Definitions
This type of acid increases the concentration of H⁺ in solution.
Arrhenius Acid
Acid/base strength depends on this.
Complete Ionization/Dissociation
The equation used to calculate pH from hydronium concentration.
pH = –log[H₃O⁺]
Products of a neutralization reaction.
water and salt
In HCl + NH₃ → NH₄⁺ + Cl⁻, the conjugate acid is this.
NH₄⁺
This type of base increases the concentration of OH⁻ in solution.
Arrhenius Base
A substance that ionizes 100% in water is classified as this.
Strong Acid
If pH = 3.4, what is pOH?
10.6
Type of reaction that acid-base reactions are classified as.
Double Replacement
In CH₃COOH + OH⁻ → CH₃COO⁻ + H₂O, the conjugate base is this.
CH₃COO⁻
A substance that donates a proton (H⁺) is called this.
Bronsted-Lowry Acid
A weak acid would show this in a particle diagram.
Mostly Undissociated Molecules with Few Ions
If [H⁺] = 1.0 × 10⁻⁶ M, what is the pH?
6
In the reaction of hydrofluoric acid and potassium hydroxide, potassium fluoride and water are produced. What is the salt?
KF or potassium fluoride
A solution that resists changes in pH is called this.
Buffer
Water acting as both an acid and a base is described by this term.
Amphoteric
As pH increases, hydronium ion concentration does this.
Decreases
If [OH⁻] = 3.5 × 10⁻⁷ M, what is the pH (approx)?
7.5
Strong acid + strong base reactions do this.
Go to completion
Buffers are made from these two components.
Weak acid/base and its salt
In the reaction NH₃ + H₂O → NH₄⁺ + OH⁻, identify the base.
NH₃
A solution with a pOH of 1 is classified as this. (include strength)
Strong Base
A solution goes from pH 4 to pH 6. The [H₃O⁺] changes by this factor.
100x or 102
Why weak acid + weak base reactions typically don’t go to completion.
Neither donates or accepts enough H+
In NH₃ + H₂CO₃ → HCO₃⁻ + NH₄⁺, identify the acid.
H₂CO₃