Chapter 18 acids and bases study guide
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1. can turn litmus paper a different color
both
2. reacts with certain metals
acid
3. contains more hydrogen ions than hydroxide ions
acid
4. feels slippery
base
5. reacts with carbonates
acid
6. feels rough
neither
7. contains equal numbers of hydrogen and hydroxide neither
ions
8. tastes bitter
base
9. tastes sour
acid
10. the _____ model of acids and bases states that an
Arrhenius, hydroacid contains the element ____ and forms ions of this gen, hydroxide,
element when it is dissolved in water. a base contains hydroxide.
the ____ group and dissociates to produce ____ ions
in aqueous solution.
11. according to the ____ model, an acid donates ____ Bronsted-Lowry,
ions, and a base accepts ____ ions. according to this hydrogen,
model, in an acid-base reaction, each acid has a ____, hydrogen,
and each base has a ____.
conjugate base,
conjugate acid.
12. acid A and B are of equal concentration and are tested B.)acid B is
with a conductivity apparatus. When the electrodes stronger than acid
are placed in acid A, the bulb glows dimly. When they A.
are placed in acid B, the bulb glows more brightly.
Which of the following is true?
13. A chemical reaction for the ionization of an acid uses C.)the ionizing
a single arrow to the right to separate the reactant and acid is strong.
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Chapter 18 acids and bases study guide
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product sides of the equation. Which of the following
is true?
14. sulfuric acid is a strong acid. what is true about its
conjugate base?
C.)its conjugate
base is weak.
15. In solution, a weak acid produces
A.)a mixture of
molecules and
ions.
16. why are Ka values all small numbers?
D.)the solutions
contain a high
concentration of
un-ionized acid
molecules.
17. Which of the following dissociates entirely into metal B.)a strong base
ions and hydroxide ions in solution?
18. In general, compounds formed from active metals,
and hydroxide ions are
B.)strong bases
19. write the simplest form of the chemical equation for
the self-ionization of water.
H2O(1)-> H+(aq)+
OH-(aq)
20. write the equilibrium constant expression Keq, for this Keq=[H+][OH-]/[H2O]
equation
21. write the expression for the equilibrium constant for Kw=[H+][OH-]
water, Kw
22. why can the concentration of water be ignored in the the concentration
equilibrium expression for water?
of water molecules
is essentially constant.
23. what is the numerical value of Kw at 298K?
1.0 x 10^-14
24. in solution, if the hydroxide ions in solution is
1.0x10^-6, what is the hydrogen ion concentration?
[H+]=Kw/[OH-]=1.0x10
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Chapter 18 acids and bases study guide
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25. is the solution in question 7 acidic, basic, or neutral? basic because
explain.
[OH-] is greater
than 1.0x10^-7
26. the pH of a solution is the negative logarithm of its
hydroxide ion concentration
false; hydrogen
27. values for pH range from 0 to 14.
true
28. stomach contents can have a pH of 2, which means
that they are basic.
false; acidic
29. the hydrogen ion concentration in a solution with a
pH of 3 is two times greater than the hydrogen ion
concentration in a solution with a pH of 5.
false; 100`
30. the pHof a neutral solution at room temperature
equals the pOH of the solution
true
31. if the pHO of a solution is 3, its pOH is 10.
false;11
32. the pH of a solution with a [H+] of 1x10^-8 is 8
true
33. the pH of a solution with a [OH-] of 1x10^-6 is 6
false;8
34. what is the pH of a 4.3x10^-2M HCL solution? HCL is [H+]=4.3x10^-2
a strong acid.
MipH=-log(4.3x
10^-2) = 1.37
35. calculate the pHOf a 5.2x10^-3MH2SO4 solution?
NaOH is a strong base.
[OH]=2.5x10^-3M=1.0x
36. what is the pH of a 2.5x10^-5M NaOH solution? NaOH [is a strong base.
OH}=2.5x10^-5M;[H+]=
37. calculate the pH of a 3.6x10^-6M Ca(OH)2 solution.
Ca(OH)2 is a strong base.
[OH]=2x3.6x10^-6M=7.
38. indicator paper can be used to measure the ____ of a pH, colors, pH mesolution. indicators are substances that are different ter
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Chapter 18 acids and bases study guide
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____ depending on the pH of the solution tested. another way to measure the acidity of the solution is the
____, which uses electrodes placed in the solution to
directly read the results.
39. 1) a chemical dye that changes color based on the pH
of a solution
2) a method for using neutralization reaction to determine the concentration of a solution
3)a reaction in which an acid and a base react to
produce a salt and water
4)a solution of known concentration
5) an ionic product of an acid-base reaction
6)the point in titration in which an indicator changes
color
7)the stoichiometric point of a titration
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1)a
2)g
3)d
4)f
5)e
6)b
7)c