Chemical Solutions and Salts Quiz

A solution containing two or more acids with the same hydrogen ion concentration. This means their [H+] is equal, even if the acids have different strengths or concentrations.

A salt formed when a base neutralizes all the acidic hydrogen atoms of a polyprotic acid.

A salt formed when a base neutralizes only part of the acidic hydrogen atoms of a polyprotic acid. This leaves some acidic hydrogen atoms remaining in the salt.

A salt formed when a base is partially neutralized by an acid. This results in a salt containing OH⁻ ions.

A salt formed by the combination of two or more salts. It's a single compound containing multiple cations and anions.

A salt containing a complex ion, a central metal ion surrounded by ligands (typically neutral molecules or anions) bonded to it.

The maximum concentration of a solute that can dissolve in a given solvent at a specific temperature.

The product of the ion concentrations raised to their stoichiometric coefficients in a saturated solution of a sparingly soluble salt. This is a constant value at a given temperature.

A solution's ability to resist pH changes when small amounts of strong acid or base are added. It typically consists of a weak acid and its conjugate base or a weak base and its conjugate acid.

The equilibrium constant that governs the solubility of a sparingly soluble ionic compound. It is the product of the ion concentrations raised to their stoichiometric coefficients. For example, for CaF2(s), Ksp = [Ca2+][F-]^2.

A measure of the extent to which a reaction proceeds to completion. A higher degree of dissociation indicates that more reactants have converted into products which is usually the case with stronger acids.

The law states that if a change of condition (concentration, temperature, pressure) is applied to a system at equilibrium, the system will shift in a direction that relieves the stress.

An equilibrium constant expressed in terms of partial pressures of gaseous reactants and products. It specifically applies to reactions involving gases in equilibrium.

A pair of chemical species that differ by a single proton. The acid donates a proton and the base accepts a proton to form conjugate pairs.

The ratio of the equilibrium concentration (partial pressure) of a particular reactant or product to its initial concentration (partial pressure). It indicates the extent to which that species has reacted.

The pH of a buffer solution can be calculated using the Henderson-Hasselbalch equation: pH = pKa + log(base/acid). The pKa is the negative logarithm of the acid dissociation constant (Ka).

The change in the number of moles of gaseous reactants and products during a reaction. It determines the effect of pressure changes on equilibrium.

The reaction will shift to the side with fewer moles of gas to relieve pressure.

The reaction will shift to the side with more moles of gas to relieve pressure.

The reaction will not shift, regardless of pressure changes.

The ratio of product concentrations to reactant concentrations, each raised to their stoichiometric coefficients, at any point during a reaction, but not at equilibrium.

Qc = Kc. The reaction is at equilibrium.

Qc > Kc. The reaction will shift backward (to the left) to reach equilibrium.

Qc < Kc. The reaction will shift forward (to the right) to reach equilibrium.

The negative logarithm of the hydrogen ion concentration ([H+]) in a solution. It measures the acidity of a solution.

The negative logarithm of the hydroxide ion concentration ([OH-]) in a solution. It measures the basicity of a solution.

The product of the hydrogen ion concentration ([H+]) and the hydroxide ion concentration ([OH-]) in a solution. It is a constant value at a given temperature. The higher the temperature the higher the value.

The pH of a solution containing only a strong acid, where the [H+] is solely determined by the acid's concentration.

The pH of a solution containing a weak monobasic acid. This involves calculating the [H+] based on the acid's ionization constant (Ka) and concentration.

The pH of a solution containing a weak polybasic acid. This involves considering the multiple ionization steps and their respective Ka values.

The pH of a solution containing a mix of two strong acids or one strong acid and one strong base.

The pH of a solution containing a weak acid (WA) and a strong acid (SA) is determined by the stronger acid, but the weak acid also contributes slightly to the [H+].

Calculating the pH of a solution containing a weak base (WB) and a strong base (SB) is similar to determining the pH of a WA and SA mix. The stronger base dominates the [OH-] while the weaker base impacts it minimally.

Amphiprotic species can act as both an acid and a base, depending on the conditions. When determining the pH of an amphiprotic salt solution, consider the relative values of K1 and K2 to find the predominant acidic/basic form.

The pH of a salt solution is determined by the hydrolysis of the ions it contains. Anionic hydrolysis occurs when an anion reacts with water, resulting in a basic solution. Cationic hydrolysis involves a cation reacting with water, producing an acidic solution.

Salts formed from weak acid and strong base reactions are basic due to anionic hydrolysis, while those from strong acid and weak base reactions are acidic due to cationic hydrolysis.