Chemistry: Acids, Bases, and Salts Study Guide

These flashcards cover key concepts about acids, bases, and salts based on the study guide notes.

What are the properties of substances recognized as acids?

Acids have a sour taste, change litmus from blue to red, and liberate hydrogen gas when metals dissolve.

What are the properties of substances recognized as bases?

Bases have a bitter taste, change litmus from red to blue, dissolve fats, and feel slippery.

Define an Arrhenius acid.

An Arrhenius acid is a hydrogen-containing compound that produces hydrogen (H1+) ions when dissolved in water.

Define an Arrhenius base.

An Arrhenius base is a hydroxide-containing compound that produces hydroxide (OH1-) ions when dissolved in water.

What ion is responsible for the acidic behavior of an acid according to Arrhenius theory?

The hydrogen ion (H1+) is responsible for the acidic behavior of an acid.

What ion is responsible for the basic behavior of a base according to Arrhenius theory?

The hydroxide ion (OH1-) is responsible for the basic behavior of a base.

Explain the difference between ionization of Arrhenius acids and dissociation of Arrhenius bases.

Arrhenius acids undergo ionization to form ions from a molecular compound, while Arrhenius bases dissociate, separating existing ions in an ionic compound.

Is HNO3(aq) → H1+(aq) + NO31-(aq) an Arrhenius acid or base reaction?

This is an example of an Arrhenius acid reaction.

Is RbOH(aq) → Rb1+(aq) + OH1-(aq) an Arrhenius acid or base reaction?

This is an example of an Arrhenius base reaction.

What are two limitations of the Arrhenius acid-base theory?

It is restricted to aqueous solutions and does not explain basicity from compounds lacking hydroxide ions.

Define a Bronsted-Lowry acid.

A Bronsted-Lowry acid is any substance that can lose a hydrogen ion (H1+) to another substance.

Define a Bronsted-Lowry base.

A Bronsted-Lowry base is any substance that can accept a hydrogen ion (H1+) from another substance.

Why must a Bronsted-Lowry acid involve a Bronsted-Lowry base in a chemical reaction?

When a Bronsted-Lowry acid loses a hydrogen ion, that ion must be accepted by a substance, thus a base must be present.

What is a hydronium ion and how is it formed?

A hydronium ion (H3O1+) is formed when a water molecule accepts a hydrogen ion (H1+).

What structural requirement must all Bronsted-Lowry acids have?

A Bronsted-Lowry acid must have at least one hydrogen atom that can be lost and converted into a hydrogen ion (H1+).

What structural requirement must all Bronsted-Lowry bases have?

A Bronsted-Lowry base must have at least one lone pair of electrons available to bond with a hydrogen ion (H1+).

What does amphiprotic mean in the context of Bronsted-Lowry theory?

Amphiprotic means a substance can both accept and lose a proton (H1+).

What identities can we assign to NH3(aq) + H3PO4(aq)?

Bronsted-Lowry acid is H3PO4 (loses H1+), Bronsted-Lowry base is NH3 (gains H1+).

What identities can we assign in HSO41-(aq) + H2O(l)?

Bronsted-Lowry acid is HSO41- (loses H1+), Bronsted-Lowry base is H2O (gains H1+).

What is a conjugate acid?

A conjugate acid is the chemical species formed when a hydrogen ion (H1+) is accepted by a Bronsted-Lowry base.

What is a conjugate base?

A conjugate base is the chemical species formed when a hydrogen ion (H1+) is lost by a Bronsted-Lowry acid.

Identify acid, base, conjugate acid, and conjugate base in H2C2O4 + ClO1- ⇄ HC2O41- + HClO.

Acid: H2C2O4, Base: ClO1-, Conjugate Acid: HClO, Conjugate Base: HC2O41-.

Identify acid, base, conjugate acid, and conjugate base in H3PO4 + PO43- ⇄ H2PO41- + HPO42-.

Acid: H3PO4, Base: PO43-, Conjugate Acid: H2PO41-, Conjugate Base: HPO42-.

What is the equilibrium constant for the autoionization of water?

Keq = [H3O1+][OH1-] = 1.00 x 10-14.

How is pH calculated?

pH = -log([H3O1+]) indicates the hydronium ion concentration in a solution.

How is pOH calculated?

pOH = -log([OH1-]) indicates the hydroxide ion concentration in a solution.

What is the relationship between pH and pOH?

pH + pOH = 14.

What is the hydroxide ion concentration ([OH1-]) of a solution if [H3O1+] is 2.250 x 10-6?

[OH1-] = 4.444 x 10-9.

What is the concentration of a 25.00 mL HCl solution neutralized by 25.250 mL of 0.250 M NaOH?

The concentration of HCl is [HCl] = 0.253 M.

What is the concentration of a 25.00 mL H2CO3 acid solution neutralized by 35.750 mL of 0.350 M KOH?

The concentration of H2CO3 is [H2CO3] = 0.251 M.