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43 Cards in this Set

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According to the Arrhenius concept, if HNO3 were dissolved in water, it would act as ________.
B) an acid
The name given to an aqueous solution of HBr is ________.
B) hydrobromic acid
The name of HClO is ________.
E) hypochlorous acid
For Kw, the product of [H3O+] and [OH-] is ________.
A) 1 × 10-14
What is the [H3O+] in a solution with [OH-] = 1.0 × 10-12 M?
E) 1.0 × 10-2 M
What is the [OH-] in a solution that has a [H3O+] = 1.0 × 10-6 M?
C) 1.0 × 10-8 M
A solution with a pH of 4 is
B) moderately acidic.
The [H3O+] of a solution with pH = 2.0 has a concentration of ________.
D) 1 × 10-2 M
In which of the following are the pH values arranged from the most basic to the most acidic?
C) 14, 10, 7, 4, 3, 1
Which of the following is the strongest acid?
E) HCl
Which of the following is correctly identified?
B) NaOH, strong base
Ammonia is a weak base because
D) it produces few hydroxide ions in water.
An acid and base react to form a salt and water in a(n) ________ reaction.
D) neutralization
In a neutralization reaction,
E) an acid and a base react to form a salt and water.
Which of the following is a neutralization reaction?
B) HNO3 + KOH → H2O + KNO3
The function of a buffer is to
B) maintain the pH of a solution.
In a buffer system of HF and its salt, NaF,
B) the HF neutralizes added base.
Which of the following is a buffer system?
C) H2CO3 and KHCO3
Which of the following could be a buffer?
B) HF + NaF
What is the molarity of a KOH solution if 24.6 mL neutralizes 44.0 mL of a 0.211 M HCl?
A) 0.377 M
A 25.0 mL sample of H3PO4 requires 50.0 mL of 1.50 M NaOH for complete neutralization. What is the molarity of the acid?

H3PO4 + 3NaOH → Na3PO4 + 3 H2O
D) 1.00 M
How many milliliters of 0.100 M Ba(OH)2 are required to neutralize 20.0 mL of 0.250 M HCl?
C) 25.0 mL
The Ka for hydrofluoric acid is 7.2 × 10-4. This means that HF is
C) a weak acid.
) In a hydrochloric acid solution, where the [HCl] is 0.010 M, what is the pH?
B) pH = 2.0
The salt that contains the anion from a weak acid and the cation from a strong base should give a solution of
C) pH > 7.
If 2.00 g of Mg reacts completely with 50.0 mL of HCl solution, what is the molarity of the HCl solution?

Mg(s) + 2HCl(aq) → MgCl2 (aq) + H2(g)
E) 3.29 M
Acetic acid is an example of ________.
A) a weak acid
One example of an Arrhenius base is ________.
B) KOH
Water is an example of a(n) ________ compound.
A) amphoteric
In water solution, the conjugate base of HF is ________.
A) F-
The conjugate acid of NO2- is ________.
B) HNO2
Bicarbonate ion, HCO3-, is an example of a(n) ________.
A) weak base
The conjugate acid of NH3 is ________.
D) NH4+
The Ka for acetic acid, CH3COOH, is ________.
D) Ka = [H+][CH3COO-]/[CH3COOH]
The pH of a 0.05 M solution of potassium hydroxide, KOH, is ________.
D) 12.7
The pH of a solution of a solution is 4.50. The pOH of this solution is ________.
D) 9.50
Calculate the acid concentration of a sample of acid rain with a pH of 4.20.
B) 6.3 × 10-5 M
What is the pOH of a solution with a pH of 3.7?
C) 10.3
Stomach acid consists mainly of what substance dissolved in water?
A) HCl
When hydrochloric acid reacts with sodium carbonate, what gas results?
C) CO2
When potassium hydroxide reacts with sulfuric acid, one product is ________.
C) H2O
When zinc metal reacts with hydrochloric acid, one product is ________.
C) H2
The Ka for acetic acid, CH3COOH, is 1.8 × 10-5. A buffer, made from 0.10 M CH3COOH and 0.10 M CH3COO- has a pH of ________.
B) 4.74