| Terms |
Definitions |
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4
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Tetra
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Polyester
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...
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-
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...
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H3PO4
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Phosphoric Acid
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sour
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acid taste
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HC6H7O7
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CITRIC ACID
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Barium Hydroxide
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Ba(OH)₂
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HBr
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hydrobromic acid
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Acid
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tastes sour
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Calcium Hydroxide
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Ca(OH)2
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H2S
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Weak Acid
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CH3NH2
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Weak Base
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+
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symbol for plus
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acceptor
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base is the
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weak acid
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H3PO4-phosphoric acid
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A strong base
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LiOH
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Bronsted-Lowry acid
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proton donor
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base
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food a bitter taste
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INCREASE CO₂
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REACTION SPEEDS UP
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BH3
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Weak Acid (lewis acid)
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Draw lung pH balance
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NH3 - ammonia
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weak base
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Nitric acid uses
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fertilizer, plastics, explosives
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dilute or concentrated
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Acids may be
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amphoteric
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behaves as acid or base
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Acids Litmus
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Blue Litmus turns Red
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Detergent
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A nonsoap water-souble cleaner that can emulsify dirt and oil.
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acid reflex disease is neutralized with a
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base
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strong acids
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completely ionized in aqueous solution
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Alkaline
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When a base completely dissociates, the solution is referred to as...
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Arrhenius base
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bases produce hydroxide ions OH⁻
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Name some Thiazide diuretics.
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HCTZ and HydroDiuril
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acidic solution
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contains more hydrogen ions than hydroxide ions.
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Acids
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taste sour, many are poisonous and destroy body tissue, electrolytes
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antacid
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a weak base that neutralizes stomach acid
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pH
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A measure of the concentration of solutions of acids and bases and is measured on a scale of 1-14. Bases are greater than 7, acids are less than 7,and 7 is nuetral
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neutralization
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the reaction of the ions that characterize acids (hydronium ions) and the ions that characterize bases (hydroxide ions) to form water molecules and a salt
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A neutral solution has a pOH of
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7
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lye
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a strong solution of sodium or potassium hydroxide
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pH Scale
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measures the concentration of Hydrogen ions in solution, ranges from 0-14
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common acids:
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lemon juice, apple juice, and shampoo. sometimes water.
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1A and 2A
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Strong bases are from group ____.
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higher
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the stronger the base (more OH- ions) the _____ the pH
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halogen containing compound
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a hydrocarbon that replaces one hydrogen with a fluorine is a
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Facts about acids
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latin word-acidus, sour taste when dissolved in water, causes the dye in litmus paper to change from blue to red, pH scale goes from 1-6
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Arrhenius Theory
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1887, Acids produce H+ in solution, Bases produce OH- in solution
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According to Arrhenius, a base is an OH- _____
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producer
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concentration
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the amount of a substance in a solution not whether it is strong or weak
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titration
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process in which a solution of known concentration is used to determine the concentration of another solution
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strong acids, H+
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____ ____ completely ionize in water and release more ___
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Acidic
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When the body has too much CO2, the blood becomes ____.
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hydronium ion
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formed when water gains a proton. it is 'the acid'
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acids react with bases to yield a salt and water
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true
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Lewis base
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an atom, ion, or molecule that donates an electron pair to form a covalent bond
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arrhenius model
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An acid is a substance that contains hydrogen and ionizes to produce hydrogen ions in aqueous solution; A base is a substance that contains a hydroxide group and dissociates to produce a hydroxide ion in aqueous solution
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Conjugate Base
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the particle that remains when an acid has donated a hydrogen ion
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conjugate acid-base pair
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two substances related by the loss or gain of a single hydrogen atom.
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a way of measuring the acidity of a solution that is based on a logarithmic scale
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pH scale
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which is faster, respiratory or renal compensation?
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respiratory (blows off CO2)
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All foods are made up of what?
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carbohydrates, water, protein, and fats
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neutralization reaction
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A reaction in which an acid and a base react in aqueous solution to produce a salt and water
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compounds linked in a chain
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a polymer is a compound made up of
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What is the equation for pH using H+ conc
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pH = -log[H+] = log(1/[H+])
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what is the equivalnce point of a titration?
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when the number of acid equivalents = number of base equivalents
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NH3
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Ammonia
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?
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...
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Hydrochloric Acid
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HCl
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CsOH
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Strong Base
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KOH
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Strong Base
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Nitric Acid
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HNO₃
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sour taste
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acid
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bromthymol blue
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acid-base-neutral
yellow-blue-green
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HCOO
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Weak Base
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RbOH
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Strong Base
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H_3PO_4
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phophoric acid (Weak)
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Lewis Acid
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Electron acceptor
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pOH equation
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pOH= -log[OH-]
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pOH
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- log [OH-]
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Phosphoric Acid (moderate)
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H3PO4
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H2CO3
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Carbonic acid (weak acid)
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STRONG ACID
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acid low pH(1-4)
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pink/red
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Cabbage juice - acid
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Pure Water
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pH = 7
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example of a solute
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salt
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PH SCALE = 7 ??
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NEUTRAL
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bases
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taste bitter, conducts electric current, changes litnus blue, feels slippery, doesnt react with active metals, doesnt react with carbonates
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Weak acid + strong base
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Basic pH
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Arrhenius Acid
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ionizes to produce H+ ions
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strong base
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metal OH that completely dissociates
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NV = NV
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titration or neutralization: normalities times the volumes..so the number of moles
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___ conjugate base stability will increase acidity
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increasing
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corrosive
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eating away by chemicals or disease; (of language) fierce
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Metallic oxides are ... when dissolved in water?
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Basic
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oxyacid
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compound of hydrogen, oxygen, and a third (usually nonmetallic) element
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equilibrium
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a chemical reaction and its reverse proceed at equal rates
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# of buffer systems crucial in maintaining human blood pH within a narrow range (pH 7.35-7.45)
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2
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ion-product of water
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equilibrium constant for the dissociation of pure water into H3O+ and OH-
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Strong Acid/Base
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100% ionized in water and strong electrolyte
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primary solution
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a highly purified solid compound used to check the concentration of the known solution
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CONJUGATED ACID
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THE SUBSTANCE THAT IS PRODUCED AFTER THE BASE ACCEPTS A PROTON FROM WATER
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strength
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how well the acid or base forms ions
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hydrogen
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metals react with acids to form the gas
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the stronger the acid the ...... the conjugate base
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weaker
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Sulfuric acid
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What acid is a very good dehydrating agent?
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transition interval
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the pH range over which an indicator changes color
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neutral solution
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any aqueous solution in whcih [H+] AND [OH-] are equal
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dissociation
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the breaking up of an acid or base into its constituent ions
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The [H+] of a basic solution is less than 1 x 10^?M
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-7
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acid-base indicator
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a dye that changes, loses, or acquires color as a solution containing the dye changes in acidity or basicity
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pH < 7.35HCO3 < 24 mmHgdecreased PCO2hyperkalemia
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metabolic acidemiaK/anion shift
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NOW,,,go prepare 500 mL (.500 L) of 6M solution NAOH!!!! straight away!!!!
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500x6x40= ans.
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7
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pH when an acid or base both strong or both weak react with each other
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stronger the acid
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The larger the X atom in H-X the
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What is the Bronsted Lowry Definition of an Acid? What is the Bronsted Lowry Definition of a Base?
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bronsted acid=proton donor,bronsted base=proton acceptor
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water and a salt
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when an acid and a base neutralize each other, this remains
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acidic substances
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0-6 on the pH scale, 1 is more of this/stronger one of these than 6
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any substance that can donate a proton (Hydrogen nucleus); any substance that can accept a proton
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Bronsted-Lowry's Definition of an Acid? ...Base?
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How do you measure the concentration
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compare the amount of solute to the amount of solvent
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Why use unsuling and glucose admint with hyper mag?
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Mag follows K into the cells which is drawn there by the insulin/gluc.
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Pyridine
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C5H5N
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Ammonia
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NH₃
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hydrochloric
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HCl
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NaOH
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sodium hydroxide
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NH₃
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Ammonia (wb)
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Calcium oxide
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CaO
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Potassium Hydroxide
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KOH
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Hydrofluoric Acid
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HF
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magnesium hydroxide
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Mg(OH)₂
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phosphorous acid
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H₃PO₃
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Sodium Carbonate
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Na₂CO3
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H₃C₆H₅O₇
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Citric Acid (wa)
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Ammonia in water
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NH₄OH
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HI (aq)
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Hydroiodic Acid (sa)
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CH3COOH
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Acetic Acid
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Ionization
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formation of ions
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Neutral
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neither acidic nor basic
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standard solution
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solution of known concentration
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Insoluble
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not able to be dissolved
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Traits of Bases
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bitter taste, corrosive, electrolyte(b/c of negative ions), above 7 on pH scale, turns red litmus paper blue, slippery
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Substances that donate hydrogen ions to form hydronium ions when dissolved in water
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acids
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What do acids and bases taste like?`
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Acid-sourBase-bitter
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Large amount of polar covalent solute in solution
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concentrated acids
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Examples of Chemical Change
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burning, corroding (putting acid on something), rusting, bubbling
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conjugate acid
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the particle formed when a base gains a hydrogen ion
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pH is measured with.... (2 things)
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pH meter, Hydrion Paper
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how does acid rain happen?
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the rainwater reacts with air pollution and acids are formed so the ph decreases
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Example for Solute/Solvent
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with salt and water, salt would be the solute and the solvent would be the water
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What causes acidity?
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The more hydrogen ions there are in a solution, the more acidic it is. In other words the more hydrogen ions there are, the lower the pH number is.
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What happens when an acid reacts with a metal?
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the metal dissolvesmakes hydrogen gas
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Why would a cook add salt to water to cook spaghetti
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the water boils at a higher temperature and will cook faster
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LiOH
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strong
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R3N
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WB
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Ca(OH)2
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Strong Base
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bitter taste
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base
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HClO₃
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Chloric acid
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NH4+
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Weak Acid
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Cabbage juice
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Indicates pH
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HNO3
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Nitric acid strong
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Carbonic Acid
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H2CO3 (weak)
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kw
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Ion product of water;
kw=[H+][OH-];
kw=1.00x10-14 at 25 C
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Alkali
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A base mixed with water
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OH
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What Bases produce in water
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phenolphthalein
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an indicator commonly used in titrations that is colorless in acid and pink in base
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solution
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a homegeneous mixture throughout which two or more substances are uniformly dispersed.
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Lewis
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What has bases as electron pair donor?
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indicator
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tells whether something is acid, base, neutral or starch
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What is Metabolic Alkalosis?
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(rare)
-overuse of bicarbonates (antacids)
-loss of acid (chronic vomiting)
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What is produced after every neutralisation?
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Metal salt
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A Bronsted-Lowry base is a...
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hydrogen proton acceptor
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Strong
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Which is more conductive? Weak or strong acids?
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triprotic
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acids which have 3 hydrogen to donate in an aqueous solution
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Bronsted-Lowry base
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proton acceptor, e.g. NH3 (+HOH), not NaOH
|
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negative ion
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An atom with more electrons than protons
|
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binary acid
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an acid composed of only two elements, one of which is hydrogen
|
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acid-base pair that is related through the loss or gain of one proton (H⁺)
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conjugate acid-base pairs
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positive ion
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an ion that has fewer electrons than protons
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acid-base reaction
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acid plus base, e.g. HF (WA) + HOH (WB) -- H3O+ (SCA) + F- (SCB)
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What is Hypocapnia?
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a state in which the level of carbon dioxide in the blood is lower than normal; can result from deep or rapid breathing
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What is the test for Hydrogen?
|
Squeaky Pop Test: Lit splint into test tube filled with H2 Gas. Squeaky pop should be heard.
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When a solution is called amphoteric, this means that
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it can be an acid or a base
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