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CHEM 1001 > Acids & Bases > Flashcards

Acids & Bases Flashcards

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1
Q

What is the arrhenius definition of an acid?

A

susbtances the produce H+, or H3O+ in aqueous solution

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2
Q

What is the arrhenius definition of a base?

A

substances that produce OH- in aqueous solution

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3
Q

What is the Bronsted-Lowry definition of an acid?

A

a proton (H+) donor

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4
Q

What is the bronsted-lowry definition of a base?

A

a proton (H+) acceptor

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5
Q

What are amphoteric substances? Examples?

A

substances that can act as either an acid or a base

H2O, H2PO4-, bicarbonate, amino acids

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6
Q

What is a conjugate acid-base pair? Examples?

A

consists of two substances that differ only by the presence of a proton

H2O is conjugate acid of OH-, OH- is conjugate base of H2O

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7
Q

What is the conjugate base of HCO3- if it reacts with water? What about the conjugate acid?

A

CO3-

H2CO3

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8
Q

What is the general equation for an acid reacting in water?

A

HA + H2O –> H3O+ + A-

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9
Q

If you put one mole of a strong acid into water what are the expected products?

A

would completely ionize (dissociate) and you would get one mole of H3O+ and one mole of the corresponding anion

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10
Q

What are some examples of strong acids?

A

hydrochloric acid (HCl), hydrobromic acid (HBr), Hydroiodic acid (HI), Nitric acid (HNO3), Perchloric acid (HClO4), Sulfuric acid (H2SO4)

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11
Q

If you put one mole of a weak acid into water what do you think will happen?

A

only partially ionize, amount that will ionize is reflected by the Ka value

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12
Q

What is the formula for Ka? What is ingored in this formula, why is it ignored?

A

Ka=[A-][H3O+]/[HA]

water, because its a solvent with a constant concentration

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13
Q

How can you tell which weak acid is stronger?

A

higher Ka means stronger and lower pka means stronger

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14
Q

What is the general equation for a base reacting in water?

A

NaOH + H2O –> Na+ + OH-

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15
Q

What are some strong bases?

A

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

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16
Q

What is the formula for Kb? What is ignored and why?

A

Kb=[BH+][OH-]/[B]

water, because its a pure solvent

17
Q

How can you tell which weak base is stronger?

A

bigger Kb, means stronger as well as smaller pKb

18
Q

What is the autoionization of water?

A

when water acts as an acid and a base by transfering a proton to another water

19
Q

What is the the Kw constant?

A

Kw=[H3O+][OH-]=1.0x10^-14

20
Q

How can you calculate the concentration of OH- using H3O+ concentration and Kw?

A

[OH-]=Kw/[H3O+]

21
Q

How can you calculate pH?

A

pH=-log[H3O+]

22
Q

What pH is basic, acidic, or neutral?

A

basic is greater than 7, acidic is less than 7, neutral is 7

23
Q

How can you calculate pOH?

A

pOH=-log[OH-]

24
Q

What equation can you use to find pH if you know pOH and vice versa?

A

pOH + pH = 14

25
Q

How can you calculate [H+] if you know pH?

A

10^-pH

26
Q

How can you calculate pKa and pKb?

A

pKa=-log(Ka)

pKb=-log(Kb)

27
Q

How can you find the pKa of a conjugate base pair if you know pKb and vice versa?

A

pKa + pKb = 14

only for conjugate acid-base pairs in water

28
Q

How can you calculate Ka or Kb if you know the other of a conjugate acid-base pair?

A

Kb x Ka = Kw

29
Q

How can you find pH of a weak acid/base?

A

ICE tables

30
Q

What is the formula for % ionization of a weak acid?

A

=[H3O+]/(initial acid concentration) x 100

31
Q

WHat is a general formula to find % ionization?

A

= square root (Ka/Ca) x 100

32
Q

If there is a mixture of acids, when can we find the pH?

A

if one acid is much stronger than the others, can ignore the other acids

33
Q

What is the properties of ions and salts for anions?

A

anions that are the conjugate base of a weak acid is itself a weak base, and anions that are the conjugate base of a strong acid is pH-neutral

34
Q

What is the properties of ions and salts for cations?

A

A cation that is the conjugate acid of a weak base is itself a weak acid, a cation that is the conjugate acid of a strong base is pH-neutral

35
Q

What are polyprotic acids?

A

can donate more than one proton

36
Q

If the Ka of the 1st proton for a polyprotic acid higher than the subsequent ones, why?

A

yes

the removal of a second and third H+ involves a separation of a positive charge (H+) from a negatively
charged anion, which are attracted by coulombic forces.

37
Q

How can you find the volume of a certain acid/base to make a solution with a certain pH and volume?

A

Find concentration of H+ or OH- (10^-pH or 10^-pOH)

Multiply that by the volume

Divide that by the concentration of the acid/base

CHEM 1001 (6 decks)

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