Name: 
 

Ch 19 - Acids, Bases and Salts



Matching
 
 
Match each item with the correct statement below.
a.
salt hydrolysis
d.
equivalence point
b.
end point
e.
buffer capacity
c.
titration
 

 1. 

process of adding a known amount of solution of known concentration to determine the concentration of another solution
 

 2. 

The number of moles of hydrogen ions equals the number of moles of hydroxide ions.
 

 3. 

Indicator changes color.
 

 4. 

Cations or anions of a dissociated salt remove hydrogen ions from or donate hydrogen ions to water.
 

 5. 

the amount of acid or base that can be added to a buffer solution before a significant change in pH occurs
 

Multiple Choice
Identify the choice that best completes the statement or answers the question.
 

 6. 

What is the formula for phosphoric acid?
a.
HPOmc006-1.jpg
c.
Hmc006-4.jpgPOmc006-5.jpg
b.
Hmc006-2.jpgPOmc006-3.jpg
d.
HPOmc006-6.jpg
 

 7. 

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

 8. 

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

 9. 

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

 10. 

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 is a hydrogen ion acceptor
d.
a substance that accepts an electron pair
 

 11. 

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

 12. 

In the reaction COmc012-1.jpgmc012-2.jpg + Hmc012-3.jpgO mc012-4.jpg HCOmc012-5.jpgmc012-6.jpg + OHmc012-7.jpg, the carbonate ion is acting as a(n) ____.
a.
Arrhenius base
c.
Arrhenius acid
b.
Brønsted-Lowry base
d.
Brønsted-Lowry acid
 

 13. 

What is the charge on the hydronium ion?
a.
1+
c.
2–
b.
0
d.
2–
 

 14. 

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

 15. 

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
 

 16. 

Which of these solutions is the most basic?
a.
[Hmc016-1.jpg] = 1 mc016-2.jpg 10mc016-3.jpgM
c.
[Hmc016-7.jpg] = 1 mc016-8.jpg 10mc016-9.jpgM
b.
[OHmc016-4.jpg] = 1 mc016-5.jpg 10mc016-6.jpgM
d.
[OHmc016-10.jpg] = 1 mc016-11.jpg 10mc016-12.jpgM
 

 17. 

An indicator is what type of compound?
a.
oxidizing agent
c.
salt
b.
strong base or acid
d.
weak base or acid
 

 18. 

What characterizes a strong acid or base?
a.
complete ionization in water
b.
ionic bonding
c.
presence of a hydroxide or hydrogen ion
d.
polar covalent bonding
 

 19. 

What is another name for the acid dissociation constant?
a.
ionization constant
c.
mole fraction
b.
equilibrium constant
d.
rate constant
 

 20. 

A 0.12M solution of an acid that ionizes only slightly in solution would be termed ____.
a.
strong and dilute
c.
dilute and weak
b.
concentrated and weak
d.
concentrated and strong
 

 21. 

Which of the following pairs consists of a weak acid and a strong base?
a.
nitric acid, calcium hydroxide
c.
acetic acid, sodium hydroxide
b.
acetic acid, ammonia
d.
sulfuric acid, sodium hydroxide
 

 22. 

A substance with a Kmc022-1.jpg of 1 mc022-2.jpg 10mc022-3.jpg would be classified as a ____.
a.
strong base
c.
weak base
b.
weak acid
d.
strong acid
 

 23. 

If an acid has a Kmc023-1.jpg = 1.6 mc023-2.jpg 10mc023-3.jpg, what is the acidity of the solution?
a.
acidic
c.
neutral
b.
The answer cannot be determined.
d.
basic
 

 24. 

Which base has the smallest base dissociation constant?
a.
ammonia
c.
calcium hydroxide
b.
sodium hydroxide
d.
potassium hydroxide
 

 25. 

In a titration, when the number of moles of hydrogen ions equals the number of moles of hydroxide ions, what is said to have happened?
a.
The equivalence point has been reached.
b.
The titration has failed.
c.
The point of neutralization has been reached.
d.
The end point has been reached.
 

Short Answer
 

 26. 

A liter of impure water has 10sa026-1.jpg mol of hydroxide ions. What is the concentration of hydronium ions in this sample of water?
 

 27. 

What is the hydrogen-ion concentration if the acid dissociation constant is 0.000 001 and the acid concentration is 0.01M?
 

 28. 

A 0.500M solution of a weak acid, HX, is only partially ionized. The [Hsa028-1.jpg] was found
to be 4.02 sa028-2.jpg 10sa028-3.jpgM. Find the dissociation constant for this acid.
 

 29. 

What is the pH if the hydrogen-ion concentration is 6.8 sa029-1.jpg 10sa029-2.jpgM?
 

 30. 

Calculate the acid dissociation constant of a weak monoprotic acid if a 0.5M solution of this acid gives a hydrogen-ion concentration of 0.000 1M?
 

Numeric Response
 

 31. 

If the hydrogen ion concentration is 10nr031-1.jpgM, what is the pH of the solution?

 

 32. 

If the hydroxide ion concentration is 10nr032-1.jpgM, what is the pH of the solution?

 

 33. 

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

 

 34. 

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

 

 35. 

What is the pH when the hydrogen ion concentration is 7.0 nr035-1.jpg 10nr035-2.jpgM?

 



 
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