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Acids & Bases: AP Chemistry

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Section 1

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Diprotic acid

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Chemistry Science

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Date created

Mar 1, 2020

Cards (40)

Section 1

(40 cards)

Diprotic acid

Front

An acid with two protons to donate

Back

Oxyacids

Front

Acids with a polyatomic ion that includes oxygen (e.g., HClO3)

Back

Neutral salt

Front

Contains the conjugate acid and base of a strong base and acid

Back

14.00

Front

= pH + pOH

Back

Weak acid (definition)

Front

A proton donor that does NOT completely dissociate in water

Back

Bronsted-Lowry base

Front

Proton (H+) acceptor

Back

pH

Front

expresses the acidity or alkalinity of a solution on a logarithmic scale, lower values are more acidic and higher values more alkaline. The pH is equal to −log [H+]

Back

Arrhenius base

Front

Generates hydroxide ions in aqueous solution

Back

Kw

Front

The equilibrium constant for the dissociation of water (1 x 10-14 at room temperature)

Back

Arrhenius acid

Front

Generates hydrogen or hydronium ions in aqueous solution

Back

Acid strength of oxyacids (number of oxygens)

Front

An oxyacid with more oxygen atoms is stronger than one with fewer (e.g. HClO is weaker than HClO3)

Back

Acid strength (atomic size)

Front

Acids with larger atoms tend to be stronger (e.g., HCl is stronger than HF)

Back

Hydronium ion

Front

H3O+

Back

Strong acids (names)

Front

Chloric, perchloric, hydrochloric, hydrobromic, hydroiodic, nitric, sulfuric

Back

Bronsted-Lowry acid

Front

Proton (H+) donor

Back

pOH

Front

-log[OH-]

Back

Monoprotic acid

Front

An acid with one proton to donate

Back

Strong bases (formulae)

Front

LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Ba(OH)2, Sr(OH)2

Back

Strong base (definition)

Front

A proton acceptor that completely dissociates in water

Back

autoionization of water

Front

pure water reacts with itself to form hydronium and hydroxide ions

Back

Polyprotic acid

Front

An acid with more than one proton to donate

Back

Acid strength (polarity)

Front

Acids that are more polar tend to be stronger (e.g. HCl is stronger than H2S)

Back

Basic salt

Front

Contains the conjugate base of a weak acid

Back

Lewis base

Front

Electron pair donor

Back

Strong bases (names)

Front

Lithium hydroxide, Sodium hydroxide, Potassium hydroxide, Rubidium hydroxide, Cesium hydroxide, Calcium hydroxide, Barium hydroxide, Strontium hydroxide

Back

Conjugate acid

Front

The acid product that results when a base accepts a proton

Back

Lewis acid

Front

Electron pair acceptor

Back

Triprotic acid

Front

An acid with three protons to donate

Back

Polyprotic acid equilibrium constants

Front

Each dissociation of a polyprotic acid has a different Ka value. Ka1 for the first dissociation is typically greater than Ka2

Back

Strong acids (formulae)

Front

HClO3, HClO4, HCl, HBr, HI, HNO3, H2SO4

Back

Ka

Front

The equilibrium constant for an acid dissociation in water. The larger the Ka, the stronger the acid

Back

Lewis acids that are not also Arrhenius or Bronsted-Lowry acids

Front

Metal cations (Al3+ or Cu2+)

Back

Relationship between Ka and Kb

Front

Kw = Ka * Kb

Back

Acidic salt

Front

Contains the conjugate acid of a weak base

Back

Conjugate base

Front

The base product that results when an acid donates a proton

Back

Kb

Front

The equilibrium constant for a base dissolving in water. The larger the Kb, the stronger the base.

Back

Strong acid (definition)

Front

A proton donor that completely dissociates in water

Back

Weak base (definition)

Front

A proton acceptor that does NOT completely dissociate in water

Back

Salt

Front

Any ionic substance

Back

Amphoteric substances

Front

Substances that can act as either an acid or a base (ex. NH3 or HSO4-)

Back