Acid-Base Equilibrium Systems

Question 1

what are acids according to Arrhenius’s theory

Answer 1

substances that produce a hydrogen ion when dissolved in water H+

Question 2

what are bases according to Arrhenius’s theory

Answer 2

substances that produce a hydroxide ion when dissolved in water OH

Question 3

acids based on bronsted lowry

Answer 3

molecules or ions that donate a proton (proton donors)

Question 4

bases based on bronsted lowry

Answer 4

molecules or ions that accept a proton (proton acceptors)

Question 5

what do conjugate pairs mean in terms of acids and bases?

Answer 5

an acid becomes a base by losing a proton, and a base becomes an acid by gaining a proton

Question 6

amphiprotic substances

Answer 6

a substance that acts as an acid with a base, and as a base with an acid. molecules that can donate or accept a proton

for example, water is amphiprotic because it can donate or accept a proton within an equation (more specifically, it can turn into H30+ or OH-)

HCO3−, H2PO4–, HSO4–

Question 7

electrolyte

Answer 7

a substance that conducts electricity when it forms ions

Question 8

the ion product constant of water

Answer 8

kw=[H3O+aq][OH-aq]=1.0 times 10^-14

hydronium ion times hydroxide ion equals ones times ten to the exponent negative fourteen

Question 9

when is a solution acidic?

Answer 9

when the hydronium concentration is larger than the hydroxide concentration

Question 10

when is a solution basic?

Answer 10

when the hydroxide concentration is larger than the hydronium concentration

Question 11

how do you find ph

Answer 11

ph concept was introduced by Danish chemist Soren Sorensen in 1909

pH refers to the acid

ph=-log [H3O+}
[H3O+]=10-ph
pH+pOH=14.00 –>pH=14-pOH

ph=-logarithm times the concentration of the hydronium ion

Question 12

how do you find pOH?

how do you find hydroxide?

Answer 12

pOH=-log[OH-]

[OH-]=10-pOH

find the pH then use the formula pH+pOH=14.00

Question 13

how do strong acids dissociate in water

Answer 13

they dissociate completely

Question 14

how do weak acids dissociate in water

Answer 14

they dissociate partially

Question 15

what are the trends of binary acids in terms of increasing

Answer 15

increases from left to right as electronegativity (ability to attract electrons) increases, and from top to bottom as the strength of the bond decreases (it can dissociate easily)

Question 16

how do you find the acid dissociation constant

Answer 16

convert to mols/L using c=n/V
plug into ICE table
Ka=[H3O+] [A]/[HA]

Question 17

how do you find percent dissociation

Answer 17

Acid percent dissociation=[H3O+][HAi] times 100

Base percen concentration=[OH-][Bi] times 100

Question 18

how do you find the equilibrium concentration of the ionization of a base

Answer 18

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

kw=(Ka) (Kb)

Question 19

what are the trends of oxyacids

Answer 19

the strength increases with the number of oxygen atoms found in the acid

HClO (aq), HClO2 (aq), HClO3 (aq). HClO4 the strength increases to the right

Question 20

what is salt?

Answer 20

an ionic compound produces as a result of a neutralization reaction of an acid and a base

Question 21

salt hydrolysis

Answer 21

when salt reacts with water to produce ions

Question 22

what makes a solution acidic during hydrolysis?

Answer 22

when there is a neutralization of a strong acid and a weak base
when the acid overpowers the base during the neutralization reaction

Hydro like water

Question 23

what makes a solution basic during hydrolysis?

Answer 23

when the base overpowers the acids when there is a strong base and a weak acid during the neutralization reaction

Question 24

what is a buffer solution?

Answer 24

made by mixing a usually a weak acid together with its conjugate base that is strong, and a weak base with its conjugate acid that is strong

a solution that resists change in pH, and its capacity is a pH of 7

Question 25

titration

Answer 25

quantitive analysis of neutralization reactions

mixing to make neutralization

is the slow addition of one solution of a known concentration called a titrant to another solution of unknown concentration called a tirand but a known volume until the reaction reaches neutralization, which is indicated by a change in colour

a technique in which one solution is used to analyze another solution

Question 26

indicator

Answer 26

weak acids that change colour as the concentration of hydronium ion changes

substances that give a visible sign, usually a change in colour with pH and suggest a chemical reaction has occurred

Question 27

endpoint

Answer 27

the physical change in colour when the reaction is complete

when the indicator changes colour

Question 28

equivalence point

Answer 28

point in a titration when enough titrant has been added to react with a substance in a solution that is being titrated, when the solution becomes neutral

Question 29

Describe what a strong acid strong base titration graph looks like?

Answer 29

graph line starts from the bottom, specifically, a pH of 1, then reaches an equivalence point/neutralization at 7, then goes up to a pH of 12

Question 30

describe the graph of a weak acid strong base titration

Answer 30

the graph starts at 3, and reaches equivalence at a pH of 8, above 7 meaning, the solution is basic, then goes up to pH at 12

Question 31

Describe weak base strong acid titration graph

Answer 31

the graphs start from the top at a pH of 13, then reach equivalence at a pH of 5, below 7 meaning, the solution is acidic, then goes down to a pH of 2

Question 32

quantitative analysis

Answer 32

a scientific approach where raw data is manipulated to give meaningful information

Question 33

what makes a solution basic?

Answer 33

with the pH is above 7 for example 8 and there is more hydroxide than hydronium

Question 34

what makes a solution acidic?

Answer 34

when the pH is below 7 for example 3 and the concentration of hydronium stronger than the concentration of hydroxide

Question 35

What is the difference between acids, bases, and amphiprotic substances in terms of their molecular formula?

Answer 35

for acids, the formula begins with H
for bases, the formula has an OH at the end
for amphiprotic substances the formula has H at the beginning, and O at the end with a negative