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CHEM 1C > Unit 2- Acid/Base Chemistry > Flashcards

Unit 2- Acid/Base Chemistry Flashcards

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1
Q

Define Acid-Base Reaction

A

A reaction in which a hydrogen ion is transferred from one species to another.

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2
Q

Define Denaturation

A

Unfolding off the protein due to the transfer of hydrogen ions.

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3
Q

Antacids contain _____ compounds that react with the stomach acid to produce water.

A

Basic

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4
Q

Define Acid

A

An acid is a substance that produces H+ or (H3O+) ions in solution.

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5
Q

Define Base

A

A substance that produces OH- ions in aqueous solutions.

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6
Q

Define Neutralization Reaction

A

Occurs when an acid is added to a base (or vice versa). In a neutralization reaction, the H+ produced by the acid reacts with OH- produced by the base to form H2O.

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7
Q

How does one identify the substance that is an acid and a base?

A

Acids DONATE protons and Bases ACCEPT protons.

AD-BA

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8
Q

What are the strong acids?

A

Hydrochloric-Hydrobromic-Hydroiodic-Nitric-Sulfuric-Perchloric

TRIPLE H- SNP

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9
Q

What are the strong bases?

A

Sodium Hydroxide-Lithium Hydroxide-Potassium Hydroxide-Calcium Hydroxide-Barium Hydroxide-Strontium Hydroxide

SLP-CBS

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10
Q

What are the weak acids and what are their formulas?

A

Hydrofluoric (HF)- Formic (HCHO2)-Acetic (C2H3O2)

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11
Q

What is the definition of a Brønsted-Lowry acid/base respectively?

A

A compound that donates a proton to another compound is a Brønsted-Lowry acid and a compound that accepts the proton is regarded as a Brønsted-Lowry base.

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12
Q

What is the definition of an Arrhenius base and acid?

A

An Arrhenius base is a substance that increases OH- in solution and an Arrhenius acid is a substance that increases H+ in solution.

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13
Q

Define Conjugate Base

A

The product that remains after an acid donates a proton is called the conjugate base of the acid.

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14
Q

Define Conjugate Acid

A

The product that results when a base accepts a proton is called the base’s conjugate acid.

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15
Q

Do all acid-base reactions involve the transfer of protons between acids and bases?

A

Yes

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16
Q

Define Acid Ionization Reaction

A

The reaction between a Brønsted-Lowry acid and water is called an acid ionization reaction.

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17
Q

Define Base Ionization Reaction

A

When a Brønsted-Lowry base reacts with water, the reaction is called a base ionization reaction.

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18
Q

Define Autoionizaiton

A

When one molecule of a substance reacts with another molecule of the same substance to form ions, the reaction is called an autoionization reaction.

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19
Q

What type of reaction is the autoionization of water?

A

Endothermic

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20
Q

Where does the equilibrium of the autoionization of water lay?

A

The equilibrium of that reaction lies far to the left; this means that it is reactant dominant.

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21
Q

Define Amphiprotic

A

Molecules and ions that may either gain or lose a proton under certain conditions are said to be amphiprotic.

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22
Q

What is the equation for Kw? What are some important things to notice regarding the concentrations of hydronium and hydroxide?

A

Kw= [H3O+][OH-]=1x10^-14

The concentrations of H3O+ and OH- are inversely proportional and they impact the solution properties and solute behavior.

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23
Q

What is meant when a solution is considered neutral?

A

It contains equal concentrations of hydronium and hydroxide ions.

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24
Q

What is meant when a solution is acidic?

A

It contains a greater concentration of hydronium ions compared to hydroxide ions.

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25
Q

What is meant when a solution is considered basic?

A

It contains greater concentrations of hydroxide compared to hydronium.

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26
Q

What are the formulas for pH and pOH?

A

PH= -log[H3O+] ; pOH= -log [OH-]

The logs have a base 10.

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27
Q

What is important to remember regarding the formation of hydronium and hydroxide ions?

A

Every time you form H+, you will also form a bit of OH-.

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28
Q

What is the formula for determining the concentration of hydronium and hydroxide when provided the pH and pOH respectively?

A

10^-pH=[H3O+]
10^-pOH=[OH-]

29
Q

When reading the pH and pOH values, what are the guidelines for determining the number of significant figures?

A

Only the values present after the decimal count as the significant figures.

30
Q

How can the relative strengths of acids be determined?

A

From their equilibrium constants.

31
Q

In solutions of the same concentration, how do stronger acids behave?

A

They IONIZE to a greater extent.

32
Q

What does a Larger Ka signify?

A

Higher concentration of [H+] and a stronger acid.

33
Q

How do weak acids/bases behave in solution?

A

They have PARTIAL dissociation.

34
Q

What is the formula for calculating percent ionization?

A

% Ionization= [H3O+]eq/[HA]0 x 100

35
Q

What do monoprotic and diprotic mean respectively?

A

Monoprotic means that there is one ionizable hydrogen atom whereas diprotic means that there are 2 ionizable hydrogens.

36
Q

How do you treat equilibrium calculations in the case that you have 2 ionization reactions?

A

If Ka1>20 x Ka2, you must treat the first ionization separately and use the results to calculate the resultes of the second ionization.

37
Q

Mixing an acid and a base can result in a _____ reaction.

A

Neutralization

38
Q

Do you always end up with a neutralization reaction when you mix acids and bases together?

A

No, you must take a look at the conjugate partners.

39
Q

What is the result of mixing a strong acid and a strong base?

A

You end up with a neutral solution because the conjugate partners are of negligible strength.

40
Q

What can be said about the conjugate base/acid of a strong acid/base? What about a weak one?

A

Weak acids/bases will give rise to weak conjugate bases/acids; conjugate bases/acids of a strong acid/base do NOTHING in solutions.

41
Q

What happens when you mix a strong acid with a weak base?

A

You end up with a slightly acidic solution; the conjugate acid of the weak base is slightly ACIDIC.

42
Q

What happens when you mix a weak acid with a strong base?

A

You end up with a slightly basic solution; the conjugate base of the weak acid is slightly basic.

43
Q

How do you determine if a salt is going to be basic/acidic/neutral in solution?

A

You write the dissociation reaction for the salt. Then, you determine if the dissociated ions are conjugate acids/bases of a weak acid/base or a strong acid/base. If it is a conjugate partner of a weak acid/base, then it will affect the pH and make it slightly basic/acidic accordingly.

44
Q

How do amphiprotic anions impact the pH?

A

You must compare the kB and kA values for each ion. Whichever one is bigger will have the greater affect.

45
Q

Solutions containing metal ions will often be _____.

A

Slightly acidic

46
Q

Define Buffer

A

A mixture that can resist changes in pH is called a buffer.

47
Q

Define Buffer Solution

A

A mixture of a weak acid and its conjugate base (or a mixture of a weak base and its conjugate acid) is called a buffer solution, or buffer. Buffer solutions resist a change in pH when small amounts of strong acid or strong base are added.

48
Q

Could you make a buffer out of a strong acid/base?

A

No

49
Q

What is the formula for the Henderson-Hasselbalch Equation?

A

PH= pKa+log [A-]/[HA]

50
Q

What is a Lewis Acid?

A

A Lewis acid is an electron pair ACCEPTOR.

51
Q

What is a Lewis Base?

A

A Lewis base is an electron pair DONOR.

52
Q

Which substances are able to have an expanded octet?

A

Substances that are located from the 3rd period (ROW) and below.

53
Q

For the purposes of this class. what will the product of an acid base reaction be?

A

It will be water and an ionic compound (salt)

54
Q

How does the addition of a strong acid impact the equilibrium of a buffer reaction?

A

It will shift it to the left; hydronium will react with the conjugate base to produce more weak acid. MORE ACIDIC

55
Q

How does the addition of a strong base impact the equilibrium of a buffer reaction?

A

it will shift the equilibrium to the right; the OH- will react with the weak acid to produce more conjugate base. MORE BASIC

56
Q

What is the equation for the addition of weak acid to water?

A

HA+ H2O —-> H3O+ (A)-

57
Q

What is the equation for the addition of weak base to water?

A

B+H2O —-> (BH+)+ (OH-)

58
Q

When dealing with strong-strong titrations, how is the pH determined before the titrations has been added?

A

The pH is simply determined by taking the -Log of the concentration of the substance provided; since the titrant has not been added, there is only 1 substance to work with.

59
Q

When dealing with strong-strong titrations, how is the pH determined before the equivalence point?

A

There will be excess moles of one substance; subtract the limiting from the excess and divide by the total volume to determine concentration. Then, calculate the pH.

60
Q

When dealing with strong-strong titrations, how is the pH determined at the equivalence point?

A

There will be equal concentrations of hydroxide and hydronium ions; so, the pH will be 7.

61
Q

When dealing with strong-strong titrations, how is the pH determined after the equivalence point?

A

There will be an excess of one of the substances; subtract the limiting from the excess and determine the concentration accordingly. Then, calculate for pH.

62
Q

When dealing with weak-strong titrations, during which stages is the ICE table used?

A

Before the addition of TITRANT AND at the equivalence point.

63
Q

When dealing with weak-strong titrations, how is the pH determined before titrant has been added?

A

Through using the Ka of the acid and using an ice table.

64
Q

When dealing with weak-strong titrations, how is the pH determined before the equivalence point?

A

You calculate the moles of weak acid and its conjugate base; you then subtract the moles of the conjugate from the weak substance and divide by the total volume to determine the concentration. Once the concentrations of the substances have been calculated, you use the Ka value to determine the concentration of the HYDRONIUM ion.

65
Q

When dealing with weak-strong titrations, how is the pH determined at the equivalence point?

A

You calculate the moles of the substance and divide it by the total volume; then, you use an ICE table and the according Ka/Kb value to determine the necessary concentrations to figure out pH.

66
Q

When dealing with weak-strong titrations, how is the pH determined after the equivalence point?

A

Once of the substances will be in excess; so, figure that out in terms of moles and determine the concentration of the substance by dividing it by the total volume. Finally, calculate pH and pOH accordingly.

67
Q

Based off a titration curve, how do you know what type of substance is being titrated by what type of substance?

A

If the substance has a strong nature, it will be extremely resistant to changes in pH in the beginning. (The curve will be relatively flat)

If the substance has a weak nature, it will be sensitive to the titrant being added (thus, there will be a dramatic change in pH with the small addition of a titrant)

68
Q

How do you know what type of indicator to use for titrations?

A

The indicator must have a noticeable color change at the equivalence point (when the moles of acid and base are equivalent to one another)

CHEM 1C (5 decks)

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