Chapter 15: Acid and Bases Definitions

Arrhenius Acid

substance that increases the concentration of Hydronium Ion (H3O+) when dissolved in water.

Arrhenius Base

substance that increasses the concentration of Hydroxide (OH-) when dissolved in water.

6 Strong Acids

HI, HClO4, H2SO4, HBr, HCl, HNO3

6 Strong Bases

KOH, NaOH, LiOH, Ca(OH)2, Sr(OH)2, Ba(OH)2

Bronsted Lowry Acid

substance that donates a proton (H+) to another substance, forming a covalent bond.

Bronsted Lowry Base

substance that accepts a proton from another substance.

Conjugate Acid

Has one proton that it donates to its conjugate base pair. (one hydrogen donation)

Conjugate Base

Has one less proton than the conjugate acid.

Lewis Acid

substance that accepts electron pair from another substance.

Lewis Base

Substance that donates an electron pair to another substance.

Can the conjugate base of a strong acid accept a proton from H2O?

it cannot.

What is the constant for water autoionization?

Kw = 1.0 × 10^-14

what is the equation to find pH?

-log (H+) = pH

what is the equation to find pOH?

pOH = -log (OH-)

what is the equation that equals 14?

pH + pOH = 14

what does (H+) = ?

10^-pH

what counts as significant when calculating pH and p(OH-)?

only the numbers after the decimal point.