Acids & Bases

Amphoteric= Can act as base and acid (H20)m

Triprotic= donate 3 protons H3PO4

Diprotic= donate 2 protons

monoprotic= donate 1 proton

acid and base react to form water and salt = neutralization

acid + base = water + salt

Salt : any class of a chemical compound formed by the neutralization of an acid by a base

Acid + metal carbonate = water + salt + CO2

Acid + metal hydrogen carbonate = water + salt + CO2

Hydrogen carbonate (HCO3) is also know as bicarbonate

pH scale

the molar concentration of H+ in an aqueous solution

pH + pOH = 14 '

pH = -log [H+] or [H+] = 10-pH

< 7 = acidic

> 7 = basic

7 = neutral

can be less than 0 and over 14

brackets means molarity [ ]

change in 1 pH unit represent a change in concentration of solution by 10

Logs

moles H+ per L of solution

-log [1.0×10^-7] = -(-7.00) = 7.00

Autoionization of water

in presence of acid water acts as a proton acceptor, in the presence of a base water acts as proton donor

one water molecule can donate a proton to another water molecule

water decomposes into acid and base, electrons steal proton

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Strong acid completely transfers its protons to water, leaving no undissociated molecules in sloution

its conjugate base has a neglible tendency to be protonated (to abstract protons) in aqueous solution

weak acid partially dissociates in aqueous solution and therefore exists in the solution as a mixture of acid molecules and their constituent ions

neglible acidity contains H but doesn’t demonstrate any a

ka= dissociation constant for acids

kb= dissociation constant for bases

value of kb and ka gives us info about the strenght of an acid/base

large ka means products are favored, small ka means reactants are favored

large kb means products are favored, small kb means reactants are favored

Equation for both = products/ reactants

you can get the reverse reaction if you take k and flip it

liquids & solids are not used in equilibrium expressions, only use gases and aqueous species

homogenous= substances involved are in same phase

heterogenous= substances in diff phases, whenever a (s) or (l) is involved then the concentration is not in included in equilibrium constant expression

2H₂(g) + 0₂(g) = 2H

weak acids = less ions