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chemistry 1302 gen chem 2 > chapter 13: Acids and Bases > Flashcards

chapter 13: Acids and Bases Flashcards

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1
Q

what is an acid

A
  • have a sour taste and ability to dissolve metals
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2
Q

what is a base

A
  • bitter taste and feel slippery to the touch
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3
Q

what is the Arrhenius theory

A
  • acids increase the concentration of H+ ions in water
  • bases increase the concentration of OH- ions in water
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4
Q

what is a neutralization reaction and what does it produce

A

solution of an acid and a solution of a base are mixed

  • products of the reaction have none of the characteristic properties of the acidic or basic solution
  • produces water and a salt
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5
Q
A
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6
Q

what is a salt

A
  • any ionic compound whose cation comes from a base and anion comes from acid
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7
Q

what is the bronsted lowry theory

HA + B —> A + HB

A
  • acids are proton donors (have a removable acidic proton H+)
  • bases are proton acceptors ( lone pair of nonbonding electrons)
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8
Q

what is an amphoteric substance

A

a substance that can act as either an acid or base

HCL + H20 –> CL = H3O+

NH3 + H2O –> NH4+ + OH- aq)

* water is acting like a base and an acid*

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9
Q

what is a conjugate acid-base pair

A

acid and a base that differ only in the presence or absence of a proton

  • conjugate base: formed by removing a proton from an acid
  • conjugate acid: formed by adding a proton to a base

NH3 + H2O = NH4+ OH-

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10
Q

what are the 7 strong acids

A
  1. sulfuric acid H2SO4
  2. Hydrochloric HCL
  3. Hydrobromic HBr
  4. Perchloric HCLO4
  5. Chloric HCLO3
  6. Hydroiodic HI
  7. Nitric HNO3
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11
Q

what arrow do strong acids and bases use/ strong electrolytes /

what arrow do weak acids and bases/ weak electrolytes use

A
  1. one way arrow not equilibrium bc they dissociate completely
  2. weak acids and bases use equilibrium arrows bc they don’t dissociate completely
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12
Q
A
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13
Q

what is a polyprotic acid and monoprotic acid

A
  • monoprotic: 1 ionizable hydrogen
  • polyprotic: >1 ionizable hydrogen
  • polyprotic is strong and amphoteric conjugate base is weak
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14
Q

what group is in organic acids

A
  • carboxyl group and these acids are weak bc H atoms are not ionizable
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15
Q

what is Ka used for and what is Ka

A

Ka is the acid dissociation constant

  • used to express the extent to which weak acid ionizes
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16
Q

what does a greater Ka mean

A

stronger the acid

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17
Q

how does polarity affect acid strength

A
  • polarity depends on the strength of the H-Y bond
  • stability of the H-Y conjug. base
  • more polar means more acidic
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18
Q

how does bond strength affect acid strength

A
  • very strong bonds are less easily dissociated when weaker ones
  • strong bonds = strong acid strength
  • weak bonds =weak acid strength
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19
Q

what happens to the base when there is a stronger acid

A

the more stable it is = the less strong

* stronger the acid, the weaker its conjugate base*

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20
Q
  • how does acidity increase in the periodic table
A
  1. acidity increases from left to right
  2. top to bottom down a group
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21
Q

what is an oxyacid

A

OH groups and possible atoms are bound to a central atom

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22
Q

what is the rule of oxyacids

Y-O-H

A
  • electronegativity of Y increases, then will the acidity of the substance
  • as electron density is drawn toward the Y, the OH bond becomes weaker and more polar
    2. base of the conjug, base is usually an anion
23
Q

what is the rule for oxyacids that have the same number of O atoms

  • H-O-I (weakest weak)
  • H-O-Br
  • H-O- Cl (strong weak)
A
  • acid strength increases w. the increasing EN of the central atom
24
Q

what is the rule for oxyacids that have the same central atom

A
  • acid strengh increases as the number of oxygen atoms attached to the central atom increases

example:

HCLO -weakest

HCLO2 - weak

HClO3 - strong acid

HCLO4 - stronger acid

25
Q

wha tis the most important chemical properties of water related to bronsted and lowry

A
  • autoionization
  • act as a base or acid
  • in pure water a few molecules act as bases and a few act as acids
26
Q

what is the Kw expression and what does it equal

A

Kw = [H3O+][OH]

  • @ 25 degrees, Kw for water is 1.0x10^-14

* if you measure one of the conc. you can find the other*

27
Q

what happens if [H3O] increases

A

OH must decrease, and it is inverse

28
Q

what are neutral solutions

A

equal amounts of H3O and OH

and it equals 1x10^-7

29
Q

what are acidic solutions

A

larger [H3O] than [OH]

[H3O] >1x10^-7

[OH] < 1.0x10^07

30
Q

what is a basic solution

A

larger [OH] than [H3O]

[OH] > 1x10^-7

[H3O] < 1.0x10^-7

31
Q

what is the ph and what is the neutral number for pH

A
  • the acidity and bascity of a solution is expressed as pH
  • neutral pH = 7
32
Q

what does a low and high pH range mean and what is the normal range

A
  • low means acidic
  • high means basic
  • normal range is 0-14
33
Q

what is the rule of sig figs when using log to calculate pH

A

of decimal places in the log = the number of sig figs in the OG number

34
Q

what is the formula for pH and H3O

A
  • Ph = -log(H3O)

H3O = 10^-pH

35
Q

what is the formula for pOH and OH

A

pOH = -log[OH]

]OH] = 10^pOH

36
Q

what is the equation for pH and PoH

A

ph + PoH = pKw = 14.00

37
Q

in an aqeuos solution of strong acids what is the source of H+ ions and how do you calculate the pH

A
  • strong acid is the source and to calculate pH

[H3O] = [acid]

38
Q

how to calculate Ka for weak acids

A
  • use an ice table
  • proton transfers for weak acids are rapid
39
Q

what does percent ionization help us with

A

show how much of the weak acid has ionized

% ion = [H3O]equilibrium \ [HA] initial x 100

= 10-Ph/ Ha initial x 100

40
Q

what happens as the concentration of an acid increases

A

the strength decreases = pH decreases = % ionization also increases

41
Q

why does % ionization increases as an acid conc. increases

A
  • acid is diuluted by adding water, it shifts the equilibrium to the left ( increase in acid concentration)
  • to reach new equilibrium the acid needs to ionnize more
  • shift to the right ( H+ concentration)
42
Q

what are the strong bases

A
  1. LiOH
  2. NaOH
  3. KOH
  4. RbOH
  5. CsOH
  6. Ca(OH)2
  7. Sr(OH)2
  8. Ba(OH)2
43
Q

what do most weak bases contain

A

Nitrogen bc the lone pair makes it a great proton acceptor

44
Q

what is a weak base dissociation constant

A

Kb

B + H2O —> Hb + OH

45
Q

what can Kb be used to find

A
  • OH directly and pOH, PH and [H]

- greater value of Kb = stronger base

46
Q

what is the rule for polyprotic acids

A
  • polyprotic acids ionize in steps

H2SO3 is stronger than HSO3

Ka becomes smaller

47
Q

when calculating pH and you’re given 2 Ka what Ka should you use

A

the stronger Ka meaning the one that is the largest

48
Q

when does percent ionizatoin and pH both increase

A

as the acid becomes more dilute (less concentrated)

49
Q

if you are given a concentration like Ca(OH)2

what happens to the concentration

A

the concentration doubles because there are two hydroxides

50
Q

what is the factor of Ka value of successive losses of protons

A

10^3 or greater

51
Q

from polyprotic acids what can you use to determine the pH

A
  • you can use the first dissociation Ka1 to determine the Ka
52
Q
A
53
Q

what is the relationship between bond strength and acidity

A
  • weaker bond strength = proton more easily donated= increase in the strength of the acid

chemistry 1302 gen chem 2 (10 decks)

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