Acids, Bases, and Salts Online Test

A pH meter provides a digital, precise measurement of the hydrogen ion concentration, whereas color-based indicators provide only an estimate based on color changes.

In any aqueous solution, the product of hydronium and hydroxide ion concentrations is constant. If pH > 7, the solution is basic, meaning hydroxide ions outnumber hydronium ions.

Strong bases, such as sodium hydroxide (NaOH) or potassium hydroxide (KOH), are ionic compounds that dissociate completely to release hydroxide ions in water.

Monoprotic acids (like HCl) can be strong, but many (like acetic acid) are weak. The number of protons an acid can donate does not determine its strength.

Antacids are basic compounds that neutralize the excess hydronium ions (H3O+) responsible for the acidity in the stomach.

Stomach acid is primarily hydrochloric acid (HCl), not sulfuric acid (H2SO4).

The hydronium ion is the primary ion formed when an acid dissolves in water. While other ions exist in chemistry, the hydronium ion is the defining characteristic of acidic solutions in the Bronsted-Lowry and Arrhenius models.

Acids are chemically characterized by their sour taste. Bases are typically bitter, and salts vary in taste depending on their composition.

Bases are known for their bitter taste and slippery feel. Acids are sour, and salts are generally salty.

Concentration refers to the amount of solute per unit volume of solvent, which can be described as concentrated (high amount) or diluted (low amount). Strong and weak refer to the degree of dissociation of an acid or base.

The pH scale ranges from 0 to 14. Values above 7 indicate a basic solution, while values below 7 indicate an acidic solution.

The pH scale measures acidity and alkalinity. Values below 7 are acidic, and values above 7 are basic or alkaline.

The pH scale is the standard logarithmic scale used to specify the acidity or basicity of an aqueous solution.

The pH scale is logarithmic; a lower pH indicates a higher concentration of hydronium ions. Therefore, a pH of 8 has 10 times more hydronium ions than a pH of 9.

The strength of an acid is defined by its ability to dissociate and donate hydrogen ions (protons) in a solution.

Water molecules can self-ionize into hydronium ions (H3O+) and hydroxide ions (OH-).

A neutralization reaction occurs when an acid and a base react to form a salt and water.

The pH scale was developed by Søren Sørensen to provide a simple numerical way to express the concentration of hydrogen ions.

Salts are ionic compounds that result from the neutralization reaction between an acid and a base.

Litmus is a classic acid-base indicator that turns red in acidic conditions and blue in basic conditions.

According to the Arrhenius definition, a base is a substance that increases the concentration of hydroxide ions (OH-) in an aqueous solution.

Anthocyanins are water-soluble vacuolar pigments that appear red, purple, or blue depending on the pH.

The Bronsted-Lowry theory defines an acid as any species that is capable of donating a proton (H+).

Ionization is the process by which atoms or molecules acquire a negative or positive charge by gaining or losing electrons, often when dissolving in water.

The Bronsted-Lowry theory defines a base as any species that is capable of accepting a proton (H+).

The Arrhenius definition states that an acid is a substance that produces hydrogen ions (H+) when dissolved in water.

Hydrated refers to a substance that is combined with water or dissolved in an aqueous solution.

A pH indicator is a chemical compound that changes color when the pH of a solution changes.