Chemistry Test (March 2023)
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Last updated 4:46 PM on 3/30/23
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32 Terms
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Arrhenius acid
produces H+ ions; works with water and can be used with electricity because of + ions
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What does “ksp” stand for?
solubility product constant
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ksp is used for
slightly soluble salts at equilibrium
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x stands for
solubility and any ion with a 1 coefficient
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math definition of ksp
the concentration of ions raised to and multiplied by ion coefficients
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arrhenius base
produces OH- ions
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bronstead-lowery base
proton acceptor
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bronstead-lowery acid
proton donor; weak acid-base equilibrium
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conjegate base
base that loses H+ ions
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conjegate acid
base that gains H+ ions
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lewis acid
an electron acceptor; new covalent bonds
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Lewis base
on electron donor
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titration
neutralization proceedure to determine the unknown concentration
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acidic solution
a solid where H+ ions are produced in water (can be ionic or covalent)
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list 5 characteristics of an acid
* produces H+ ions in water
* tastes sour
* corrode acids (corrosive)
* acids neutralize bases
* pH is less than 7
* tastes sour
* corrode acids (corrosive)
* acids neutralize bases
* pH is less than 7
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list 3 common acids
* Hydrochloric acid
* Sulfuric acid
* Nitric acid
* Sulfuric acid
* Nitric acid
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basic solution
produce hydroxide ions in water
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list 6 characteristics of a base
* produces OH- ions in water
* tastes bitter or chalky
* feels soppy or slippery
* neutralize acids
* turns red litmus paper blue
* pH is greater than 7
* tastes bitter or chalky
* feels soppy or slippery
* neutralize acids
* turns red litmus paper blue
* pH is greater than 7
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list 3 common bases
NaOH -- sodium hydroxide
KOH -- potassium hydroxide
Ba(OH)2 -- barium hydroxide
KOH -- potassium hydroxide
Ba(OH)2 -- barium hydroxide
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amphoteric (Arrhenius)
can act as an acid or a base (ex. water + water)
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strong acid
ionizes completely in water
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weak acid
does not ionize completely in water
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strong base
ionizes completely in water
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weak base
equilibrium
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Brønsted-Lowery Acids
proton donor
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Brønsted-Lowery Base
proton acceptor
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equilibrium
steady rate (forming product + reforming reactants)
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negative logarithm
scale between 0-1
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indicator
when the end point changes (when color changes from an acid to a base)
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examples of indicators
universal indicator
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devices that measure pH
titration, pH stick, pH meter
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buffer
a substance that maintains a constant pH
