HCl → H + + Cl - NaOH → Na + + OH -
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Transcript of HCl → H + + Cl - NaOH → Na + + OH -
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What makes an acid an acid or a base a base can vary depending on definition being used. The first definition was created by Svante Arrhenius in 1883. Arrhenius said compounds that will ionize to give off H+ ions are acids and compounds that will ionize to give off OH- ions are bases.
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HCl → H+ + Cl-
NaOH → Na+ + OH-
ACID
BASE
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The Bronsted-Lowry definition for a base is that it is an H+ acceptor. The definition of an acid is still the same as for Arrhenius - an acid gives off H+
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HCl + NH3 → NH4+ + Cl-
ACID BASE
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NH4+ + Cl- → HCl + NH3
ACID BASE
The equation backwards shows chlorine accepting hyrdrogen., making it a base. In the other equation HCL gave off hydrogen, making it an acid. Therefore we call the pair a conjugate acid-base pair.
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HCl + H2O → H3O+ + Cl-
NH3 + H2O → NH4+ + OH-
Substances that can act as both an acid and base are called amphoteric.
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H3PO4 + H2O → H2PO4- + H3O+
H2PO4- + H2O → HPO4
-2 + H3O+
HPO4-2 + H2O → PO4
-3 + H3O+
Acids that can give off more than one H+ (protons) are called polyprotic. H3PO4 is a triprotic acid, and H2SO4 would be a diprotic acid.
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A concentrated acid has a lot of acid dissolved in water, and a dilute acid has only a little
Strong acids ionize completely, and weak ones only ionize a little.
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0 1 2 3 4 5 6 7 8 9 10 11 12 13 14
Strong Acid WeakAcid
WeakBase
Strong Base
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To determine the pH of a substance requires an indicator. Indicators are substances that turn colors at certain pH’s.
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When an acid and base are added together in appropriate amounts, the resulting pH is near 7 - neutral. This is why acids and bases are said to “neutralize” each other. In a neutralization reaction the acid and base (according to the Arrhenius definition) react to form water and a salt.
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HCl + NaOH → HOH + NaClWater Salt
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Neutralizing an acid and base to determine an unknown amount of H+ or OH- is called titration. In a titration a small amount of indicator is added that will change color when the neutralization is complete.
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