Acids and Bases Flashcards
Do not mix: ____ and ____
* Produces chlorine gas which can cause coughing, breathing problems, burning and watery eyes.
Bleach and Vinegar
Do not mix: ____ and ____
* Produce a toxic gas called chloramine that causes shortness of breath and chest pain.
Bleach and Ammonia
Do not mix: ____ and ____
* Makes chloroform which is highly toxic.
Bleach and Rubbing Alcohol
Do not mix: ____ and ____
* This combination makes peracetic or peroxyacetic acid which can be highly corrosive.
Hydrogen Peroxide and Vinegar
- Prefix hydro- is used to represent hydrogen, followed by the name of the nonmetal with its ending replaced by the suffix –ic and the word acid added.
- HCl: Hydrochloric Acid
- HBr: Hydrobromic Acid
Naming Binary Acids
- Replace hydrogen with a metal = oxysalt.
- A salt is a compound consisting of a metal and a non-metal.
- If the salt consists of a metal, a nonmetal, and oxygen it is called an oxysalt.
Naming Oxyacids and Oxysalts
Acid: H+ or H3O+ producer.
Base: OH- producer.
Arrhenius Definition
Acid: Proton (H+) donor.
Base: Proton (H+) acceptor.
Bronsted-Lowry Definition
Acid: Electron-pair acceptor.
Base: Electron-pair donor.
Lewis Definition
- Earliest acid-base definition, which classifies these substances in terms of their behavior in water.
- Acid is a substance with H in its formula that dissociates to yield H3O+
- Base is a substance with OH in its formula that dissociates to yield OH-
Arrhenius Acid-Base Definition
When an acid reacts with a base.
Neutralization
- Acid that dissociates completely into ions in water.
- Its dilute solution contains no HA molecules.
Strong Acid
- Acid that dissociates slightly to form ions in water.
- Its dilute solution, most HA molecules are undissociated.
Weak Acids
Indication of acid strength.
Value of Ka
- Stronger acid: higher H3O+ = ____ Ka.
- Weaker acid: lower % dissociation of HA = ____ Ka.
Larger; Smaller
- Acid is a proton donor, any species that donates an H+ ion. Acid must contain H in its formula.
- Base is a proton acceptor, any species that accepts an H+ ion. Base must contain a lone pair of electrons to bond to H+
Bronsted-Lowry Acid-Base Definition
Acid-base reaction.
Proton-transfer Process
A Brønsted–Lowry acid must contain a ____ atom.
Hydrogen
- Make neutral compounds bases.
- (N)H3 - ammonia
- H2(O) - water
Lone Pairs
- Base in each metal salt.
- Na(OH) - sodium hydroxide
- K(OH) - potassium hydroxide
- Mg(OH)2 - magnesium hydroxide
- Ca(OH)2 - calcium hydroxide
OH-
Product formed by loss of a proton from an acid.
Conjugate Base
Product formed by gain of a proton by a base.
Conjugate Acid
Depends on the relative strength of the acids and bases involved.
Net Direction of an Acid-Base Reaction
The stronger the acid is, the ____ its conjugate base.
Weaker
When an acid reacts with a base that is farther down the list, the reaction proceeds to the ____ (Kc > 1).
Right
- A compound that contains both a hydrogen atom and a lone pair of e−.
- It can be either an acid or a base.
Amphoteric Compound
Process where water dissociates very slightly into ions in an equilibrium.
Autoionization or Self-Ionization
Acid dissociation constant.
Ka
Ion-product constant for water.
Kw
- A change in [H3O+] causes an ____ change in [OH-], and vice versa.
- Higher [H3O+] = lower [OH-]
- Higher [OH-] = lower [H3O+]
Inverse
- Acidic solution: ____ [H3O+]
- Neutral solution: ____ [H3O+] and [OH-]
- Basic solution: ____ [OH-]
- Higher
- Equal
- Higher
- pH of a solution indicates its relative acidity.
- ____: pH < 7.00
- ____: pH = 7.00
- ____: pH > 7.00
- Acidic
- Neutral
- Basic
Higher the pH, the ____ the [H3O+] and the ____ acidic the solution.
Lower; Less
A low pKa corresponds to a ____ Ka.
High
If pH increases, pOH ____.
Decreases
A solution whose pH changes very little when acid or base is added.
Buffer
Most buffers are solutions composed of roughly equal amounts of
Weak Acid and Salt of its Conjugate Base
Added ____, OH− reacts with the weak acid.
Base
Added ____, H3O+ reacts with the conjugate base.
Acid
If an ____ is added to the following buffer equilibrium, then the excess acid reacts with the conjugate base, so the overall pH does not change much.
Acid
If a ____ is added to the following buffer equilibrium, then the excess base reacts with the conjugate acid, so the overall pH does not change much.
Base
Effective pH range of a buffer depends on its ____.
Ka
Normal blood pH is between ____ and ____.
7.35 and 7.45
- Results when the body fails to eliminate enough CO2, due to lung disease or failure.
- Lower RR = increases [CO2]
Respiratory Acidosis
- Caused by hyperventilating; very little CO2 is produced by the body.
- Faster RR = decreases [CO2]
Respiratory Alkalosis
