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https://play.kahoot.it/#/k/ba1d7145-92b8-484c-b7b6-4f2a5e435946

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Covalent Oxides form acids in water (examples include CO2, SO3)

Ionic Oxides form bases in water (examples include CaO and NaO2

Polyprotic acids have multiple protons to give up. Each ionization happens in a separate step, with each successive ionization occurring to a lesser degree

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When referring to an acid or base as strong or weak, we are talking about whether or not the substance fully disassociates within a solution. Strong substance have a k value that is greater than 1 and will fully disassociate. Meanwhile, weak substance have a k value less than 1 and will not fully dissociate.

A strong acid will have a weak conjugate base, and a strong base will have a weak conjugate acid. These conjugates are weaker than water and unable to hydrolyze.

A weak acid will have a weak conjugate base, and a weak base will have a weak conjugate acid. HOWEVER, these conjugates are stronger than water, and can effectively hydrolyze with water.

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Formulas for ka,kb,pka, pkb, and how to calculate pH from pka

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Formulas for ka,kb,pka, pkb, and how to calculate pH from pka

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pka = -log(ka)
pkb = -log(kb)
ka = ([H+] [A-]) / [HA]
kb = ([OH-] [HB]) /[ B]
pH = pka + log([A-]/[HA])

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Kw = [H3O+][OH-]
Kw = 1.0•10^-14
pH + pOH = 14

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Salts are formed through the neutralization of acids and bases. However, it is important to realize that the salt formed is not always neutral. A salt is made up of a cation and an anion, which come from the base and the acid respectively.

If both the cation and the anion are unable to hydrolyze with water, the salt is neutral.
If the cation is stronger than water, the salt will be slightly acidic.
If the anion is stronger than water, the salt will be slightly basic.
If both the cation and anion are stronger than water, the stronger ion 'wins' and pH shifts in that direction.

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pH does not determine the strength of an acid

Substances containing H aren't always acidic (NH3 is basic)

Equilibrium constants are only constant at constant temperatures

Water is not always neutral at a pH of 7

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Acids are electron pair acceptors (have open orbital)

Bases are electron pair donors (have lone pairs)

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Can act as an acid or a base, depending on the

circumstance

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Base-ionization Constant

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Acid-ionization Constant

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Two water molecules act as an acid and base at the same time to self ionize

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Product made when a base accepts a proton

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Product that remains after an acid donates a proton

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Acids produce H+ ions in water

HCl + H2O➡️H3O+ + Cl-

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JUST THE BASICS: What you need to know about acids and bases

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JUST THE BASICS: What you need to know about acids and bases

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Acid/Base reactions are focused on the exchange of protons among species in solution. An acid donates a proton and forms H3O+ in water, while a base accepts a proton to form OH- in water. Some substances can do either, and these species are referred to as Amphiprotic.

H3O+ and OH- are always proportional to each other, based on the ionization constant of water.

An acidic pH is one that is less than 7, while a basic pH is greater than 7.

pH is a measure of the hydronium concentration in a solution, and pOH is a measure of hydroxide concentration in a solution. Because they are proportional, pH and pOH can be converted to each other.

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Formulas for calculating hydronium to pH, hydroxide to pOH, and vice versa 

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Formulas for calculating hydronium to pH, hydroxide to pOH, and vice versa 

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pH = -log[H3O+]
[H3O+] = 10^-pH
pOH = -log[OH-]
[OH-] = 10^-pOH