Common Acids & Bases
Properties & Strength
pH
Titration
Formulas
100
What is an acid?
An aqueous solution of a hydrogen compound.
100
What is the definition of a strong acid?
Acid that completely ionizes.
100
Draw and label the pH scale.
0 Acidic<----7 Neutral---->14 Basic
100
What is the term representing the pH at which the indicator changes color?

** DOUBLE JEOPARDY - 200 POINTS **

The end point.
100
pH + POH equals
14
200
Which compound below is an acid and which is a base?

NaOH, H2SO4

Acid: H2SO4

Base: NaOH

200
What substance do acids and bases ionize in?
Water (H2O)
200
Which molar concentration is greater in a basic solution?
[OH-]>[H3O+]
200
What is the term representing the pH at which the # moles of H30+ equals the # moles OH-, and at which the solution is neutralized?
The equivalence point.
200
What is the formula for molarity (M)?
M= moles solute/liters of solution
300
Which acid is commonly referred to as "stomach acid"?
Hydrochloric acid (HCl)
300
Give an example of a weak base and a strong base.
Weak base: OH with Group 1 or 2 metals

Strong base: OH with a non- Group 1 or 2 metal, NH3

300
How do you determine the significant figures when converting from pOH to [OH-]?

** DOUBLE JEOPARDY - 600 POINTS **

The significant figures are based on the number of decimals after pOH.

Ex: pOH=1.532 [OH-]=.029M

300
What is the first thing you always have to do when solving a titration problem?
Write the balanced equation.
300
What is the formula for a dilution?
M1V1 = M2V2
400
What is the formula and the name for "slaked lime"?
Ca(OH)2

Calcium Hydroxide

400
Write the ionization equation for NH3
NH3 + H2O > NH4 + OH-
400
If the [H3O+] of a solution is 1.4 × 10−3, then what is the pH?

REMEMBER SIG FIGS!

The pH is 3
400
How many milliliters of 0.0947 M NaOH are needed to neutralize 21.4 mL of 0.106 M HCl?
24.0 mL NaOH
400
[OH-] equals

[H3O+] equals

10-pOH

10-pH

500
What is an example of an organic acid?
Vinegar

CH3(OOH)

500
Explain why acids and bases are electrolytes.
Because they produce ions in solutions that move and carry the charge.
500
What is the pH of a solution with an [OH-] of 2.74 × 10−5?

REMEMBER SIG FIGS!

pH=7.438
500
If 26.4 mL of LiOH solution are required to neutralize 21.7 mL of 0.500 M HBr, what is the concentration of the basic solution?
.411 M LiOH
500
pOH equals

pH equals

-log[OH-]

-log[H3O+]

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