Which one of the following is characteristic of a base?

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What are 3 characteristics of a base?
What is a characteristic of a base quizlet?

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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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