acids/ bases Flashcards

Terms Definitions
Water
H₂O
C6H5NH2
wb
Amobarbital Sodium
WA/SB
hydrochloric acid
HCl
hydrofluoric acid
HF
HBr
hydrobromic acid
HI
strong acid
Weak Acid
HC9H8O4
CsOH
strong base
NaOH
strong base
H₂SO₄
Sulfuric acid
sulfuric acid
battery acid
cleaning
use of ammonia
Kb
base-dissociation constant
weak base+water
Ca (OH)2
strong base
Citric Acid
Oranges and lemons
H2SO4
sulfuric acid, strong acid
Bronsted-Lowry acid
a proton donor
slippery
how do bases feel?
less than 7
acidic solution
sodium hyrdoxide
NaOH strong base
Lewis base
donates electron pair; weak
pH stands for...
potential of Hydrogen
hydronium ion
hydrogen ion aka ________
Acids
taste sour, conduct electricity, recognized by an H+ ions
Acid
a substance that releases hydrogen (H+) ions when it dissolves
salt + H2O
acid + metal oxide
Nonelectrolyte
does not conduct electricity because it has not ions
Salts that produce acidic solutions contain ________ ions that release protons to water
positive
The pH of Acids
Less than 7
H2 SO4 - sulfuric acid
strong acid
Acid-carbonate reaction
produce carbon dioxide, water and salt.
what does pH stand for?
potential of hydrogen
diprotic acids
acids that contain two ionizable hydrogens
Binary Compound
A compound composed of 2 elements
litmus
What indicator turns blue in basic solution and red in acidic solution?
titration
delivering a measured volume of a solution of known concentration into the solution being analyzed
Hydrangea
different color based on pH of soil
bromthymol blue
yellow for acids, blue for bases
indicator
a device for showing the operating condition of some system
CO2 in body
dissolved 10%bicarb 65%carbamin Hbg 30%
Vitamin C
What is another name for ascorbic acid?
WEAK
when a solution is not concentrated so it has not got many particles mixed in with the water particles
strong acid
an acid that ionizes completely in aqueous solution
Neutralization reaction...
in a neutralization reaction an acid reacts with a base to produce a salt and water.
Oxy Acids
What contain hydrogen, oxygen, and one otehr element?
end point
the point at which the indicator changes color
Acids react with
bases to produce salts and water
Kidneys excrete K in echanges for___, controlled by ________.
Na, Aldosterone
Uses of Ammonia Solution
In Window Cleaning Solutions and Fertilisers
Weak Base
a base that partially ionizes in an aqueous solution. The scale goes from 11-14.
acids will become neutral when
an equal base is added
Particle formed when a base gains a H+.
Conjugate acid
H20
NH3 + H20 ==> NH4+ + OH-
The Bronsted Lowry acid is ______
Nsg Interventions for Hyper K?
Cardiac monitor, Kayexalate, Ca gluconate, IV insulin and IV D50, sodium Bicarb.
common ion effect
shift in position of an equilibrium on addition of a substance that provides an ion in common with one of the ons already involved in equilibrium; equilibrium is shifted in the direction that reduces the concentration of the common ion
lewis acid-base reaction
the formation of one or more covalent bonds between an electron-pair donor and an electron-pair acceptor
amphoteric compound
a compound that can either be an acid or a base
Hydrogen (H2), Nitrogen (N2), Oxygen (O2), Fluorine (F2), Chlorine (Cl2), and Bromine (Br2), and Iodine (I2)
Seven Nonmetal elements that are diatomic Elements, or molecular elements, two identical atoms
Bicarbonate Buffer System (Blood)
Optimum blood pH is 7.4 (normal range = 7.35 - 7.45).
Outside this range can be lethal.
Blood pH is modulated by levels of HCO3− & CO2.
Ratio of HCO3− (15mM) : CO2 (1.2mM) is 12:1 (pH 7.4).
What does CHEMO stand for ( in hyperphophatemis?)
Cardiac irregularites, Hyperreflexia, Eat poor, Muscle weakness, Oliguria
In metabolic acidosis, what happens with the K?
It enters the cell and HypOkalemia results.
the weak acid stays together
if there is a solution of a weak acid and a strong base what happens in the CIE?
Neutralize
...
saliva
6.5-6.9
PO4-3
phosphate
feel slippery
bases
NH3
Ammonia
weak base
aluminum hydroxide
deodorant
CH3COOH
Acetic Acid
Sr(OH)2
Stronium hydroxide
strong base
LiOH
SB Lithium Hydroxide
electrolytes
conductors of electricity
concentration of tritation:
MVN=MVN
conducts electricity (electrolyte); source of ions (hydroxide)
base
litmus paper
commercially prepared indicator
acid:
yields hydrogen cations, usually bonded to oxygen and other hydrogen.
soap
organic salts with nonpolar, hydrocarbon ends that interact with oils and dirt and polar ends that help them dissolve in water
base
-bitter taste/soapy feel
-litmus paper blue
-strong/weak electrolytes
-usually OH- (hydroxide) group, except those like NH3 (weak base)
autoprotolysis of water is an _________________ reaction
endothermic
In problems involving titration or neutralization of acids and bases, the equation to remember is:
NaVa=NbVb
diprotic
Acids that contain two ionizable hydrogen atoms per molecule.
any substance that increases the Hydroxide concentration
Bases
amphoteric
having characteristics of both an acid and a base and capable of reacting as either
Physical Properties
size, shape, color, density, melting point, boiling point
pH
a measure of the concentration of hydronium ions in a solution using a scale ranging from 0 to 14, with 0 being the most acidic and 14 being the most basic
Lewis acid
electron pair acceptor, e.g. H+ (+NH3)
Note: ammonium ion produced with covalent bond, H+ represents any Lewis acid
Oxyacid
An acid that is a compound of hydrogen, oxygen, and a third element, usually a nonmetal.
salt
an ionic compound composed of a cation from a base and an anion from an acid
What is Kw?
ion product constant of water (Kw=[H30+][OH-]); MUST EQUAL 1*10^-14
conjugate base
the particle that remains when an acid has donated a hydrogen ion
diprotic acid
an acid that can donate two protons per molecule.
Normal blood plasma bicarbonate level (HCO3)
- 21 -28 mmol
Ionic Compounds
made of metal and nonmetals OH- are released when dissovled in water
conjugate acid
the species that is formed when a Bronsted-Lowry base gains a proton
PHYSICAL CHANGE
A CHANGE IN THE SIZE, SHAPE, COLOR, OR STATE OF MATTER.
Industrially, Hydrochloric Acid is used to do what
"Pickling" iron and steel (acid solutions remove surface impurities
hydroxide ion (OH-)
a negative ion made of oxygen, and hydrogen
Classical Names - "ite"
If the anion ends in "ite," the acid will be:
name of polyatomic ion ending in "ous" + acid
example: HNO₂ - nitrous acid
Self Ionization of Water
H2O + H2O <=> H3O + OH-;
H2O => H+ + OH-
Is BCL3 a lewis acid or lewis base?
lewis acid because it has fewer than 8 e- in its valence shell and a lewis acid is defined as something that can accept e-.
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Term:
Definition:
Definition:

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