| Terms |
Definitions |
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Ephedrine
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WB
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base
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NaOH
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?
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...
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H2SO4
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Sulfuric Acid
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hydrofloric
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disovles glass
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H2CO3
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CARBONIC ACID
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OH-
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hydroxide ions
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LiOH
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lithium hydroxide
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weak acid
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HC2H3O2
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Nitric Acid
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HNO3
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H3PO4
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Phosphoric Acid W
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Acid
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Hydrogen ion donar
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Acids pH range
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1-6
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Acids taste _________.
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sour
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6 Strong Bases
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CH3O-
OH-
CO3-
NH3
HCO3
CH3COO-
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salt
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KBr is a _______
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PH SCALE 7< ??
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BASE
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neutral
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neither acidic nor basic
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Plants store carbohydrates as
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starch
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Which of the amphoteric
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H2O
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Do acids react with carbonates?
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yes
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conjugate base
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acid minus a proton
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iodine
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starch (dark purple or black)
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Amino Acids
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building blocks of protein
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what is strength?
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the degree of ionization
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HSO3-
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name the conjugate base of H2SO3
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Ionization
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Ionization occurs when a molecular compound (made up of covalent bonds) produces ions when in water.
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Arrhenius acid
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dissociate to form hydrogen ions
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As H increases pH does what?
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Decreases
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Arrhenius base
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produces OH- ions in a solution
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diprotic acids
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acids that have two ionizable hydrogens like sulfuric acid H2SO4.
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Acidosis
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Abnormally high acidity (low pH) of the blood and body tissues. Can be brought about by . . .
Severe lack of oxygen, excess carbon dioxide (hypoventilation).
diabetes - accumulation of acidic ketone bodies.
Kidney disease - over-excretion of bicarbonate.
Severe diarrhea - loss of bicarbonate.
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HSO4-
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amphoteric- can donate and accept a proton.
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Indicator
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changes color in an acid or base
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Disinfectant
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Is a substance that kills harmfull bacteria and viruses.
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Strong Bases
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NaOH, KOH, LiOH, Ba(OH)2, Sr(OH)2, (CH3)4NOH
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amphoteric
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hydroxides of metals like Zn, Al, and Cr capable of reacting as either an acid or base
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Strong acids
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___ are acids that completely ionized in water.
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Base dissociation constant (Kb)
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? = [B+][OH-] / [BOH]
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pH
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-log[H+]. ((The scale) goes from 1 to 14).
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Carboxylic Acids
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Acids that contain a carboxyl group whose relative strengths depend on polarity, meaning that CH3COOH is weaker than CH3COOCl because Cl is more electronegative and thus the molecular structure is more polar.
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Concentration
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the amount of particles dissolved in a particular amount of solution
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According to Arrhenius, an acid is an H⁺________
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producer
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titration
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a measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
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neutral solution
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an aqueous solution in which the concentrations of hydrogen and hyroxide ions are equal
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Basic Anhydrides
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Compounds that when added to H2O form bases. Metallic oxides.
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Soap
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A substance that is used as a cleaner and that dissolves in water.
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pH scale
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used for measuring strength of acid or base
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conjugate acid-base pair
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consists of two substances related by the loss or gain of a single hydrogen ion
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Example of a saturated solubility
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sponge (with too much water)
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Lewis Acid-Base Reaction
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the formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
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GENERAL PROPERTIES OF ACIDS
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they dissociate into ions in water, their aqueous solutions conduct electricity, they have sour taste, change the color of litmus paper into red, they react with active metals and produce hydrogen gas, they react with bases
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Reactions in which an acid and a base react in an aqueous solution to produce a salt and water are called
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neutralization reactions
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they increase the concentration of hydroxide ions in aqueous solution
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Which statement about Arrhenius acids is false?
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neutralization reaction
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the reaction of an acid and a base to form a neutral solution of water and a salt
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The weaker the H-X bond and the more polar the bond...
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the stronger the acid.
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What type of salt produces a basic solution? One that contains ________ ____ _____ _______ ____________ _____ __________
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negative ions that attract protons from water
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molarity of acid x volume of acid = molarity of base x volume of base; tiltration
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Whats does "MaVa=MbVb" mean? What is it used for?
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8
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Octa
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Lactic Acid
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Milk
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strong base
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pH14
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HCL
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HYDROCHLORIC ACID
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pH 3
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cola
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Sulfuric Acid
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H2SO4
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HNO3
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Strong Acid
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Hydrogen
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Most acids contain
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phenolphtalein orginal color
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clear
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A weak acid
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HF
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Solution is Acidic
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pH<7
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PH = ?
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H₃0 LOG-
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Bronsted Lowry base
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proton acceptor
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Animals store carbohydrates as
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glycogen
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reacts with certain metals
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acid
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Kb
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Equilibrium constant for weak bases
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increase in oxygen atoms
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increases acidity
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From [H+] to pH
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-log [H+]
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Organic Acids
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"carboxyl group" all organic
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Acids
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electrolytes, sour taste, turn litmus red, react with metals to form H2 gas
ex: vinegar, milk, soda, apples, citrus fruits
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inorganic acids include:
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hydrochloric, sulfuric, and nitric
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strength
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Quantitative tests measures the ____ of an acid or a base on a pH scale.
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Arrhenius Bases
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substances that increase the concentration of hydroxide ions in aqueous solutions
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solvent
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a liquid substance capable of dissolving other substances
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Phosphorus has an inverse relationship with?
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Calcium
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equivalence point
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The stoichometric point in a titration.
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Strong acid
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ionizes completely in an aqueous solution
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properties of bases
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taste bitter
cause indicators to change color
react with acids to produce neutral solutions
dissociate in water
feel slippery (like soap)
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triprotic acids
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acids that have three ionizable hydrogens like phosphoric acid H3PO4
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bases
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What is a substance that is characterized by bitter taste, slippery feel, and a pH of 8 or higher?
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Hair/Shampoo
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Hair consists of strands of protein called kertain and shampoo does not take out all of the grease and oils because you still need some natural oils and greases in your hair.
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Solution
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mixture in which one substance is evenly mixed with another substance
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Lewis acid
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an electron pair acceptor; any species that will bond to an unshared pair of electrons
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Weak acids
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___ are acids that partly dissociate in water having a mixture of acid molecules and component ions.
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Acid dissociation constant (Ka)
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? = [H3O+][A-] / [HA]
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metals
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what substance can acids react with to produce hydrogen gas?
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get stronger as go down group
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Halogen acid trend
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Brønsted-Lowry Theory
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1923, Acid: proton donor, Base: proton acceptor
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Name the buffer system involving dihy--
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dihydrogen phosphate ion-hydrogenphosphate ion,
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dehydrating agent
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a substance that remove water from materials
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monoprotic acid
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any acid that contains one ionizable proton
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Hydronium ion
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an ion consisting of a proton combined with a molecule of water; H3O+
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Stay Together
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Strong acids break apart in water and weaks acids ____ in water (stay together/ break appart)
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base ionization constant
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the value of the equilibrium constant expression for the ionization of a base
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Bronsted-Lowy Acid
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a molecule or ion that is a proton donor
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Le Chatelier's principle
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a change in any of the factors determining equlibrium will cause the system to adjust to reduce the effect of the change
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The product of the concentrations of the hydrogen ions and hydroxide ions in water is called the (long name)
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ion-product constant for water
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A diluted substance
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Only has a little bit of a solute
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bases and some metals
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acids turn blue litmus paper red with _____ to form salts
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Acid strength is related to...
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bond strength (since a proton must be lost).
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The purpose of titration is what?
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To find the strength of an unknown solution
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How are teh substances in a conjugate acid-base pair related to each other?
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by the donating and accepting of a single proton
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