acids and bases

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25 Terms

1
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define an acid in Arrhenius’ model

substances yielding hydronium ions

2
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define a base in the Arrhenius Model

substances yielding hydroxide ions

3
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define an acid in the Bronsted-Lowry Model

any substance capable of donating hydrogen ion or proton to another substance (proton donors)

4
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define a base in the Bronsted-Lowry Model

any substance capable of accepting a proton or hydrogen from another substance (proton acceptors)

5
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why is water considered amphoteric?

water can act as either an acid or as a base

6
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if an acid is strong, how much does it dissociate in water?

completely

7
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if an acid is weak, how much does it dissociate in water

only dissociate to a very small percentage

8
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what is a weak base?

a base which is only slightly dissociates in aqueous solution

9
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what is a strong base?

a base which is highly dissociated in aqueous solution

10
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What are the five strong bases?

NaOH, KOH, RbOH, Ca(OH)2, Ba(OH)2

11
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what characteristic makes acids strong (easily dissociated)?

bond length - the longer it is, the stronger the acid is

12
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what are the five strong acids?

HCl, HBr, H2SO4, HNO3, and HClO4

13
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what does it mean if an acid is monoprotic?

it has 1 acidic proton (ex: HCl)

14
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what does it mean if an acid is diprotic?

it has 2 acidic protons (Ex: H2SO4

15
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What two things determine how strong an acid is?

  • in strong acids, the hydrogen is bonded either to a very electronegative element or to an oxygen bonded to a non-metal

  • in this oxyacids, the strength of the acid increases with the electronegativity of the non-metal (ex: H2SO4 strong, H3PO4 weak) and the number of oxygens present (ex: HNO3 strong, HNO2 weak)

16
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Draw the relationship between [H3O+], [OH-], pH, and pOH (the square of calculations)

knowt flashcard image
17
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what is the calculation for how water acts as its own acid and conjugate base

2H2O ←→ H3O+ + OH-

18
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What is Kw at 25 degrees

1 × 10-14

19
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how does the pH range change as temperature increases

decreases as temperature increases

20
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what will the Ka value be if the acid is strong?

very high

21
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what will the Ka value be if the acid is weak?

very small

22
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if the pKa is lower, the acid is ____; if the pKa is high, the acid is ____ (strong/weak)

strong, weak

23
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what is the relationship between Kw, Ka, Kb (formula)

Kw=KaKb

24
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what is the relationship between an acid and it’s conjugate base?

the stronger the acid (easier to give away H+), the weaker its conjugate base (less willing to accept H+)

25
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which does equilibrium prefer in acid-base reactions and why? (weaker or stronger?)

prefers the production of the weaker acid and base

  • the stronger the reacting acid and base, the more complete the reaction