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Terms in this set (54)
T/F-
...
According to the Arrhenius concept, if HNO3 were dissolved in water, it would act as _____________.
an acid
The name given to an aqueous solution of HBr is _____________.
hydrobromic acid
Which one of the following is characteristic of a base?
A) produces H3O+ in water
B) has a sour taste
C) has a slippery, soapy feel
D) turns blue litmus red
E) is insoluble in water
has a slippery, soapy feel
Which one of the following is characteristic of an acid?
A) produces
H3O+ in water
B) has a bitter taste
C) has a slippery, soapy feel
D) turns litmus blue
E) is insoluble in water
produces H3O+ in water
The name of Al(OH)3 is ____________.
aluminum hydroxide
Which of the following is identified correctly?
A) NH3, strong acid
B) NaOH, strong base
C) HCl, weak acid
D)
H2CO3, strong acid
E) Ca(OH)2, weak base
NaOH, strong base
According to the Bronsted-Lowry definition, ___________.
a base is a proton acceptor
Identify the Bronsted-Lowry acid in the following reaction.
H2O + CO32- → HCO3- + OH-
H2O
The conjugate acid of H2O is ____________.
H3O+
The conjugate base of H2O is ____________.
OH-
Ammonium hydroxide is a weak base because ______________.
it dissociates only slightly in water
Which of the following is the strongest acid?
A)
H3PO4
B) NH4+
C) NaOH
D) H2CO3
E) HCl
HCl
A chemical reaction has reached equilibrium when ____________.
the rate of the forward reaction equals the rate of the reverse reaction
Which of the following statements correctly describes the hydronium-hydroxide balance in the given solution?
A) In acids, [OH-] is
greater that [H3O+]
B) In bases, [OH-] = [H3O+]
C) In neutral solutions, [H3O+] = [H2O]
D) In bases, [OH-] is greater than [H3O+]
E) In bases, [OH-} is less than [H3O+}
In bases, [OH-] is greater than [H3O+]
What is the [H3O+] in a solution with [OH-] = 1 x 10-12 M?
1 x 10-2 M
What is the [OH-] in a solution that has a [H3O+] = 1 × 10-6 M?
1 x 10-8 M
What is the [H3O+] in a solution with [OH-] = 2.5 x 10-2 M?
4.0 x 10-13 M
What is the pH of a solution with [H3O+] = 1 x 10-9 M?
9.0
What is the pH of a solution with [OH-] = 1 x 10-4 M?
10.0
The [H3O+] of a solution with pH= 2.0 is _____________.
1 x 10-2 M
The [H3O+] of a solution with pH= 8.7 is ____________.
2 x 10-9 M
A solution with [ OH-] of 5 x 10-3 has a pH of ________.
11.7
The [H3O+] of a solution with pH= 9.7 is ______________.
2 x 10-10 M
An acid and base react to form a salt and water in a(n) ________ reaction.
neutralization
When an acid reacts with a metal like Al, the products are _____________.
a salt and hydrogen
Which of the following is the correctly balanced equation for the complete neutralization of H3PO4 by Ca(OH)2?
2H3PO4 (aq) + 3Ca(OH)2 (s) ----> Ca3(PO4)2 (aq) + 6H2O (l)
The neutralization reaction between Al(OH)3 and HNO3 produces the salt with the formula ____________.
Al(NO3)3
Which of the following is a neutralizatio reaction?
HNO3 (aq) + KOH (aq) -----> H2O (l) + KNO3 (aq)
25.0 mL of 0.212 M NaOH is neutralized by 13.6 mL of an HCl solution. The molarity of the HCl solution is ____________.
0.390 M
A 10.0 mL of 0.121 M H2SO4 is neutralized by 17.1 mL of KOH solution. The molarity of the KOH solution is __________.
0.142 M
The function of a buffer is to __________.
maintain the pH of a solution
Normal blood pH is about _______________.
7.4
In a buffer system of HF and its salt, NaF, ______________.
the HF neutralizes added base
Which of the following is a buffer system?
H2CO3 (aq) and KHCO3 (aq)
When hyperventilation (rapid breathing) causes a patient to exhale large amounts of CO2, the blood pH rises in a condition called ___________________.
respiratory alkalosis
T/F- The name of H2SO4 is hydrosulfuric acid
False
T/F- The name of NaOH is sodium hydroxide
True
T/F- Acids turn litmus blue
False
T/F- The conjugate base of H20 is H3O+
False
T/F- HF is a strong acid
False
T/F- When a system is at equilibrium, all concentrations are 1 M
False
T/F- KOH is a strong base
True
T/F- A system is at equilibrium when the rate of the forward and reverse reactions are equal
True
T/F- When more reactant is added to a system at equilibrium, the reverse reaction is favored
False
T/F- In any aqueous solution, [H3O+][OH-] = 1.0 x 10-7
False
T/F- In any aqueous solution, [H3O+] = [OH-]
False
T/F- If a solution has [H3O+] = 1.0 x 10-12 M, the [OH-] is also 1.0 x 10-12 M
False
T/F- An aqueous solution with [OH-] = 1.0 x 10-12 has a pH of 12.0
False
T/F- For many reactions of acids and bases, the resulting products are salt and water
True
T/F- Strong acids react with Zn metal to produce H2 gas
True
T/F- If the carbon dioxide level in the blood is too high, more carbonic acid is produced, and this results in the condition termed acidosis
True
T/F- Alkalosis is the blood condition in which the blood pH is higher than normal
True
T/F- A buffer is a solution that tends to maintain a neutral pH.
False
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