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General
Vocabulary
Titration
Conjugates
K Problems
pH problems
100

What is another name for a hydrogen atom?

Proton

100

Why is water described as amphoteric?

Because it acts as both an acid and a base

100
The products of a neutralization reaction are

water and a salt

100

What is the partner of a conjugate acid?

A base

100

What are the formulas for Ka and Kb?

Ka = [H+]2 / [HA]

Kb = [OH-]2 / [B]

100

If the hydrogen ion concentration is 2.3 x 10-3 M, what is the pH?

2.64

200

What is the range of the pH scale?

0-14

200

According to the Arrhenius definition, acids contain _____ and produce ______ and bases contain _____ and produce ______

hydrogen, hydrogen ions, hydroxide, hydroxide ions

200

What is the equivalence point? What is the end point?

Equivalence point - end of titration (when the known neutralizes the unknown)

End point - when the color of indicator changes

200

The stronger the conjugate base...

the weaker the acid

200

Write the Ka expression for the weak acid: 

H2CO3(aq) + H2O(l) = HCO3-1(aq)  + H3O+1(aq)

Ka = [HCO3-1] [H3O+1] / [H2CO3]   

or Ka = [HCO3-1] [H+1] / [H2CO3]  

200

Calculate the hydrogen ion concentration if the hydroxide ion concentration is 1.8 x 10-3 M and Kw = 1.0 x 10-14

5.56 x 10-12 M

300

What is present in a container of the weak acid, HF?

HF molecules and hydrogen (hydronium) ions and fluoride ions

300

What is a Bronsted-Lowry acid?

A hydrogen ion donor (or a proton donor)

300

If a strong base and a weak acid are titrated, the indicator should have a pH range of _____

8 - 9 or 10

300

Identify the base and conjugate acid pair in this reaction:  C6H5COOH + NH3 = C6H5COO-1 + NH4+1

Base = NH3 and conjugate acid is NH4+1

300

What is the hydroxide ion concentration for a 0.033 M base whose Kb is 5.6 x 10-4?

0.0043 M or 4.3 x 10-3 M

300

What is the hydrogen ion concentration of a solution with a pOH of 4.4 given the Kw = 1.0 x 10-14?

2.51 x 10-10 M

400

How much does the hydrogen ion concentration increase from pH 9 to pH 6?

concentration increases by 1000

400

What is the difference between a strong base and a weak base?

A strong base completely dissociates (splits) into ions; a weak base partially dissociates into ions 

400
What is the concentration of HBr if 11.5 mL of it are neutralized with 17.8 mL of 0.60 M KOH? (Write the BCE)

HBr +  KOH = H2O + KBr

0.93M

400

What is the conjugate acid of CrO4-2 ?

HCrO4-1

400

Find the pH of a 0.45 M acid whose Ka is 8.3 x 10-12

5.7

400

What is the pOH of a 0.125 M solution of NaOH?

0.9 or 9.0 x 10-1

500

Write the ionization for Ca(OH)2 and for H2SO4

Ca(OH)2 = Ca2+ + 2OH-1   and

H2SO4 = H+1  + HSO4-1

500

What solution resists a change in pH?

A buffer solution
500

15.00mL of a solution of calcium hydroxide is titrated with 9.88mL of 0.75 M hydrochloric acid. Calculate the molarity of the base (write the BCE) 

2HCl + Ca(OH)2 = 2H2O + CaCl2
0.25 M 
500

Write the dissociation of HMnO4 in water and label the acid, base, and conjugates

HMnO4 + H2O = MnO4-1 + H3O+1  (A + B = CB + CA)

500

Find the Kb for a 0.0156 M basic solution with a pH of 8.7?

1.61 x 10-9

500

Calculate the hydrogen ion concentration of a 0.33 M solution of Sr(OH)2 given the ionization constant Kw is 1.0 x 10-14.

1.52 x 10-14