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A hydrogen-containing substance that is capable of donating a hydrogen ion to another substance.

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=a pH less than 7
=usually sour
=has high concentration of H+ in solution
=Amphoteric compounds react with acids to form a metal salt
=rough texture
=turns litmus paper blue to red
=reacts with metals(H2) and carbonated compounds(CO2)

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A molecule that takes up or accepts protons. A compound that reacts with an acid to form a salt.

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=a ph of greater than 7
=tastes bitter
=soapy and slippery texture
=turns litmus paper red to blue
=does not typically react with metals or carbonated compounds
=reacts with oils and fats
=has high concentration of hydroxide (OH-) ions
=Amphoteric compounds react with a base to form a polyatomic metallic ion

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a salt is produced when a strong acid and strong base react.

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the disconnection or separation of something from something else or the state of being disconnected.

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Why there are Strong & Weak acids and bases due to dissociation..

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Why there are Strong & Weak acids and bases due to dissociation..

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Strong acids are molecules that end up completely dissociating their ions into water, and weak acids are molecules that partially dissociate into water.

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a compound, which ionizes to yield hydrogen ions (H+) in aqueous solution.

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An Arrhenius base is a compound, which ionizes to yield hydroxide ions (OH−) in aqueous solution.

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Phosphoric acid (H₃PO₄)

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Magnesium hydroxide Mg(OH)₂

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is a molecule or ion that donates a hydrogen ion in a reaction.

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is a molecule or ion that accepts a hydrogen ion in a reaction.

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Hydrochloric acid (HCl) reacting with base ammonia (NH3).

HCl is a Brønsted-Lowry acid.

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Hydrochloric acid (HCl) reacting with base ammonia (NH3).

(NH3) It is a Brønsted-Lowry base.

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is a substance that accepts a pair of electrons to form a covalent bond.

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is a substance that donates a pair of electrons to form a covalent bond.

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H+, K+, Mg2+, Fe3+, BF3, CO2, SO3, RMgX, AlCl3, and Br2.

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OH-, F-, H2O, ROH, NH3, SO42-, H-, CO, PR3, and C6H6

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pH stands for stand for Power of Hydrogen, which makes 'p' mean the power of the hydrogen ion.

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a solution is the negative logarithm of the hydrogen-ion concentration.

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5.80 pH

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3.50 pH

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13.00 pH

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10.00 pH

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pH = −log [H+]

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pH = -log[H3O+]
pH = -log(1.2 x 10^-3)
pH = -(-2.9)
pH = 2.9

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pH = -log[H3O+]
pH = -log(4.7 x 10^-9)
pH = -(-8.3)
pH = 8.3

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The negative logarithm of the hydroxide-ion concentration.

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pH is a measure of hydrogen ions, while pOH is a measure of hydroxide ions.

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a solution that can resist pH change upon the addition of an acid or a base.

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How does a buffer stabilize the pH of a solution if an acid is added to the solution

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How does a buffer stabilize the pH of a solution if an acid is added to the solution

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the buffer gets rid of the hydrogen ions fast enough for the pH to remain stable.

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How does a buffer stabilize the pH of a solution if a base is added to the solution

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How does a buffer stabilize the pH of a solution if a base is added to the solution

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the hydroxide ions interact with hydrogen ions to remove the basic presence, causing no dramatic pH change.

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it is a tool that someone uses in order to determine the pH of something, if it's higher than 7 its basic, and if it's lower than 7 it's acidic.

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pOH = -log[OH-]

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pH = 14 - pOH

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An acid-base indicator is either a weak acid or weak base that exhibits a color change as the concentration of hydrogen (H+) or hydroxide (OH-) ions changes in an solution.

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4 pOH

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10.5 pOH

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1 pOH

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pOH = -log[OH-]
pOH = -log(1.0 x 10^-7)
pOH = 7.0

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pOH = -log[OH-]
pOH = -log(3.2 x 10^-11)
pOH = 10.5

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pH is inversely proportional to pOH.

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pH is a measure of hydrogen ions, while pOH is a measure of hydroxide ions.