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Acids and bases

Melissa McFarland

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3.For oxyacids, the more electron withdrawing (more electropositive) the non- metal center, the stronger the acid due to a weakening of the O-H bond. This trend is approximated by the equation: PK a = 8 - 9f + 4n , where f is the formal charge on A when all oxygens are singly bound to A, and n represents the number of O atoms bound to A that are not bound to an H.
4.A measure of the strength of a base, it is equal to – log K b, where K b is the base dissociation constant in water
5.A molecule that can be described as an acid that has lost one proton.
6.Having a pH greater than 7 or a pOH less than 7.
8.Arrhenius proposed that acids are substances that produce protons (H+) in aqueous solution, whereas bases produce hydroxide ions (OH-) in aqueous solution. Compare his model with the Bronsted-Lowry definition and the Lewis definition.
12.Separate into its ion constituents.
14.A base with a pK b greater than zero. Weak bases do not completely dissociate in water.
16.A base with a pK b less than zero. Strong bases completely dissociate in water.
17.A molecule that can be described as a base that has gained one proton
18.Lewis defined an acid as an electron pair acceptor and a base as an electron pair donor. Compare his model with the Arrhenius model and the Bronsted-Lowry definition.
19.A species that can either donate or accept a proton, e. g. water.
20.A species that can either donate or accept a hydroxide ion, such as Al(OH)3. Many chemistry texts incorrectly use this term to mean that a substance can act as either an acid or a base.
Down
1.Bronsted and Lowry define an acid as a proton (H+) donor and a base as a proton acceptor. Compare this model with the Arrhenius Model and the Lewis definitio
2.An acid with a pK a greater than zero. Weak acids do not completely dissociate in water.
3.A measure of the hydroxide ion concentration, it is equal to - log [OH-], where [OH-] is the concentration of hydroxide ions
7.A substance that has the potential to donate a proton or accept an electron pair.
9.An acid with a pK a less than zero. Strong acids completely dissociate in water.
10.A molecule of the form AOn(OH)m, where A is a non-metal.
11.A substance that can accept a proton, release OH-, or donate an electron pair.
13.A measure of the strength of an acid, it is equal to – log K a, where K a is the acid dissociation constant in water.
15.Having a pH less than 7 or a pOH greater than 7
21.A measure of the hydrogen ion concentration, it is equal to - log [H+], where [H+] is the concentration of protons.

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