Unit 8: Acids and Bases

Neutralization reactions

________ occur when an acid donates its proton to a base.

weak acids

Indicators are ________ that change colors based on pH change.

Strong acids

________ will dissolve completely in water and never reach equilibrium.

1x10^-14

value of Kw constant

14

pH + pOH =

1x10^-14

\[H+\]\[OH-\] =

buffer

A(n) ________ is a solution with a stable pH.

Polyprotic acids

________ can give up more than one hydrogen in a solution.

Bases

________ do not dissociate but accepts protons.

equivalence point

When just enough acid/base is added to an acid/base to neutralize

half-equivalence point

when exactly half the amount of acid/base is turned into its conjugate in a titration

pH

Increasing ________ means decreasing [H+] and making a solution less acidic.

Greater Ka value

________ means more acid dissociation (stronger acid)

Greater Kb value

________ means more protonatization (stronger base)

Complete dissociation, only hydrogen and hydroxide ions remail

Strong acid and strong base reaction

Proton is donated, conjugate of base is created

Strong acid and weak base reaction

Protons accepted, created conjugate of acid and water

Weak acid and strong base

Simple proton transfer

Weak acid and weak base reaction

Ka

equilibrium constant for weak acids

Kb

equilibrium constant for weak bases