DAT chemistry 7 - acid base equilibria and titratins

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Last updated 4:33 AM on 6/3/26
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48 Terms

1
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arrehnius acids

substance that donates H+ ions in water

<p>substance that donates H+ ions in water </p>
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arrehnius bases

Substance that doantes OH- in aqeous solution

<p>Substance that doantes OH- in aqeous solution</p>
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Bronstead acid

substance that donates protons

<p>substance that donates protons</p>
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Bronstead base

substance that accepts protons

<p>substance that accepts protons</p>
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lewis acid

substance that accepts electrons

<p>substance that accepts electrons </p>
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lewis base

substance that donates electrons

<p>substance that donates electrons </p>
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how to draw conjugate bases

add a proton and -1 to the charge

<p>add a proton and -1 to the charge </p>
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how to draw conjugate acids

remove a proton and +1 to the charge

<p>remove a proton and +1 to the charge </p>
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amphoteric

a substance that can act as both an acid and a base

<p>a substance that can act as both an acid and a base</p>
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amphiprotic

substance that can be both a proton acceptor and donor

(works when talking about bronstead lowry bases and acids)

<p>substance that can be both a proton acceptor and donor </p><p>(works when talking about bronstead lowry bases and acids) </p>
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kw

1×10^-14

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why is water ph neutral

pure water’s neutral ph due to the fact that pure water autoionizes to form equal amounts of H3O+ and OH-

<p>pure water’s neutral ph due to the fact that pure water autoionizes to form equal amounts of H3O+ and OH-</p>
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What happens if you increase the temperature of water

it changes ph, as kw changes with temp

<p>it changes ph, as kw changes with temp </p>
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monoprotic acids

completley dissacociates in water,

resulting in 0.1 mols of H+ and 0.1 mols of conjugate base if acid has a concentration of 0.1

<p>completley dissacociates in water,</p><p></p><p>resulting in 0.1 mols of H+ and 0.1 mols of conjugate base if acid has a concentration of 0.1</p>
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polyprotic acids

first H+ completley dissacociates in water, while conjugate will dissacociate a bit further

resulting in 0.1+ mols of H+ and 0.1 mols of conjugate base if acid has a concentration of 0.1

<p>first H+ completley dissacociates in water, while conjugate will dissacociate a bit further </p><p></p><p>resulting in 0.1+ mols of H+ and 0.1 mols of conjugate base if acid has a concentration of 0.1</p>
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Dihydroxide bases

completley dissacociate, producing 0.1 of metal and 0.2 of OH-

<p>completley dissacociate, producing 0.1 of metal and 0.2 of OH-</p>
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Binary acid strengths

left to right - atom is more electronegative

top to down - atoms get larger, electrons can distribute more

<p>left to right - atom is more electronegative </p><p>top to down - atoms get larger, electrons can distribute more </p>
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Oxyacids

acids with at least one oxygen and some other element (called a heteroatom)

<p>acids with at least one oxygen and some other element (called a heteroatom)</p>
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Oxyacid strength trend - oxygen amount

the more oxygens, the more resonance, the more stable the conjugate base is

The more acidic the oxyacid

<p>the more oxygens, the more resonance, the more stable the conjugate base is </p><p></p><p>The more acidic the oxyacid </p>
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Oxyacid strength trend - heteroatom

the more electronegative the atom, the more dipole induction, the more acidic the oxyacid

<p>the more electronegative the atom, the more dipole induction, the more acidic the oxyacid </p>
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ph calculation

-log [H+]

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Poh scale

as opposed to ph, it portrays Oh concentration

<p>as opposed to ph, it portrays Oh concentration </p>
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poh calculation

-log [OH-]

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When does a strong base not affect a solution

when the reulting H+ concentration is less than 10^-7

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shortcut to find H3O given Ka and HA

H30 = Sqrt(Ka[HA])

<p>H30 = Sqrt(Ka[HA])</p>
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shortcut to find OH given Kb and A-

OH- = Sqrt(Ka[A-])

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how to calculate pKa and pKb

pKa or pkb = -log [ka or Kb]

<p>pKa or pkb = -log [ka or Kb]</p>
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how to calculate Ka or kb using Kw

Kw = Ka*Kb

<p>Kw = Ka*Kb</p>
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Pka+Pkb

14

<p>14</p>
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Neutralization reactions

Reactions between acids and bases that always make H2O and a salt

type of mettheisis reaction

<p>Reactions between acids and bases that always make H2O and a salt </p><p></p><p>type of mettheisis reaction</p>
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What PH does a reaction between two strong acids and bases result in?

a pH of 7.0

<p>a pH of 7.0</p>
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What does a neutralization reaction between a strong base and a weak acid result in

a ph above 7.0

<p>a ph above 7.0</p>
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What does a neutralization reaction between a strong acid and a weak base result in

a ph bellow 7.0

<p>a ph bellow 7.0</p>
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neutralization reactions equation

na MA VA = nb MB VB

<p>na MA VA = nb MB VB</p>
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normality

mols/liter, whats actually in the solution, as opposed to molarity, which only portrays what you dissolved in it in mols/liter

<p>mols/liter, whats actually in the solution, as opposed to molarity, which only portrays what you dissolved in it in mols/liter</p>
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How to increase the solubility of a salt that forms a basic anion

decrease the pH adding H+ syphons off the acidic cation

<p>decrease the pH adding H+ syphons off the acidic cation</p>
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How to increase the solubility of a salt that forms an acidic cation

lower the Ph, removing acids syphons off the acidic cation

<p>lower the Ph, removing acids syphons off the acidic cation</p>
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How are acidic buffers made

by combining a weak acid with a source of its conjugate base

<p>by combining a weak acid with a source of its conjugate base</p>
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How are basic buffers made

adding a weak base alongside its conjugate acid

<p>adding a weak base alongside its conjugate acid </p>
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Whats another way of making a basic buffer

adding 2 parts weak base to 1 part strong acid, which will lead to the strong acid being completley used up, and in turn generating the conjugate acid of the weak base in a 1:1 ratio

<p>adding 2 parts weak base to 1 part strong acid, which will lead to the strong acid being completley used up, and in turn generating the conjugate acid of the weak base in a 1:1 ratio</p>
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Whats another way of making a acidic buffer

adding 2 parts weak acid to 1 part strong base, which will lead to the strong acid being completley used up, and in turn generating the conjugate base of the weak acid in a 1:1 ratio

<p>adding 2 parts weak acid to 1 part strong base, which will lead to the strong acid being completley used up, and in turn generating the conjugate base of the weak acid in a 1:1 ratio</p>
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how range do buffers work in

+- range arounf target pH

<p>+- range arounf target pH</p>
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Titrations

when looking to find the concentration of a strong acid, you can add a weak base in incrmemental amounts until the ph is 7. this is when the concentration of the acid is equal to that of the base .

<p>when looking to find the concentration of a strong acid, you can add a weak base in incrmemental amounts until the ph is 7. this is when the concentration of the acid is equal to that of the base .</p>
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Equivalence point

when the concentration of the acid is equal to that of the base .

<p>when the concentration of the acid is equal to that of the base .</p>
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Titrant

solution that has a known concentration

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titrand

unknown solution

<p>unknown solution</p>
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half equavalence point

the pka, where HA =A-

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Polyprotic titrations

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