Acids and Bases 26 Flashcards

Terms Definitions
pOH=
-log[OH-]
BCl3
acid
HCl
Hydrochloric Acid
HClO3
weak acid
H2CO3
carbonic acid
HC2H3O2
Weak Acid
STRONGEST ACID
H₃0
HNO₃
nitric acid
LiOH
strong base
Acids taste
Sour
H2S
Hydrosulfuric Acid W
HI
hydroiodic acid SA
neutral substance
pure water
an acid increases
[H+]
HCN
hydrocyanic acid weak acid
acids
pH lower than 7
Acidic pH values
below 7
bases
Red litmus paper blue
ph
(chemistry) p(otential of) H(ydrogen)
concentrated
Acids can be dilute and?
Alkali + Acid
Salt + Water
HClO (hypochlorous acid)
Weak Acid (HA)
CH3OH
NOT AN ACID OR BASE
What is released when acids Dissolve
Hydrogen
Acid
A substance that produces hydrogen ions in an aqueous solution; proton donor
Acidic
Worker Bee Stings are ____ (acidic/basic)
Strong acids dissociate into ions ....%
100
acid dissociation constant
[H^+][conjugate base] / [acid]
H+ is what?
OH - is what?
high
low
renal tubular acidosis
METABOLIC ACIDOSIS
NORMAL ANION GAP
Amphoteric
substance that can behave as either acid or base EX-water
neutral
Something that is neither acidic nor alkaline but in the middle! pH7
endpoint
the point at which the indicator changes color
HCL HBr HI HCLO4 HCLO3 H2SO4 HNO3
acids
strong bases
hydroxides of alkali and alkaline earth metals. All exhibit a high rate of dissociation making them good electrolytes.
neutralization
a chemical reaction between an acid and a base
Whenever ammonia forms a covalent bond, it acts as a
Lewis base
What is normal PaO2?
80 - 100 mmHg
Arrhenius Base
Gives off Hydroxide ions in an acid-base reaction
Bronsted-Lowry base
receives an H+; has a conjugate; weak
strong acids
HCl, HBr, HI, HNO3, HClO4, HClO3, H2SO4 (the first)
Combustibility
the ability of materials to burn in the presence of oxygen
Conjugate base
the species formed when an acid transfers a proton to a base
Who proposed that an acid accepts a pair of electrons during a reaction?
Lewis
what does a higher Ka indicate?
a stronger acid
Bleach Stains
Removes stains by removing the color from the unwanted stain by oxidizing the compound.
acid + base --> ? + ?
water + salt
Bronsted-Lowry acid base reaction
protons are transferred from one reactant (acid) to another (base)
acid ionization constant
the value of the equilibrium constant expression for the ionization of a weak acid
bronsted lowry acid
substance that donates a proton, needs H+
end point
what is the point at which the indcator shows that neutralization has taken place called?
name the following anions and their conjugate acids. ClO-, ClO2-,ClO3-,ClO4-, NO2-,NO3-.
hypochlorite/hypochlorous acid, chlorite/chlorous acid, chlorate/chloric acid, perchlorate/perchloric acid, nitrite/nitrous acid, nitrate/nitric acid
strong acid
yields a weak conjugate base - one that has a low affinity for a proton
conjugate acid-base pair
consists of two substances related by the loss or gain of a single hydrogen ion
basic solutions
Salts derived from a strong base and a weak acid.
Neutralization Reactions
what is the process of mixing an acid with a base of equal strength to produce a neutral product. the resulting solution has neither the properties of an acid nor a base
The substances produced when KOH(ap) neutralizes HCI(aq) are
H2O (l) and KCI (aq)
conjugate acid
an acid that forms when a base gains a proton
Bronstred-Lowry model
A model of acids and bases in which an acid is a hydrogen-ion donor and a base is a hydrogen-ion acceptor.
Do liquids factor into a Ka, Kb or Keq problem?
No, only Aq
The equation for acids reacting with metals is:
Zn + 2HCl -> ZnCl2 + H2
how does putting an acid or base in water measure strength?
the better separated the hydrogen ions are, the stronger it is
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