Acid-Base Chemistry Quiz

A substance that produces hydroxide ions (OH-) when dissolved in water.

The ability of a substance to act as a base can vary depending on the solvent it is dissolved in.

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

The study of chemical reactions and equilibrium involving substances dissolved in water.

The balance between the forward and reverse reactions in a chemical reaction.

The process where water molecules spontaneously split into hydrogen ions (H+) and hydroxide ions (OH-) in equal amounts.

In solutions of salts formed from strong acids and strong bases, the hydrogen ion concentration is solely determined by the dissociation of water molecules.

The concentration of hydrogen ions (H+) in pure water is 10^-7 M at 25°C.

A measure of the acidity or alkalinity of a solution. It is the negative logarithm of the hydrogen ion concentration (pH = -log[H+]).

Neither potassium ions (K+) nor chloride ions (Cl-) react with water to alter its hydrogen ion concentration.

The point in a titration where the moles of acid and base are equal, resulting in complete neutralization.

The pH at the equivalence point depends on the strength of the acid and base. For the reaction of a strong acid and strong base, the pH at the equivalence point is 7.00.

The pH at the equivalence point for a titration involving a weak acid and strong base will be greater than 7.00 due to the formation of the conjugate base of the weak acid.

The pH at the equivalence point for a titration involving a strong acid and weak base will be less than 7.00 due to the formation of the conjugate acid of the weak base.

A graphical representation of the pH of a solution as a function of the volume of titrant added during a titration.

A solution containing a weak acid and its conjugate base, or a weak base and its conjugate acid. Buffers resist changes in pH upon addition of small amounts of acid or base.

The region of a titration curve where the pH changes gradually as the titrant is added. This occurs when the weak acid and its conjugate base (or weak base and its conjugate acid) are present in significant amounts.

The quantitative analysis of the concentration of an analyte in a solution by reacting it with a solution of known concentration (titrant). The reaction is typically carried out until the equivalence point is reached, which can be determined using an indicator.

A substance that changes color in response to a change in pH, indicating the endpoint of a titration. The endpoint ideally coincides with the equivalence point.

The pH at the equivalence point is not 7 for the titration of a weak acid and strong base. It is greater than 7 because the conjugate base of the weak acid is a weak base, and it hydrolyzes water slightly to produce OH- ions, thus making the solution slightly basic.

The pH of a solution of a weak acid can be calculated using the Henderson-Hasselbalch equation, which relates the pH, pKa, and the concentrations of the weak acid and its conjugate base. This equation is particularly useful for calculating the pH of buffer solutions.

A titration method that uses the difference in solubility between two silver salts, AgCl and Ag2CrO4, to determine the chloride ion concentration. AgCl precipitates first due to its lower solubility, and the endpoint is indicated by the formation of a brick-red precipitate of Ag2CrO4.

An indirect method used to determine the concentration of silver ions (Ag+) or chloride ions (Cl-) by back titration. Excess silver nitrate (AgNO3) is added to precipitate chloride ions. The remaining silver ions are then titrated with potassium thiocyanate (KSCN) in the presence of iron(III) indicator. The endpoint is reached when a red complex (FeSCN2+) is formed, signaling the complete consumption of silver ions.

A method for determining the endpoint of a precipitation titration by using adsorption indicators. These indicators are organic dyes that adsorb onto the surface of the precipitate, leading to a color change at the equivalence point. For instance, dichlorofluorescein adsorbs onto silver chloride (AgCl), changing from green to pink at the equivalence point.

In the Fajans titration, prior to the equivalence point, there is an excess of chloride ions (Cl-) in solution. This excess Cl- will be adsorbed onto the surface of the AgCl precipitate. The adsorption of Cl- results in a negative charge on the surface of the precipitate, which attracts the positively charged indicator ions. As the titration progresses, the concentration of Cl- decreases, leading to a decrease in the adsorption of Cl- ions and a decrease in the indicator adsorption, thus signaling the endpoint.

This technique relies on the difference in solubility between two silver salts. AgCl precipitates first due to its lower solubility. The endpoint is indicated by the formation of a brick-red Ag2CrO4 precipitate.

A chemical compound that forms stable complexes with metal ions. It has six binding sites (hexadentate) and is commonly used in analytical chemistry, for example, to determine water hardness.

A chemical reaction where a metal ion and a ligand (like EDTA) combine to form a stable complex.

The strength of a complex is measured by its formation constant, also known as stability constant (KMY). A higher KMY indicates a more stable complex.

The pH-dependent form of EDTA that binds to metal ions most effectively. To calculate it, you consider all possible protonated and deprotonated forms of EDTA.

A factor that accounts for the pH-dependence of EDTA's ability to bind metal ions. It tells you the fraction of EDTA in its most reactive form (Y4-) at a specific pH.

The effective formation constant for a metal-EDTA complex at a specific pH. It considers the pH-dependent availability of the fully deprotonated form of EDTA (Y4-) and the overall stability constant (KMY)

The study of the equilibrium between different forms of a substance in solution, including the interaction of metal ions with ligands like EDTA.

The concentration of the total EDTA in solution, considering all possible protonated and deprotonated forms. It's used when calculating the conditional formation constant (KMY').