CH10 Acids and Bases

Question 1

Arrhenius Acid/Base definition

Answer 1

Acid: donates/dissociates H+ in solution (HCl, HNO3)

Base: donates/dissociates OH- in solution (NaOH, CaOH2)

Question 2

Bronsted-Lowry acid/base definition

conjugate acid/base?

Answer 2

Acid: donates H+

Base: Accepts H+

Conjugate acid: the molecules that receive the H+

Question 3

Lewis acid/base definition

Answer 3

Acid: accepts electrons

base: donates electro

one pair is shared in its entirety. (coordinate covalent bond formation)

Question 4

Amphoteric species

Answer 4

i.e H2O

under acidic condition behaves life a base H3O

under basic condition behaves like an acid OH-

Question 5

Oxygen suffixes and preffixes for quantity

suffixes for acids with o2

Answer 5

Hypo- =less HYPOchlorite (ClO)

ite=less Chlorite (ClO2)

ate= 1 more Chlorate (ClO3)

Per- = 1 more PERchlorate (ClO4)

ite = ous

ate = ic

Question 6

pH and pOH formulas

Answer 6

pH= - log {H+] = log 1/[H+]

Question 7

acid/base equilibrium constant Kw

what does affected?

Answer 7

only dependent on TEMP

changes in Conc, pressure or volume will NOT affected

Question 8

how to get the P value from a concentration

[x] to pH

what is the pH of an acid with [H+] = 1.8 x 10^-5 ?

Answer 8

-log(n x 10^-m)

what is the pH of an acid with [H+] = 1.8 x 10^-5

pH= -log (1.8 x 10^-5) = 5 - log 1.8 = 5 - 0.18

Question 9

Strong Acids, do they form unstable or stable conjugate bases?

Answer 9

1. HCl
2. HBr
3. HI
4. H2SO4 sulfuric acid
5. HNO3 Nitric acid
6. HClO4 Perchloric Acid

the stronger the acid the more stable the conjugate base

Question 10

Strong bases

Answer 10

KOH

NaOH

and other soluble hydroxides with group 1 or 2

Question 11

Ka of acid

and

which one is a stronger acid pka:10 or pKa:20

Answer 11

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

the smaller the Ka the weaker the acid (there is more HA did not dissociate)

pKa:10 is a stronger acid. the smaller pka the stronger the acid

Question 12

electronegativity and acidity what is the relationship?

Answer 12

Acid molecules with a highly electronegative element near where the H is attached will make it easier to donate

since its pulling e- away from the site of where the H is bonded

Question 13

what is Kb x Ka

and what is pKa + pKb

Answer 13

= 1.0 x 10^-14= Kw

Question 14

Strong acid + Strong base

what happens

Answer 14

HCl + NaOH = H2O + NaCl

all salt, SB and SA neutralize each other

Question 15

Strong acid + weak base

what happens increase or decrease pH?

Answer 15

HCl + NH3 = NH4+ Cl-

NH4 will react with H2O and donate its Hs making more H3O+ therefore decreasing the pH making it more acidic

Question 16

Strong base + Weak Acid

what happens?

increase or decrease pH?

Answer 16

NaOH + CH3COOH = H2O + Na+ CH3COO-

CH3COO- will react with h2o

CH3COO- + H2O = CH3COOH + OH-

it will make the solution more basic it will increase pH

Question 17

pH of a buffer solution Henderson-Hasselbalch equation

Answer 17

pH= pKa + log [B+]/[BOH]

Question 18

Formula at equivalence for acid/base titration

Answer 18

NaVa=NbVb

N is the acid/base normalities

Question 19

Titration Curve and labels, where is pKa, where is equivalence point

Answer 19

Question 20

what is the gram equivalent of phosphoric acid?

problem

Answer 20

Question 21

Normality problem

Answer 21

Question 22

Titration what is it used for?

Answer 22

It is to determine the concentration (molarity) of a known solution. i.e solution with HCl is titrated with NaOH