy transferred in a substance. It is calculated by multiplying the mass of the substance, its specific heat capacity, and the change in temperature.

The amount of energy needed to raise the temperature of 1g of a substance by 1K.

The amount of heat transferred depends on:

Acid + Alkali → Salt + Water

The fundamental building blocks of atoms, including protons, neutrons, and electrons.

Standard units used in chemistry include:

A chemical bond formed by the sharing of electron pairs between atoms.

Covalent compounds typically have low melting and boiling points, are often liquids or gases at room temperature, and do not conduct electricity well.

A reaction that releases heat into the surroundings, resulting in a decrease in the overall energy of the system. It has a negative enthalpy change.

A reaction that absorbs heat from the surroundings, resulting in an increase in the overall energy of the system. It has a positive enthalpy change.

The minimum amount of energy required for a reaction to occur. It is the difference in energy between the reactants and the transition state.

Isotopes of the same element have the same chemical properties because they have the same electron arrangement. Electrons determine how an atom interacts with other atoms, defining its chemical behavior.

Ionic bonding occurs due to the strong electrostatic attraction between oppositely charged ions. This attraction extends throughout the entire compound, meaning every negative ion attracts every positive ion.

Ionic compounds form a giant ionic lattice structure. This means the ions are arranged in a repeating, three-dimensional pattern, extending throughout the entire compound.

Ionic compounds are solid at room temperature due to the strong electrostatic forces holding the ions together in the lattice. These forces require high energy to break, resulting in high melting points.

Ionic compounds don't conduct electricity as solids because the ions are fixed in the lattice. However, when molten or dissolved, the ions become free to move and can carry electric current.