Name: 
 

Chapter 19 Test - Section 19.1 and 19.2


Matching (Value 5)
 
 
Match each item with the correct statement below.
a.
acid dissociation constant (Ka)
d.
Lewis acid
b.
diprotic acid
e.
pH
c.
hydrogen-ion donor
 

 1. 

 acid with two ionizable protons
 

 2. 

 ratio of the concentration of the dissociated to the undissociated form
 

 3. 

 can accept an electron pair
 

 4. 

 Brønsted-Lowry acid
 

 5. 

 negative logarithm of the hydrogen ion concentration
 

Multiple Choice (Value 24)
Identify the choice that best completes the statement or answers the question.
 

 6. 
Which of the following is a property of an acid?
a.
unreactive
c.
strong color
b.
nonelectrolyte
d.
sour taste
 

 7. 
What is transferred between a conjugate acid-base pair?
a.
an electron
c.
a hydroxide ion
b.
a hydronium ion
d.
a proton
 

 8. 
The formula of the hydrogen ion is often written as ____.
a.
Hmc008-1.jpg
c.
Hmc008-3.jpgNmc008-4.jpg
b.
OHmc008-2.jpg
d.
Hmc008-5.jpgOmc008-6.jpg
 

 9. 
What is the best description for a solution with a hydroxide-ion concentration of 1 mc009-1.jpg 10mc009-2.jpgM?
a.
acidic
c.
basic
b.
neutral
d.
The answer cannot be determined.
 

 10. 
Which of these solutions is the most basic?
a.
[OHmc010-1.jpg] = 1 mc010-2.jpg 10mc010-3.jpgM
c.
[Hmc010-7.jpg] = 1 mc010-8.jpg 10mc010-9.jpgM
b.
[OHmc010-4.jpg] = 1 mc010-5.jpg 10mc010-6.jpgM
d.
[Hmc010-10.jpg] = 1 mc010-11.jpg 10mc010-12.jpgM
 

 11. 
A Lewis acid is a substance that can ____.
a.
donate a hydrogen ion
c.
accept a pair of electrons
b.
donate a pair of electrons
d.
accept a hydrogen ion
 

 12. 
Which of these is an Arrhenius base?
a.
NHmc012-1.jpg
c.
CHmc012-5.jpgCOOH
b.
Hmc012-2.jpgPOmc012-3.jpgmc012-4.jpg
d.
LiOH
 

 13. 
In the reaction of aluminum bromide with ionized sodium bromide, which compound is the Lewis acid?
a.
aluminum bromide
c.
sodium ion
b.
bromide ion
d.
None are Lewis acids.
 

 14. 
In a neutral solution, the [Hmc014-1.jpg] is ____.
a.
zero
c.
1 mc014-3.jpg 10mc014-4.jpgM
b.
10mc014-2.jpgM
d.
equal to [OHmc014-5.jpg]
 

 15. 
Which compound can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base?
a.
ammonia
c.
hydrochloric acid
b.
water
d.
sodium hydroxide
 

 16. 
What are the acids in the following equilibrium reaction?
CNmc016-1.jpg + Hmc016-2.jpgO mc016-3.jpg HCN + OHmc016-4.jpg
a.
CNmc016-5.jpg, OHmc016-6.jpg
c.
Hmc016-9.jpgO, HCN
b.
Hmc016-7.jpgO, OHmc016-8.jpg
d.
CNmc016-10.jpg, Hmc016-11.jpgO
 

 17. 
Which hydroxide compound yields the lowest concentration of hydroxide ions in aqueous solution?
a.
potassium hydroxide
c.
magnesium hydroxide
b.
calcium hydroxide
d.
sodium hydroxide
 
p. 589
 

 18. 
When an acid reacts with a base, what compounds are formed?
a.
a salt and water
c.
a salt only
b.
metal oxides only
d.
water only
 

 19. 
What type of acid is sulfuric acid?
a.
triprotic
c.
diprotic
b.
monoprotic
d.
none of the above
 

 20. 
In the reaction COmc020-1.jpgmc020-2.jpg + Hmc020-3.jpgO mc020-4.jpg HCOmc020-5.jpgmc020-6.jpg + OHmc020-7.jpg, the carbonate ion is acting as a(n) ____.
a.
Brønsted-Lowry acid
c.
Arrhenius acid
b.
Brønsted-Lowry base
d.
Arrhenius base
 

 21. 
Which type of solution is one with a pH of 8?
a.
basic
b.
neutral
c.
acidic
d.
The type varies, depending on the solution.
 

 22. 
Which of the following reactions illustrates amphoterism?
a.
NaCl mc022-1.jpg Namc022-2.jpg + OHmc022-3.jpg
c.
Hmc022-7.jpgO + Hmc022-8.jpgO mc022-9.jpg Hmc022-10.jpgOmc022-11.jpg + OHmc022-12.jpg
b.
NaOH mc022-4.jpg Namc022-5.jpg + OHmc022-6.jpg
d.
HCl + Hmc022-13.jpgO mc022-14.jpg Hmc022-15.jpgOmc022-16.jpg + Clmc022-17.jpg
 

 23. 
If the hydrogen ion concentration of a solution is 10mc023-1.jpgM, is the solution acidic, alkaline, or neutral?
a.
alkaline
c.
acidic
b.
The answer cannot be determined.
d.
neutral
 

 24. 
What is an acid according to Arrhenius?
a.
a substance that is a hydrogen ion donor
b.
a substance that ionizes to yield protons in aqueous solution
c.
a substance that accepts an electron pair
d.
a substance that is a hydrogen ion acceptor
 

 25. 
What is a property of a base?
a.
watery feel
c.
strong color
b.
bitter taste
d.
unreactive
 

 26. 
Which of the following represents a Brønsted-Lowry conjugate acid-base pair?
a.
COmc026-1.jpgmc026-2.jpg and CO
c.
NHmc026-6.jpgmc026-7.jpg and NHmc026-8.jpg
b.
SOmc026-3.jpgmc026-4.jpg and SOmc026-5.jpg
d.
Hmc026-9.jpgO and Hmc026-10.jpg
 

 27. 
What is pH?
a.
the negative logarithm of the hydroxide ion concentration
b.
the positive logarithm of the hydrogen ion concentration
c.
the positive logarithm of the hydroxide ion concentration
d.
the negative logarithm of the hydrogen ion concentration
 

 28. 
The products of self-ionization of water are ____.
a.
Hmc028-1.jpgOmc028-2.jpg and Hmc028-3.jpgO
c.
OHmc028-6.jpg and OHmc028-7.jpg
b.
OHmc028-4.jpg and Hmc028-5.jpg
d.
OHmc028-8.jpg and Hmc028-9.jpg
 

 29. 
What is the formula for phosphoric acid?
a.
Hmc029-1.jpgPOmc029-2.jpg
c.
HPOmc029-5.jpg
b.
Hmc029-3.jpgPOmc029-4.jpg
d.
HPOmc029-6.jpg
 

Short Answer (Value 5)
 

 30. 
A liter of impure water has 10sa030-1.jpg mol of hydroxide ions. What is the concentration of hydronium ions in this sample of water?
 

 31. 
If the hydrogen-ion concentration is 1 sa031-1.jpg 10sa031-2.jpgM, what is the pOH of the solution?
 

 32. 
What is the ion-product constant for water?
 

Numeric Response (Value 10)
 

 33. 
If [OHnr033-1.jpg] = 1 nr033-2.jpg 10nr033-3.jpgM, what is the pH of the solution?

 

 34. 
What is the pH when the hydrogen ion concentration is 7.0 nr034-1.jpg 10nr034-2.jpgM?

 

 35. 
If the hydroxide ion concentration is 10nr035-1.jpgM, what is the pH of the solution?

 

 36. 
What is the pH of a solution with a concentration of 0.01M hydrochloric acid?

 

 37. 
If the hydrogen ion concentration is 10nr037-1.jpgM, what is the pH of the solution?

 



 
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