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43 Cards in this Set
- Front
- Back
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According to the Arrhenius concept, if HNO3 were dissolved in water, it would act as ________.
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B) an acid
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The name given to an aqueous solution of HBr is ________.
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B) hydrobromic acid
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The name of HClO is ________.
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E) hypochlorous acid
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For Kw, the product of [H3O+] and [OH-] is ________.
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A) 1 × 10-14
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What is the [H3O+] in a solution with [OH-] = 1.0 × 10-12 M?
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E) 1.0 × 10-2 M
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What is the [OH-] in a solution that has a [H3O+] = 1.0 × 10-6 M?
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C) 1.0 × 10-8 M
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A solution with a pH of 4 is
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B) moderately acidic.
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The [H3O+] of a solution with pH = 2.0 has a concentration of ________.
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D) 1 × 10-2 M
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In which of the following are the pH values arranged from the most basic to the most acidic?
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C) 14, 10, 7, 4, 3, 1
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Which of the following is the strongest acid?
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E) HCl
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Which of the following is correctly identified?
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B) NaOH, strong base
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Ammonia is a weak base because
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D) it produces few hydroxide ions in water.
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An acid and base react to form a salt and water in a(n) ________ reaction.
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D) neutralization
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In a neutralization reaction,
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E) an acid and a base react to form a salt and water.
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Which of the following is a neutralization reaction?
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B) HNO3 + KOH → H2O + KNO3
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The function of a buffer is to
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B) maintain the pH of a solution.
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In a buffer system of HF and its salt, NaF,
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B) the HF neutralizes added base.
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Which of the following is a buffer system?
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C) H2CO3 and KHCO3
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Which of the following could be a buffer?
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B) HF + NaF
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What is the molarity of a KOH solution if 24.6 mL neutralizes 44.0 mL of a 0.211 M HCl?
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A) 0.377 M
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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
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How many milliliters of 0.100 M Ba(OH)2 are required to neutralize 20.0 mL of 0.250 M HCl?
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C) 25.0 mL
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The Ka for hydrofluoric acid is 7.2 × 10-4. This means that HF is
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C) a weak acid.
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) In a hydrochloric acid solution, where the [HCl] is 0.010 M, what is the pH?
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B) pH = 2.0
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The salt that contains the anion from a weak acid and the cation from a strong base should give a solution of
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C) pH > 7.
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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
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Acetic acid is an example of ________.
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A) a weak acid
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One example of an Arrhenius base is ________.
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B) KOH
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Water is an example of a(n) ________ compound.
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A) amphoteric
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In water solution, the conjugate base of HF is ________.
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A) F-
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The conjugate acid of NO2- is ________.
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B) HNO2
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Bicarbonate ion, HCO3-, is an example of a(n) ________.
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A) weak base
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The conjugate acid of NH3 is ________.
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D) NH4+
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The Ka for acetic acid, CH3COOH, is ________.
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D) Ka = [H+][CH3COO-]/[CH3COOH]
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The pH of a 0.05 M solution of potassium hydroxide, KOH, is ________.
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D) 12.7
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The pH of a solution of a solution is 4.50. The pOH of this solution is ________.
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D) 9.50
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Calculate the acid concentration of a sample of acid rain with a pH of 4.20.
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B) 6.3 × 10-5 M
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What is the pOH of a solution with a pH of 3.7?
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C) 10.3
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Stomach acid consists mainly of what substance dissolved in water?
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A) HCl
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When hydrochloric acid reacts with sodium carbonate, what gas results?
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C) CO2
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When potassium hydroxide reacts with sulfuric acid, one product is ________.
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C) H2O
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When zinc metal reacts with hydrochloric acid, one product is ________.
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C) H2
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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 ________.
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B) 4.74
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