| Terms |
Definitions |
|
Ampetamine
|
WB
|
|
acid
|
HCl
|
|
?
|
...
|
|
HNO3
|
Nitric Acid
|
|
Mg(OH)2
|
weak base
|
|
HCl
|
hydrochloric acid
|
|
CH3COOH
|
acetic acid
|
|
NaHCO₃
|
Bicarbonate (ion)
|
|
H3C6H5O7
|
acid-citric acid
|
|
NaOH
|
Sodium Hydroxide S
|
|
Weak acid
|
dissociates partially
|
|
Aqueous
|
solution mainly water
|
|
Acidic
|
Strong Acid+Weak Base
|
|
Bronsted-Lowry acid
|
a hydrogen-ion donor
|
|
sour taste
|
acids have a
|
|
Arrhenius acids
|
increased proton concentration
|
|
accept hydrogen
|
bronsted lowry base
|
|
Citric Acid
|
Oranges and lemons
|
|
strong bases
|
dissociate completely in water
|
|
corrosive
|
eating away gradually, acidlike; bitterly sarcastic
|
|
Acids react with _______
|
many metals
|
|
Acids and Bases
|
Examples of inorganic compounds
|
|
Ternary
|
Contains a polyatomic ion. H₃Po₄ or H₂So₄ are examples.
|
|
DISSOCIATION
|
separation or disintegration of a substance to atoms or ions.
|
|
electrolyte
|
substance that conducts an electric current when it is dissolved in water
|
|
Bases
|
Taste bitter, feel slippery, conduct electricity, may be corrosive and cause burns, react with chemicals to produce predictable color changes.
|
|
salt
|
a compound formed by replacing hydrogen in an acid by a metal (or a radical that acts like a metal)
|
|
sulfuric acid
|
H2SO4 strong acid
|
|
weak acids
|
hold onto their protons in water
|
|
neutralization
|
the reaction of hydronium ions and hydroxide ions to form water molecules
|
|
Arrhenius base
|
chemical compound that increases the concentration of hydroxide ions, OH-, in a an aqueous solution.
|
|
equilibrium
|
a chemical reaction and its reverse proceed at equal rates
|
|
What occurs to breathing when pH rises?
|
hypoventilation
|
|
Neutral
|
an equal number of hydrogen and hydroxide ions and has no charge
|
|
Types of Acids
|
carbonic- fizzy drinks, tanic-tea, citric-lemon, Absorbic-Vitamin C, Ethnoic-vinegar.
|
|
soap
|
a cleansing agent made from the salts of vegetable or animal fats
|
|
Acid Solutions
|
Salts with small, highly charged metal cations (e.g. Al3+, Cr3+, and Be2+) and the conjugate base of a strong acid.
|
|
organic acid
|
COOH; they are weak, example: acedic acid
|
|
common acids
|
HCl = hydrochloric acid
HNO3 = nitric acid
H2CO3 = carbonic acid
H2SO4 = sulfuric acid
HC2H3O2 = acetic acid
H3PO4 = phosphoric acid
|
|
conjugate acid
|
formed when proton is transferred to base
|
|
____ bases react with water to form the hydroxide ion and the conjugate acid of the base
|
weak
|
|
Buffer
|
A solution that resists change in pH when limited amounts of acid or base are added.
|
|
triprotic acid
|
any acid that contains 5 ionizable protons
|
|
Bronsted-Lowry
|
An acid is any substance that can donate H+ ions.
A Base is any substance that can accept H+ ions
|
|
OH
|
Bases often have ____ at the end of them (Chemical formula)
|
|
balsamic vinegar is made from
|
a specific type of grape
|
|
Covalent Bond
|
A type of chemical bond formed by atoms when they share electrons
|
|
oxyacid
|
an acid that is a compoud of hydrogen, oxygen, and a third element, usually a non-metal
|
|
Equivalence point in titration of weak base
|
ph < 7
|
|
acid base indicator
|
chemical dye whose color is affected by acidic and basic solutions
|
|
3 Factors of solubility
|
pressure, type of solvent, and temp
|
|
Lewis Base
|
Donate a pair of electrons to form a dative bond
|
|
Who's What in Terms of pH?
|
Classify various solutions according to their pH levels Arrange the different substances in order of the prediction of their pH level Prediction - pH result
Lemon Juice-1 Vinegar-2
Apple Juice-4 Orange Juice-3
Coke-4 Tap Water-6
Bleach-7 Sodium Hydroxide-12
Detergent-10 Acetic Acid-2
Ammonia-12 I learned the difference between acids and bases and which substances go in each category and pH level
|
|
Ca(OH)₂, Sr(OH)₂, Ba(OH)₂
|
Name all the Group 2 Metals strong bases in descending order.
|
|
What does the pH measure?
|
Measure of the hydrogen ion concentration in a solution
|
|
Baking powder is bicarbonate plus
|
1. dry acid (single acting)
2. dry acids (double acting)
|
|
what can affect shapes of molecules and affect chemical reaction rates?
|
the acidity of the environment
|
|
Base strength is determined by..?
|
how many hydroxide ions break off in water.
|
|
ionization constant; gives the relative strength of an acid
|
Each acid has a specific Ka, __, which ...?
|
|
A Bronsted-Lowry base is defined as a substance that __.
|
acts as a proton acceptor in any system
|
|
Thiophenol
|
WA
|
|
base
|
KOH
|
|
acetic acid
|
vinegar
|
|
H+
|
hydrogen ions
|
|
HClO4
|
perchloric acid
|
|
HBr
|
Hydrobromic Acid
|
|
strong
|
many ions
|
|
Ca(OH)2
|
Strong Base
|
|
H2so4
|
Sulfiric car batteries
|
|
phenolphthalein acid color
|
clear
|
|
Bases taste ________.
|
bitter
|
|
6 Strong Acids
|
HI
HCl
HBr
H2SO4
HNO3
H3O
|
|
H2CO3
|
Carbonic acid carbonated water
|
|
BDH
|
bronsted/lowry acid donates H+
|
|
Bronstead-Lowry base
|
a proton reciever
|
|
Molality Formula
|
Moles solute/L solution
|
|
Do bases react with carbonates?
|
no
|
|
Lewis acid
|
accepts an electron pair
|
|
bases will dissolve
|
fats and oils
|
|
Aqueous solutions
|
have a sour taste
|
|
esters
|
used widely in flavors and perfumes
|
|
NH2-
|
name the conjugate base of NH2
|
|
indicator
|
(chemistry) a substance that changes color to indicate the presence of some ion or substance
|
|
arrhenius
|
This definition states that acids produce H+ in solution, and Bases produce OH- in solution.
|
|
Name a K sparing diuretic.
|
Spironolactone
|
|
Arrhenius acid
|
produces H+ ions in a solution
|
|
Titration
|
An analytical method used to determine the amount of acid (or base) in a solution by adding known amounts of a base (or acid) and observing its effect on the pH of the solution.
|
|
Fe3+ ions in solution would decrease the pH
|
true
|
|
pH 3
|
Very Acidic ( Lemon Juice )
|
|
a substance that decreases the number of H+ ions.
|
base
|
|
Strong Acids
|
HCl, Hl, HBr, H2SO4, HNO3, HClO4
|
|
Halogen Acids
|
Simple structured acids in which a halogen ion is singly bonded to Hydrogen ion (i.e. HF)
|
|
cabbage juice
|
color on a chart (number) natural indicator
|
|
Can be strong or weak electrolytes in aqueous solution
|
Acid
|
|
hydroniumion
|
the hydrogen ion bonded to a molecule of water, h3o+, the form in which hydrogen ions are foind in aqueous solution
|
|
strong acid
|
an acid that is almost completely ionized in an aqueous solution
|
|
protonation
|
the addition of an acid's H+ ion (proton) to a water molecule to form hydronium (H3O+)
|
|
red litmus paper
|
in a base this will turn blue
|
|
taste bitter and chalky, are electrolytes, feel soapy and slippery, react with acids to form salts and water
|
bases _________, ___________, _________, and _________
|
|
basic solutions
|
Rules for salts: Strong Base + Weak Acid =
pH>7
|
|
Conjugate Base
|
member of conjugate pair with one less H+
|
|
end point
|
the point at which the indicator that is used in a titration changes color
|
|
Unsaturated solubility
|
If you can continue to dissolve more solute
|
|
THE BRONSTED-LOWRY MODEL
|
an acid is always the substance that donates a proton to another substance and base is always the substance that accepts the proton.
|
|
more acidic
|
On a pH, the numbers 6-1 are: acidic, basic, or neutral
|
|
Bronsted-lowry model
|
an acid is a hydrogen-ion donor and a base is a hydrogen ion to a base
|
|
taste sour, corrode metals, react with bases to form salts and water
|
acids ________, ______, and __________
|
|
properties of acids and bases
|
react with one another to produce a salt and water, conduct electricity, change color of indicator
|
|
Hybridization and the % s character of the atom bearing the negative charge
|
the greater s-character of a hybridized atom, the more acidic the bonded hydrogen is; electrons in s orbitals are lower in energy and closer to the nucleus than ones in p orbitals; less orbital overalap; therefore, the more s character in a hybrid orbital, the more electronegative the atom will be, and the more acidic a hydrogen bonded to it will be (and the more stable the anion will be); sp3 = 25% s, sp2 = 33% s, sp = 50% s
|
|
reaction between an active metal and water; reaction between salt and another base; reaction between a basic anhydride (metallic oxide) and water
|
How do we prepare bases? (3 ways) [Ex. 2NA(s) + 2 H₂O(l) => 2NAOH(aq) + H₂(g)], [Ex. Na₂CO₃(aq) + Ca(OH)₂(aq) => 2 NaOH(aq) + CaCO₃(s)], [Ex.CaO(s) + H₂O(l) => Ca(OH)₂(s)]
|
|
9
|
Nona
|
|
Malic Acid
|
Apples
|
|
weak base
|
pH8
|
|
Al(OH)3
|
ALUMINUM HYDROXIDE
|
|
Sr(OH)2
|
strontium hydroxide
|
|
H2SO3
|
Sulfurous Acid W
|
|
phenolphthalein base color
|
pink
|
|
A strong acid
|
HNO3
|
|
Solution is Neutral
|
pH=7
|
|
PH SCALE >7 ??
|
ACID
|
|
Bronsted Lowry acid
|
proton donor
|
|
Whic molecule is larger
|
plolysaccharide
|
|
Strong bases are
|
strong electrolytes
|
|
chemical indicator
|
red and blue litmus
|
|
from [OH-] to pOH
|
-log [OH-]
|
|
phenolphthalein turns
|
purple in a base
|
|
1 x 10^-14
|
[OH-] x [H+] (Kw)
|
|
red to orange
|
pH paper - acids
|
|
What is SIADH
|
Syndrome of Inappropriate ADH
|
|
amphoteric
|
having characteristics of both an acid and a base and capable of reacting as either
|
|
acidic solution
|
When H+ is greater than OH-
|
|
pH
|
The negative logarithm of the hydrogen ion concentration of a solution; acidic solutions have pH values between 0 and 7, basic solutions have values between 7 and 14, and a solution with a pH of 7.0 is neutral.
|
|
Acidic Marinades
|
Can be used to tenderize meats.
|
|
Examples of Bases
|
soap, milk, milk of magnesia
|
|
Weak bases
|
___ ionize only partially in dilute aqueous solution.
|
|
Neutralization Reaction
|
HA + BOH -> BA + H2O
|
|
monomer
|
each link in a polymer is called a
|
|
O2-
|
strongest base EVER (so strong that it automatically produces hydroxide no matter what its added to)
|
|
Molarity
|
a measure of concentration of an acid or base, equal to moles of solute per liter of solution
|
|
A base is a source of ______________ ions
|
hydroxide
|
|
tenfold difference
|
between each whole number of the pH scale there is a __ in hydrogen ion concentration
|
|
pH scale
|
use to measure the strength of acids and bases
|
|
monoprotic acid
|
an acid that can donate only one proton (hydrogen ion) per molecule
|
|
Polyprotic Acids
|
have multiple H+ ions; more H+ means stronger acid
|
|
Bronsted-Lowry Base
|
a molecule or ion that is a proton acceptor
|
|
CONJUGATE ACID-BASE PAIR
|
a substance that differ only in the presence or absence of a proton. every acid has a conjugated base formed by a removal of a proton. and every base has a conjugated acid formed by the addition of a proton.
|
|
When an acid and base are mixed, the ____________ _________ is when the number of moles of hydrogen ions equals the number of moles of hydroxide ions
|
equivalence point
|
|
13g of salt and 100ml of water =
|
13% saltwater concentration
|
|
neutralization reactions
|
the reaction of an acid with a base to produce a salt and water
|
|
ion product constant for water
|
the value of the equilibrium constant expression for the self-ionizarion of water.
|
|
Water can act as...
|
(either) an acid or a base. (It can also) auto-ionize.
|
|
Bronsted-lowry acids and bases
|
an acid is a proton donor and a base is a proton acceptor.
|
|
What type of type of salt produces an acidic solution? One that contains ________ ____ _____ _______ ____________ _____ __________
|
positive ions that release protons to water
|
|
Urine
|
6
|
|
pOH
|
-log[OH]
|
|
LiOH
|
Strong Base
|
|
KOH
|
potassium hydroxide
|
|
diprotic acids
|
H2SO4
|
|
Bases taste
|
bitter
|
|
acids
|
neutralize bases
|
|
NH4+
|
Weak Acid
|
|
C_5H_5N
|
pyridine (Weak Base)
|
|
color turns phenolphthalein-base
|
pink
|
|
Strong base
|
Strong/Weak Base/Acid?
LiOH
|
|
diuretic therapy
|
METABOLIC ALKALOSIS
CHLORIDE-SENSITIVE
|
|
universal indicator original color
|
orange
|
|
reacts with metals (corrosive/poisonous to skin)
|
acid
|
|
cirtic acid
|
found in fruits
|
|
bronsted-lowery base
|
accept a proton
|
|
HClO3
|
Strong acid H+(aq) + ClO3-(aq)
|
|
Group 1 Alkli Metals
|
Strong Base
|
|
NaOH and RbOH
|
which are strong bases?
|
|
Phenolphtalein
|
colorless in acid; pink in base
|
|
What is respondsible for the appearance of what appears to be un-altered plant material in animal feces?
|
cellulose
|
|
Conduction
|
Heat moving between objects that are touching.
|
|
properties of acids
|
- sour taste
- corrosive
- electrolytes
- react with indicator to produce a color change
|
|
Said that bases are compounds that ionize to yield hydroxide ions (OH-) in aqueous solution
|
Arrhenius
|
|
Oxy Acids
|
contain hydrogen, oxygen, and one other element. (H2SO4)
|
|
lewis model
|
a lewis acid is an electron-pair acceptor and a lewis base is an electron-pair donor
|
|
Oxidation Number
|
A positive or negative number assigned to an element to show its combining ability in a compound
|
|
The species that remains after a Bronsted acid has given up a proton is __.
|
conjugate base
|
|
Blue to red
|
acid turns litmus paper from ......
|
|
bronsted lowry
|
Suggested that acids are proton donors and bases are proton acceptors.
|
|
salt hydrolysis
|
process in which anions of the dissociated salt accept hydrogen ions from water, or the cations of the dissociated salt donate hydrogen ions to water
|
|
acid ionization constant
|
the value of the equilibrium constant expression for the ionization of a weak acid.
|
|
equivalence point
|
the point when there are equal molar amounts of acid and base
|
|
THE DISSOCIATION CONSTANT
|
measure the extent of dissociation , with the symbol K= c(A) x c(B) /c(AB)
|
|
bronsted-lowry acid-base reaction
|
the transfer of protons from one reactant (the acid) to another (the base)
|
|
The __ of a solution is the negative logarithm of the hydrogen-ion concentration
|
pH
|
|
strong base + strong acid
|
neutralization will have pH 7
|
|
Acid-base indicator
|
A chemical dye whose color is affected by acidic and basic solutions
|
|
When an acid and base mix it forms ____
|
Salt
|
|
BL conjugate base
|
particle formed when an acid donates a H+
|
|
Can accept a pair of electrons to form a covalent bond. (broad, any substance that can)
|
Lewis acid
|
|
Bases & Alkalis
|
- Bases are oxides or hydroxides of metal.- Soluble bases are called alkalis.- All alkalis are bases, but not all bases are alkalis.
|
|
between m-1 and m
|
n X 10^-m, what will the estimation of the log function be (for calculating pH, pkb, etc)
|
|
What is a polyprotic acid, base?
|
A polyprotic acid is a compound that can donate more than one proton. A polyprotic base is a compound that accept more than one proton.
|
|
How does Litmus react to acids and bases?
|
Acid turns blue Litmus paper red and a base turns red litmus paper blue.
|
|
hydrochloric
|
HCl
|
|
HF
|
Weak
|
|
H3PO4
|
Phosphoric Acid
|
|
Neither
|
a salt
|
|
HC2H3O2
|
acetic acid
|
|
Kw (expression)
|
[H3O+][OH-]
|
|
CCl3COOH
|
Weak Acid
|
|
HClO
|
weak acid
|
|
What neutralizes H⁺s?
|
OH⁻s
|
|
Base dissociation constant
|
Kb
|
|
Hyrdrobromic Acid symbol?
|
HBr
|
|
log(xy) =
|
logx + logy
|
|
solution of known concentration
|
titrant
|
|
monoprotic acids
|
1 acidic proton
|
|
what is acidotic pCO2?
|
44
|
|
Henderson Hasselbach
|
used to calculate pH
|
|
oxyacids
|
___________ have acid hydrogens attached to an oxygen atom, ie Sulfuric acid and nitric acid
|
|
standard solution
|
the solution of known concentration
|
|
Example of a: Strong Acid
|
car battery
|
|
Draw the reabsorption of bicarbonate ion
|
|
|
Ca, Sr, Ba
|
Three strong base exceptions.
|
|
stronger
|
The larger Ka the ____ the acid.
|
|
binary acids
|
acids that are name "hydro_____ic acid"
|
|
organic
|
over 90% of compounds are what type
|
|
common bases
|
NaOH = sodium hydroxide
KOH = potassium hydroxide
Ca(OH)2 = calcium hydroxide
Al(OH)3 = aluminum hydroxide
NH3 = ammonia
CaO = calcium oxide
|
|
The reaction in which water molecules produce ions is called
|
self-ionization
|
|
common strong acids
|
sulfuric acid - H₂SO₄(aq), hydrochloric acid - HCl(aq), nitric acid - HNO₃(aq), perchloric acid HClO₄(aq)
|
|
Arrhenius solution
|
hydrogen chloride gas dissolves in water. HCl molecules ionize to form H+ ions which make the solution acidic.
|
|
2
|
if the concentration of a solution of HCl is 10^-2, the pH is _______
|
|
conjugate acid-base
|
two substances related to each other by the donating and excepting of a single proton
|
|
Red to blue
|
Base turns litmus paper from .......
|
|
bronsted base
|
any substance capable of accepting a proton from another substance
|
|
chloride shift
|
ionic conc increaseallows Hgb to give up O2(water moves in)
|
|
neutral solution
|
any aqueous solution in which [H] and [OH] are equal
|
|
acid rain
|
S oxide and N oxide gases cause this
|
|
A substance can act as both an acid and a base is said to be ___________
|
amphoteric
|
|
Acid base indicators
|
a substance that changes in color depending on the pH of the solution that the substance is in
|
|
arrhenius model
|
A model of acids and bases; states that an acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solution and a base in a substance that contains a hydroxide group and dissociates to produce a hydroxide ion in aqueous solution.
|
|
How is molecular struture and acid strength related?
|
Acid Type Trend---------------------------Binary 1. More polar H-A bond, the stronger the acid.(observed for acids of the same period) 2. The weaker the H-A bond, the stronger the acid (observed for acids in the same grop)Oxoacid 1. The greater number of O atoms attached to the central atom (greater oxidation state), the stronger the acid. 2. For same number of O attached to thes ame central atom, the greater electronegativity of the central atom, the stronger the acid. Carboxylic: The greater the electronegativites of the groups attached to the carboxyl group, the stronger the acid.
|
|
What is salt?
|
Salt is an ionic compound made from the neutralization of an acid with a base.
|
|
Buffered solution
|
a solution that resists a change in pH when either an acid or a base are added
|
|
What is Hypertonic dehydration?
|
Fluid has more solutes than plasma, Dm, DKA, hyperglycemia and DI
|
|
How can hydranea flowers indicate acids and bases?
|
because hydrangea flowers change color depending on the pH level.
|
|
Titration curve (pH curve)
|
a plot of pH of solution versus volume of titrant added to a given solution
|
|
CO2 is constantly being formed by what?
|
metabolism so the resp system is contantly balancing the amount of CO2 in the ECF
|
|
If you are ever given grams in this unit, what do you do?
|
Find the M using mols/grams from the periodic table.
|
|
cation
|
positively charged ion
|
|
hydroxide ion
|
diatomic (2 atom) anion with chemical formula OH−. It consists of an oxygen and a hydrogen atom held together by a covalent bond, and carrying a negative electrical charge
|
|
Litmus
|
Is an example of an indicator, which is a compound that changes color when in contact with an acid or a base.
|
|
Corrosive (Corrode)
|
to destroy or damage in a certain way; most acids are very corrosive of metals.
|
|
chlorate
|
CLO3-1
|
|
pH above 7
|
base
|
|
Examples of Acids
|
vinegar, lemon juice
|
|
acids are sometimes called...
|
proton donors
|
|
Chemical Formula of Potassium Hydroxide
|
KOH
|
|
What is the PH of saliva
|
7
|
|
What do strong bases contain?
|
lost of OH-ions
|
|
Polar covalent solutes that Ionize in H2O
|
Acid
|
|
what color does litmus paper turn with a base?
|
blue
|
|
What color do acids turn litmus paper?
|
turns red
|
|
What do acids do in water?
|
makes h+ ions
|
|
What does an acid turn with a metal?
|
H(2) gas
|
|
What is pH?
|
pH is something that measures how acidic or basic a substance is. It is measured on a pH scale.
|
|
What is an indicator?
|
something that changes color in the presence of an acid or base
|
|
Give an example of a dilute solution
|
weak tea, weak lemonade
|
|
what are the characteristics of an acid?
|
corrosive, sour, react with metals
|
|
Why would a solute settle to the bottom of a beaker even if you stir it?
|
if it was saturated
|
|
What are some various indicators we learned about in class?
|
red litmus paper- turns blue in basesblue litmus paper- turns red in acidsph paper- turns different colors in acids and bases
|
|
vinegar
|
acids
|
|
Propane
|
C(3)H(8)
|
|
taste sour
|
acid
|
|
NH3
|
WB Amonia
|
|
Bases feel...
|
slippery
|
|
litmus blue
|
base
|
|
Bronsted Bases
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Accepts Protons
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Lewis Bas
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Donates electron pairs
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HClO4 (Perchloric Acid)
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Strong Acid
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Basic
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a pH HIGHER than 7
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"salt"
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a compound formed by replacing hydrogen in an acid by a metal (or a radical that acts like a metal)
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conjugate acid pairs differ by
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and H+
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traditional base
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contains hydroxide ions and dissociates in an aqueous solution
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digestion
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breaks down the complex molecules of foods into smaller molecules
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properties of bases
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electrolytes, bitter taste, turn litmus blue, slippery feel
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Metabolic Acidosis
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pH ↓ = [HCO3] ↓/ [CO2]
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amphiprotic
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any substance that can accept and donate protons
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false
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bases turn blue litmus paper red tf
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Which of the following is the conjugate base of HCl?
Cl4 or H-1
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H-1
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true
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true of false? weak bases only partially accept protons
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What is Sulfuric Acid effective as
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A dehydration agent
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HIGH pH (number)
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has a LOW concentration of H+
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hydronium ion
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H3O+, same thing as proton H+(aq), hydrated
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cohesion
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the force that holds molecules of a single material together
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Polyprotic Substances
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• polyprotic acid will react to give off 2 hydrogen ions but at different pH's
• polyprotic base can accept more than one hydrogen ion
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What is compensation in the renal system of acid-base balance?
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(slow, powerful compensation)
-compensates for respirator causes of acidosis or alkalosis
-effective for imbalances of a few days or longer
-acidosis causes increase in H+ secretion
-alkalosis causes bicarbonate secretion
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hydronium
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formed when an acid is added to water (H3O+)
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buffer solution
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a solution with resists change in pH/ changes pH very slightly/ keeps pH constant when SMALL amounts of acid or base are added
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the ability of an acid to ionize 100% in water and produce 100% hydronium ions (H₃O⁺) with virtually no molecular form of the acid left in the acid water (aqueous) solution
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strong (acid)
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hydrogen ion
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an atom of hydrogen that has lost its electron
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Arrhenius definition of an acid
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is a substance that produces H+(H30+) in water
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first step in concentration problems
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M = mol / L; to cancel out
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What happens when Blue Litmus and Red Litmus paper are dipped upon by Neutral Solution?
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Both litmus will stay the same colour
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HCIO4
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strong
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Ammonium
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NH3
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H2S
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Weak Acid
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Nitric acid
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HNO3
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Ba(OH)₂
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Barium hydroxide
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Are bases electrolytes
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Yes
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Calcium Hydroxide
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Ca(OH)2 (strong)
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Arrhenius bases
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form hydroxide ions
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Ate
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Ic. Drop the hyrdogen.
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blue
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acids turn........... litmus paper red
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IUPAC
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names acids as aqueous ionic compounds
HCl (aq) - aqueous hydrogen chloride
H₂SO₄ (aq) - aqueous hydrogen sulfate
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Is windex and bleach a base?
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yes
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pH of 0 to less than 7
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acid
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What is a buffer?
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Resist changes in pH
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What is the formula for Calcium Hydroxide?
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Ca(OH)2
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ion
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charged particle that has either more or fewer electrons than protons
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formula ends with OH or is a negatively charged ion
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base
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acids and a base
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Neutralization is a reaction between?
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transition interval
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pH range over which indicator changes color, p. 749
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molecules
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Two or more atoms held together by covalent bonds.
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diprotic acid
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an acid that can donate two protons per molecule.
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7 strong acids are:
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H2SO4 (Sulfuric Acid), HNO3 (Nitric Acid), HCL (Hydrochloric Acid), HBR (Hydrobromic acid), HI (Hydroiodic acid), HCLO3 (Chloric acid), HCLO4 (percholoric acid)
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universal indicator
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turns the acid or base a colour to show the pH level on the scale.
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Arrhenius model (acid def)
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any substance that produces H+ ions (protons) in AQ SOLUTION
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Why Will Sulphuric acid give more Hydrogen than Hydrochloric acid or Nitric acid?
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As there are more hydrogen atoms within the sulphuric acid than the other acids. Therefore it will not need as many acid molecules to make up the same amount as Sulphuric acid.
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how do you find H+ when you are given OH-
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1.0 x 10^-14 divided by OH-
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