Acid-Base Strength Quiz

A weak acid only partially dissociates in water, meaning that not all of its molecules break apart into ions.

The concentration of a solution, expressed as moles of solute per liter of solution.

The percentage of the initial acid molecules that have dissociated into ions in a solution.

A measure of the concentration of hydrogen ions (H+) in a solution, indicating its acidity or basicity.

An ionic compound composed of iron(III) cations and nitrate anions.

Solutions of iron(III) nitrate are acidic due to the hydrolysis of the nitrate ion.

The given order indicates acid strength decreases from HI to HCN.

The strongest acid's conjugate base is the weakest base.

Correct answer to the question regarding acidity.

The acidity of a solution can be determined by considering the nature of the dissolved substance.

The anion that accepts a proton (H+) least readily.

HI > HSO4- > HF > HCN

Hydriodic acid, a strong acid

Hydrogen sulfate ion, a moderately strong acid

The species formed when an acid loses a proton (H+)

After a strong base reacts, a strong conjugate base remains.

A strong conjugate base is formed when a strong base reacts.

At 450°C, tert-butyl alcohol breaks down into water and isobutene.

The decomposition reaction produces water and isobutene.

The decomposition of tert-butyl alcohol requires 450°C.

Changing the volume of a container holding a reaction at equilibrium affects the relative amounts of products and reactants to re-establish equilibrium.

Decreasing the volume of a reaction container containing gaseous substances will favor the side with fewer moles of gas to relieve pressure.

The stoichiometric ratios of gaseous substances in a balanced equation. Is crucial for volume changes.

A constant that relates the amounts of products and reactants at equilibrium. Independent of volume and pressure.

In the given reaction, the reverse reaction is favored to reestablish equilibrium when container volume reduces, leading to more products than reactants.

The pH of a 0.183 M aqueous solution of hypobromous acid (HOBr), given its acid dissociation constant (Ka).

The equilibrium constant for the dissociation of butyric acid in water, determining its strength as an acid.

The pH of a 0.25 M solution of butyric acid is 2.71.

A weak acid that partially dissociates in water.

The equilibrium constant for the dissociation of HO Br in water.

A measure of a weak acid's strength, indicating the extent of its ionization in solution.

Determine the acidity or basicity of a solution based on its hydrogen ion concentration.

The pH of a 0.183 M aqueous solution of hypobromous acid is related to the $K_a$ and concentration of HOBr.

Concentration of a solution expressed in moles per liter.

The method to determine the acidity constant from the pH of a solution.

The measure of acidity of a 0.183 M hypobromous acid solution, given its Ka value.

A weak acid that only partially dissociates in water.

The acid dissociation constant, a measure of the strength of a weak acid.

Aqueous solution of hypobromous acid with a concentration of 0.183 moles per liter.

Determining the acidity (H+ concentration) of a solution.

Changes that shift the equilibrium of the reaction, favouring the forward reaction, causing more $N_2$ to be produced

Increasing the total pressure on a gaseous system in equilibrium will shift the equilibrium to the side with fewer moles of gas.

Removing a reactant from the system in a reaction at equilibrium forces the reaction to shift toward the reactants to produce more of the removed substance

Adding a product to a reaction in equilibrium will shift the equilibrium toward the reactants.

For an exothermic reaction, decreasing the temperature shifts the equilibrium towards the products (heat is a product of the reaction).

A reaction at equilibrium shifts to the left when conditions favor the reverse reaction, increasing the concentration of reactants.

When a change in conditions (such as temperature, pressure, or concentration) is applied to a system in equilibrium, the system shifts its equilibrium position to counteract the change.

Adding more NOBr shifts the equilibrium to the left (toward reactants) by increasing the reactant concentration.

For an exothermic reaction at equilibrium, decreasing the temperature favors the forward reaction and thus increases the products at equilibrium.

Removing a product shifts the equilibrium to the right (toward products) to replenish the removed product.