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Chem 102 > ch 14a-c > Flashcards

ch 14a-c Flashcards

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1
Q

What is the Arrhenius definition of an acid?

A

A substance that produces H+ ions in aqueous solutions.

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2
Q

What is the Arrhenius definition of a base?

A

A substance that produces OH- ions in aqueous solutions.

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3
Q

What is the Brønsted-Lowry definition of an acid?

A

A substance that donates H+ ions.

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4
Q

What is the Brønsted-Lowry definition of a base?

A

A substance that accepts H+ ions.

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5
Q

What are strong acids?

A

Acids that completely ionize in solution.

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6
Q

What is the acid ionization constant (Ka)?

A

A value used to compare the strength of weak acids, defined like an equilibrium constant.

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7
Q

What is the pH of a solution?

A

The negative logarithm of the hydronium ion concentration, pH = -log[H3O+].

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8
Q

What is the relationship between pH and acidity?

A

Acidic solutions have pH < 7, and basic solutions have pH > 7.

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9
Q

What is pKa?

A

The negative logarithm of the acid ionization constant, Ka, indicating the strength of an acid.

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10
Q

How can pKa predict the relative concentration of acid and conjugate base?

A

If pH > pKa, [A-] > [HA]; if pH < pKa, [A-] < [HA].

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11
Q

What are polyprotic acids?

A

Acids that have more than one acidic hydrogen, like H2SO3 (diprotic) or H3PO4 (triprotic).

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12
Q

How does bond polarity affect acid strength in binary acids?

A

Higher bond polarity often increases acid strength in binary acids (e.g., HCl is stronger than HF).

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13
Q

What are strong bases?

A

Bases that completely ionize in solution.

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14
Q

What is the base ionization constant (Kb)?

A

A constant used to measure the strength of weak bases.

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15
Q

How are Ka and Kb related?

A

For a conjugate acid-base pair, pKa + pKb = 14.

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16
Q

How do you find the pH of a strong base solution?

A

Calculate [OH-] and use pH = 14 - pOH.

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17
Q

What determines if an anion will act as a base?

A

Anions of weak acids are weak bases; anions of strong acids are generally pH-neutral.

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18
Q

How can you classify a salt solution as acidic, basic, or neutral?

A

Compare the Ka of the cation and the Kb of the anion; the ion with the larger value determines the pH.

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19
Q

What are the six common strong acids?

A

Hydrochloric acid (HCl), hydrobromic acid (HBr), hydroiodic acid (HI), nitric acid (HNO3), sulfuric acid (H2SO4), and perchloric acid (HClO4).

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20
Q

Why are these acids considered strong?

A

They completely ionize in water, releasing H+ ions fully in solution.

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21
Q

What is the formula for hydrochloric acid?

A

HCl

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22
Q

What is the formula for sulfuric acid?

A

H2SO4

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23
Q

What is unique about sulfuric acid (H2SO4) as a strong acid?

A

Only the first ionization (H2SO4 → H+ + HSO4-) is strong; the second ionization (HSO4- → H+ + SO4^2-) is weak.

24
Q

What are the six common strong bases?

A

Lithium hydroxide (LiOH), sodium hydroxide (NaOH), potassium hydroxide (KOH), calcium hydroxide (Ca(OH)2), strontium hydroxide (Sr(OH)2), and barium hydroxide (Ba(OH)2).

25
Q

Why are these bases considered strong?

A

They completely dissociate in water, releasing OH- ions fully in solution.

26
Q

What is the formula for sodium hydroxide?

A

NaOH

27
Q

What is the formula for calcium hydroxide?

A

Ca(OH)2

28
Q

What is a characteristic of strong bases with formulas like Ca(OH)2, Sr(OH)2, and Ba(OH)2?

A

They release two OH- ions per formula unit, making them highly basic.

29
Q

What is the Arrhenius definition of an acid?

A

A substance that produces H+ ions in aqueous solutions.

30
Q

What is the Arrhenius definition of a base?

A

A substance that produces OH- ions in aqueous solutions.

31
Q

What is the Brønsted-Lowry definition of an acid?

A

A substance that donates H+ ions.

32
Q

What is the Brønsted-Lowry definition of a base?

A

A substance that accepts H+ ions.

33
Q

What are strong acids?

A

Acids that completely ionize in solution.

34
Q

What is the acid ionization constant (Ka)?

A

A value used to compare the strength of weak acids, defined like an equilibrium constant.

35
Q

What is the pH of a solution?

A

The negative logarithm of the hydronium ion concentration, pH = -log[H3O+].

36
Q

What is the relationship between pH and acidity?

A

Acidic solutions have pH < 7, and basic solutions have pH > 7.

37
Q

What is pKa?

A

The negative logarithm of the acid ionization constant, Ka, indicating the strength of an acid.

38
Q

How can pKa predict the relative concentration of acid and conjugate base?

A

If pH > pKa, [A-] > [HA]; if pH < pKa, [A-] < [HA].

39
Q

What are polyprotic acids?

A

Acids that have more than one acidic hydrogen, like H2SO3 (diprotic) or H3PO4 (triprotic).

40
Q

How does bond polarity affect acid strength in binary acids?

A

Higher bond polarity often increases acid strength in binary acids (e.g., HCl is stronger than HF).

41
Q

What are strong bases?

A

Bases that completely ionize in solution.

42
Q

What is the base ionization constant (Kb)?

A

A constant used to measure the strength of weak bases.

43
Q

How are Ka and Kb related?

A

For a conjugate acid-base pair, pKa + pKb = 14.

44
Q

How do you find the pH of a strong base solution?

A

Calculate [OH-] and use pH = 14 - pOH.

45
Q

What determines if an anion will act as a base?

A

Anions of weak acids are weak bases; anions of strong acids are generally pH-neutral.

46
Q

How can you classify a salt solution as acidic, basic, or neutral?

A

Compare the Ka of the cation and the Kb of the anion; the ion with the larger value determines the pH.

47
Q

What are the six common strong acids?

A

Hydrochloric acid (HCl), hydrobromic acid (HBr), hydroiodic acid (HI), nitric acid (HNO3), sulfuric acid (H2SO4), and perchloric acid (HClO4).

48
Q

Why are these acids considered strong?

A

They completely ionize in water, releasing H+ ions fully in solution.

49
Q

What is the formula for hydrochloric acid?

A

HCl

50
Q

What is the formula for sulfuric acid?

A

H2SO4

51
Q

What is unique about sulfuric acid (H2SO4) as a strong acid?

A

Only the first ionization (H2SO4 → H+ + HSO4-) is strong; the second ionization (HSO4- → H+ + SO4^2-) is weak.

52
Q

What are the six common strong bases?

A

Lithium hydroxide (LiOH), sodium hydroxide (NaOH), potassium hydroxide (KOH), calcium hydroxide (Ca(OH)2), strontium hydroxide (Sr(OH)2), and barium hydroxide (Ba(OH)2).

53
Q

Why are these bases considered strong?

A

They completely dissociate in water, releasing OH- ions fully in solution.

54
Q

What is the formula for sodium hydroxide?

A

NaOH

55
Q

What is the formula for calcium hydroxide?

A

Ca(OH)2

56
Q

What is a characteristic of strong bases with formulas like Ca(OH)2, Sr(OH)2, and Ba(OH)2?

A

They release two OH- ions per formula unit, making them highly basic.

Chem 102 (1 decks)

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