Gen Chem Flashcards
1
Q
Almost all oxidizing agents contain ______ or another strongly _________ element such as a ________
A
Oxygen; electronegative; halogen
2
Q
Reducing agents often contain ______ ions or _____
A
Metal; hydrides (H-)
3
Q
What are some common oxidizing agents?
A
O2 H2O2 Halogens (F2,Cl2, etc) H2SO4 HNO3 KMnO4 common in organic chem CrO3, NaCr2O7 common in organic chem PCC NAD+, FAD+ common in biochem
4
Q
What are some examples of common reducing agents?
A
CO C B2H6 NaBH4 LiAlH4 Hydrazine Pure metals Zn(Hg) NADH, FADH2
5
Q
Define atomic mass
A
Equal to the mass number, the sum of an elements protons and neutrons
6
Q
Isotopes have the same number of __________ but differ in the number of __________
A
Protons, but differ in the number of neutrons
7
Q
The quantum mechanical model posits what?
A
The quantum mechanical model posits that electrons do not travel in defined orbits but rather are localized in orbitals
8
Q
What is the Heisenberg uncertainty principle?
A
States that it is impossible to know both an electrons position and its momentum exactly at the same time
9
Q
What are the four quantum numbers and what do they describe in general
A
Principal quantum number (n)
Azimuthal quantum number (l)
Magnetic quantum number(ml)
Spin quantum number (ms)
These numbers completely describe any electron in an atom
10
Q
What does the principal quantum number (n) describe?
A
The average energy of a shell
11
Q
What does the azimuthal quantum number (l), describe?
A
Subshells within a given principal energy level (s,p,d, and f)
12
Q
For any principal quantum number n, there will be n possible values for l, ranging from _______ to ______
A
0 to (n-1)
13
Q
When l = 0 the sub shell is called ________
When l = 1 the sub shell is called ________
When l = 2 the sub shell is called ________
When l = 3 the subshell is called ________
A
s
p
d
f
14
Q
The maximum number of electrons within a subshell = ___________
A
4l + 2
15
Q
T/F: 4s subshell has a lower energy than the 3d subshell
A
True
16
Q
For any value of l, there will be __________ possible values for ml
A
2l + 1
17
Q
For any value of n, there will be a maximum of 2n squared electrons ________
A
Two per orbital
18
Q
What are the two possible values for ms (a quantum number telling spin)
A
+1/2 and -1/2
19
Q
Whenever two electrons are in the same orbital, they must have ______
A
Opposite spins
20
Q
n+1 rule can be used to rank subshells by increasing energy. What does this rule state?
A
That the lower the sum of the values of the first and second quantum numbers , n + l, the lower the energy of the subshell
21
Q
If two subshells possess the same n+l value, the subshell with the lower ______ value has lower energy and will fill with electrons ______
A
n value ; first
22
Q
What does hunts rule state?
A
Within a given subshell, orbitals are filled such that there are maximum amount of half filled orbitals with parallel spins before pairing up.
23
Q
Paramagnetic means what?
A
That a magnetic field will cause parallel spins in unpaired electrons and therefore cause an attraction
24
Q
What are valence electrons?
A
Electrons in the valence shell that are the farthest from the nucleus and have the greatest amount of potential energy
25
At the atomic level, a metal can be defined by
```
A low effective nuclear charge
Low electronegativity
Large atomic radius
Small ionic radius
Low ionization energy
Low electron affinity
```
26
Nonmetals are periodically defined as
```
High ionization energies
High electronegativities
High electron affinities
Small atomic radii
Large ionic radii
```
27
Metalloids are also called ______ because they share some of the characteristics with both metals and nonmetals
Semi metals
28
For elements in the same ______, Zeff(effective nuclear charge) increases from ________ to _______
Period; left ; right
29
As one moves down the elements of a given group, the principal quantum number ______________ each time
Increases by 1
30
How is the Zeff in a given group (family)?
It is more or less constant
31
What are the three key rules that control how valence electrons work in an atom?
As one moves from left to right across a periodic table, electrons and protons are added one at a time
As one moves down the elements of a given group, the principal quantum number increases by one each time
Elements also gain or lose electrons in order to achieve a stable octet formation representative of the noble gases.
32
What is the difference between the atomic radius and the ionic radius?
Atomic radius: refers to the size of a neutral element
Ionic radius: is dependent on how the element ionizes based on its element type and group number
33
_________ is essentially opposite that of all the other periodic trends. While others increase going up and to the right, this one does what?
Atomic radius increased going down and to the left
34
What is ionization potential (ionization energy)
The energy required to remove an electron from a gaseous species
35
The higher the Zeff or the closer the valence electrons are to the nucleus, the _________ the ionization energy is
Higher
36
What is electron affinity?
The energy dissipated by a gaseous species when it gains electrons
37
Electron affinity is an _________ process which means it has a _________ enthalpy (delta H rxn), how ever the electron affinity it reported as a positive number
Ionization energy is an _________ process which means it has a ________ enthalpy
Exothermic ; negative
Endothermic; positive
38
What are the periodic trends that increase from left to right?
Ionization energy
Electron affinity
Electronegativity
39
What are the period trends that decrease from left to right?
Atomic radius
40
What are the periodic trends that increase from top to bottom?
Atomic radius
41
What are the periodic trends that decrease from top to bottom
Ionization energy
Electron affinity
Electronegativity
42
What is the smallest, most electronegative, highest ionization energy, most exothermic (highest electron affinity) element of the periodic table?
Fluorine
43
What element of the periodic table is the largest, least electronegative, lowest ionization energy, and least exothermic (lowest electron affinity)
Cesium
44
What are the characteristics of alkali metals?
Typically take on the oxidation state of +1
Prefer to lose an electron to achieve the octet
Most reactive of all metals
45
C-C
| bond length and bond strength
Longest bond
Weakest bond
46
C=C
| Bond length and bond strength
Medium length
Medium strength
47
C-triple bond-C
Bond length and bond strength
Short length
Strongest bond
48
7 Naturally occurring diatomic elements
```
H2
N2
O2
F2
Cl2
Br2
I2
```
49
SF6 has what shape and what angle between electron pairs?
Shape: octahedral
Angle between electron pairs: 90, 180
50
PCl5 shape and angle between electron pairs
Shape: trigonal bipyramidal
Angle between electron pairs: 90, 120, 180
51
CH4 shape and angle between electron pairs
Tetrahedral
109.5
52
BH3 shape and angle between electron pairs
Trigonal planar
120
53
BeCl2 shape and angle between electron pairs
Linear
180
54
CH4, NH3, and H2O all have a tetrahedral electronic geometry but differ in their molecular shapes. What are their molecular shapes?
CH4: tetrahedral
NH3: Pyramidal
H2O: bent or angular
55
Hydrogen bonds exist in molecules containing a H bonded to _______, _______, or ________
Fluorine, Oxygen, Nitrogen
56
When the change in electronegativity is less than .5 some bonds can be considered _________
Nonpolar
57
What is a combination reaction?
Has two or more reactants forming a product
A+B----> C
58
What is a decomposition reaction?
A single reactant breaks down into two or more products usually as a result of heating, high-frequency, radiation, or electrolysis
A-----> B+C
59
What is a combustion reaction? What does it involve? And what are the typical products
Involves a fuel (usually a hydrocarbon) and an oxidant (normally oxygen)
CO2 and H2O
60
What is a single displacement reaction? What are they often further classified by?
Occur when an atom or ion in a compound is replaced by an atom or ion of another element
Often further classified as oxidation-reduction reactions
61
What type of double displacement reaction in which an acid reacts with a base to produce a salt (and usually water
Neutralization reaction
62
Stoichiometry, an application of dimensional analysis is often simplified to a series of 3 fractions. These fractions demonstrate an underlying three step process. What is that process?
1) convert from the given units to moles
2) use the mole ratio
3) convert from moles to the desired units
63
Common conversions of stoichiometry include:
1 mole of any ideal gas at STP= _______
1 mole of any substance =___________ (avagadro's number)
1 mole of any substance = ____________ (from the periodic table)
22. 4 L
6. 22x10 23
Its molar mass
64
What is the limiting reagent?
It limits the amount of product that can be formed in the reaction
It is the reactant that is used up or consumed first
65
When determining the limiting reagent, keep in mind what two principles?
1) all comparisons of reactants must be done in units of moles.
2) the rate at which the reactants are consumed, combined with the absolute mole quantities determines which reactant is the limiting reagent
66
The yield of a reaction can refer to what 2 things?
1) the amount of product predicted (theoretical yield)
2) the amount of product actually obtained (raw or actual yield)
When a reaction is carried out
67
What is the theoretical yield?
The maximum amount of product that can be generated as predicted from the balanced equation assuming that:
All of the limiting reactant is consumed
No side reactions have occurred
And the entire product has been collected
**** it is rarely ever attained through the actual chemical reaction
68
What is the actual yield?
The amount of product one actually obtains during the reaction
69
How is the percent yield determined?
The ratio of the actual yield to the theoretical yield times 100 percent
70
Ionic compounds are held together by ionic bonds, which rely on what?
The force of electrostatic attraction between oppositely charged particles
71
Monatomic anions are named by dropping the ending of the name element and adding _____.
Some examples are H-, F-, O2-, S2-, N3-
-ide
Hydride, Fluoride, oxide, sulfide, nitride
72
Many polyatomic ions contain oxygen and are therefore called ________. When an element forms two of these, the name of the one with less oxygen ends in______ and the one with more oxygen ends in ______
Ex: NO2-, NO3-, SO3-2, SO4-2
Oxyanions
-ite
Nitrite, sulfite
-ate
Nitrate, sulfate
73
Hypo- and per- are used to indicate what?
Ex: ClO-, ClO2-, ClO3-, ClO4-
Less oxygen and more oxygen
| Hypochlorite, Chlorite, Chlorate, Perchlorate
74
What polyatomic ions have a positive 1 charge?
Ammonium
75
What polyatomic ions have a -1 charge?
Acetate C2H3O2
Cyanide CN-
Permanganate MnO4-
Thiocyanate SCN-
76
What polyatomic ions have a -2 charge?
Chromate CrO4-2
Dichromate Cr2O7 -2
77
What polyatomic ions have a -3 charge?
Borate BO3-3
78
What are the active metals (groups from periodic table) that have charges of +1 and +2 in their natural state?
The alkali metals (group 1 or group IA)
The alkaline earth metals (group 2 or group IIA)
79
Alkali metals are not typically found in nature in their uncharged state because ________
Instead they are found as cations in __________
They are highly reactive with moisture.
Salts (like NaCl)
80
What compounds make good electrolytes and what makes them good electrolytes?
Ionic compounds
Because they dissolve most readily
81
What compound are the weakest electrolytes? And why?
Nonpolar covalent compounds because they do not form current-carrying ions.
82
What determines whether or not a reaction is spontaneous or non spontaneous?
Gibbs free energy (delta G)
83
The rate of the whole reaction is only as fast as the ______
Rate-determining step
84
What is the activation energy?
The minimum energy of collision necessary for a rxn to take place
85
_____ activation energy and ______ temperatures make the negative component of the arrhenius equation smaller in magnitude and thus increase the rate constant k
Low; high
86
What are the factors that affect reaction rate?
Reaction concentrations
Temperature
Medium
Catalysts
87
How does the reaction concentrations affect the reaction rate?
The greater the concentrations of the reactants, the greater the number of effective collisions per unit time, which increases the reaction rate for all but zero-order reactions
88
Catalysts only change what in a rxn?
The activation energy
89
What are the only factors that can change the rate of a zero-order reaction
Temperature and the addition of a catalyst
90
In a zero-order reaction, the rate of formation of product is _________ of the concentration of reactant. And the rate of reaction (k) is _______
Independent
Opposite of the slope
91
What is a first order reaction? The rate of formation of product is dependent on ______________
Has a rate that is directly proportional to only one reactant
The concentration of reactant
Ln[A] vs time: k= -slope
92
What is a second order reaction?
Has a rate that is proportional to either the concentrations of two reactants or the square of the concentrations of a single reactant
1/[A] vs time graph: the k= slope
93
At equillibrium , the rate of the forward rxn equals the rate of the reverse rxn, entropy is at a _______, and Gibbs free energy is at a ________.
Maximum; Minimum
94
The law of mass action states what?
That if the system is at equillibrium at a constant temperature then the ratio of
Keq =products / reactants with moles as exponent of each
95
In equillibrium the exponents are equal to the ______________
Coefficients in the balanced equation
96
In rate laws the exponents must be determined __________________
experimentally and often do not equal the stoichiometric coefficients
97
What is the definition of an Arrhenius acid?
Will dissociate to form an excess of H+ in solution
98
What is the definition of an Arrhenius base?
Will dissociate to form an excess of OH- in solution
99
What is the definition of a Brønsted-Lowry acid?
A species that donates hydrogen ions
100
What is the definition of a Brønsted-Lowry base?
A species that accepts them
101
Arrhenius definition of acids and bases is limited to what?
Aqueous solutions
102
With the Bronsted-Lowry definition of an acid or base, is water an acid or a base?
An acid bc it is able to donate a proton to other species
103
What is the Lewis definition of an acid?
Lewis acids are electron pair acceptors
104
What is the definition of a Lewis base?
An electron pair donor
105
Lewis acid-base chemistry appears in many names and its when one species pushes a lone pair to form a bond with another, what are the names of this type of chemistry?
Coordinate covalent bond formation
Complex ion formation
Nucleophile-electrophile interactions
106
What is the definition of an amphoteric species?
One that reacts like an acid in a basic environment and like a base in an acidic environment
107
In the bronsted Lowry sense, amphoteric species can__________________
Either gain or lose a proton, making it amphiprotic
108
What is the most common example of an amphiprotic species
Water.
When water reacts with a base, it behaves as an acid
When water reacts with an acid, it behaves as a base
Other examples are H2SO4 and hydroxides that contain Al, Zn, Pb and Cr. And amino acids
109
What is a proper way of estimating p values on test day?
P value= m - 0.n
With n being the exponent (ex 10^6- so n would be 6)
m being the number in front (ex: 1.66X10^-6) 1.66 would be m
110
What is the difference between weak acids or bases and strong acids or bases?
Strong acids and bases tend to dissociate completely in aqueous solution.
Weak acids and bases only dissociate partially in aqueous solution
111
The smaller the Ka, _______ the acid and the _______ it will dissociate
Weaker ; less
112
The smaller the Kb the _______ the base and the _______ it will dissociate
Weaker ; less
113
A species is characterized as a weak acid if its Ka is _________ than 1 and a weak base if its Kb is _________ than 1. Molecular (nonionic weak bases are ____________
Almost exclusively amines
114
When is a conjugate acid formed? And when is a conjugate base formed?
When a base gains a proton
The base formed when an acid loses a proton
**** based on the bronsted-Lowry definition of acid base reactions
115
Ka and Kb are ________ related. If Ka is large, then Kb is ________.
Inversely
Small and vice versa
116
When acids and bases react with each other to form a salt and often water what type of reaction is it?
A neutralization reaction
117
What is the ground state of an atom?
The state of lowest energy, when all of the electrons are in the lowest possible ortbials
118
What is an excited state?
When at least one electron has moved to ta subshell of higher than normal energy
119
How can electromagnetic energy of photons be determined?
By multiplying planks constant with the speed of light and then dividing that by the wavelength
120
What is a molecule?
A combination of two or more atoms held together by covalent bonds
121
What is the basis of equivalents?
How many moles are we interested in?
122
What does the gram equivalent weight represent in acid-base chemistry?
The mass of acid that yields one mole of OH ions
123
What does the empirical formula give?
The simplest whole number ratio of elements in the compound
124
When do isothermal processes occur? And what is temperatures relation to internal energy?
When the systems temperture is constant.
Constant temperature implies the total internal energy of the system is constant throughout the process
Temperature and internal energy are directly proportional
125
When does Adiabatic processes occur? How does it appear on a P-V curve?
When no heat is exchanged between the system and the environment
The internal energy of the system is constant throughout the process.
The change in internal energy of the system is equal to work done on the system.
Appears hyperbolic on a P-V graph
126
When do isobaric processes occur? How do they change the first law? How do they appear on a P-V graph?
When the pressure of the system is constant
They do not alter the first law
As a flat line
127
When do isovolumetric (isochoric) processes occur? How does it affect the first law? How is it represented on a P-V graph/?
Experience no change in volume because the gas neither expands no compresses, no work is performed in this process/
The first law is simplified to the change in internal energy is equal to the heat added to the system
As a vertical line on the P-V graph
128
What does a state function describe? What can they not do?
The system in an equilibrium state
They cannot describe the process of the system (how the system got to its current equilibrium
129
The pathway taken from one equilibrium state to another is described by process functions. What are the most importna t process functions?
Work (W) and Heat (Q)
130
What are examples of state functions? What happens to these when a system changes from equilibrium
Pressure, density, temperature, volume, enthalpy, internal energy, Gibbs free energy, and entropy
When a state of a system changes from equilibrium, one or more of these states will change
131
What is the ideal gas law? And what does it show a relationship of?
PV=nRT
R being the ideal gas constant of 8.21x10^-2 Lxatm/mol.K or 8.314 J/Kxmol
The relationship amoung four variable that define a sample of gas
132
How would one calculate the density of any gas?
p=m/V=PM/RT
133
Pressure is ______ to volume
Pressure is ______ to number of moles
Pressure is _____ to temperature
Volume is _____ to temperature
Inverse
Proportional
Proportional
Inverse (unless n and P are constant)
134
When temperature what is the ideal gas equation?
P1xV1=P2xV2
135
What is the ideal gas equation when moles are constant?
P1xV1/T1=P2xV2/T2
136
What are solutions?
Homogenous (the same throughout) mixtures of two or more substances that combine to form a single phase, usually the liquid phase
137
What does a solution consist of?
A solute dissolved in a solvent.
A solute such as NaCl, NH3, C6H12O2
A Solvent is something like H20 benzene or ethanol
138
What is the definition of a solvent?
The component of the solution that remains in the same phase after mixing.
139
What is solvation ?
The electrostatic interaction between solute and solvent molecules
AKA a dissolution c
140
When the new interactions are stronger than the original ones, solvation is ________ and the process is favored at _________ temperatures.
Exothermic
Low
141
The dissolution of gases into liquids such as ________________ is an ___________ process
CO2 into water.
Exothermic s
142
At constant temperature and pressure, entropy always _________ upon dissolution
Increases
143
Whether or not dissolution will happen spontaneously depends on what?
Both the change in enthalpy and the change in entropy for both the solute and the solvent of the system
144
When the change in Gibbs free energy for the dissolution reaction is neg at a given temperature, the process will be spontaneous and the solute is said to be ________
Soluble
145
When the change in Gibbs free energy is postive, the dissolution reaction. Will be nonspontaneous , and the solute is said to be ____________
Insoluble
146
Solute are soluble if they have a molar solubility _________ .1M in solution. Those solute that dissolve minimally in the solvent have a molar solubility _______ .1M and are called _______
Above
Under
Sparingly soluble salts
147
What do aqueous reactions rely on?
The interactions between water molecules and solutes in solutions
148
What are the two absolute solubility rules?
All salts of group 1 metals and all nitrate salts are soluble
149
What are coordinate covalent bonds?
An electron donor (Lewis base) and an electron acceptor (Lewis acid) form very stable Lewis acid-base adducts.
Ex: proteins utilize this complex ion binding and transition metal complexes to carry out their functions
150
What does the presence of transition metal allows coenzymes and co factors to do?
Bind other ligands or assist with electron transfer
151
What is percent composition by mass?
Mass of solute divided by mass of solution times 100%
152
What is mole fraction used to calculate and what is the sum of the mole fractions in a system always equal to?
Used to calculate the vapor pressure depression of a solution
The sum of the mole fraction in a system will always equal 1
153
What is the molarity of a solution defined as?
Moles of solute divided by liters of solution
154
What is molality of a solution defined as?
Moles of solute divided by kilograms of solvent
155
What is normality? What is an equivalent?
The normality of a solution is equal to the number of equivalents of interest per liter of solution.
An equivalent is equal to a mole of the species of interest. (Protons, OH ions, electrons, or ions)
An equivalent is a measure of the reactive capacity of a molecules
156
When is a solution considered diluted? How is the concentration then determined?
When solvent is added to a solution of higher concentration to produce a solution of lower concentration
After dilution the concentration can be determined by molarity times volume (initial) = molarity time volume (final)
157
What is the saturation point?
Where the solute concentration is at its maximum value for a given temperature and pressure
158
What is dynamic equillibrium?
The rates of dissolution and precipitation are equal and the concentration of dissolved solute reaches a steady-state (constant) value
159
Pure _______ and __________ do not appear in the equillibrium constant
Solids and liquids
160
Solubility product constants like all other equillibrium constants are all _________. When the solution consists of a gas dissolved into a liquid the value of the equillibrium constant will also depend on _________
Temperature dependent
Pressure
161
How does the solubility product constant differ between non gas solutes and gas solutes when temperature increases?
The solubility product constant increases with increasing temperature for non gas solutes and decreases for gas solutes
162
How does ion product indicate that the solution is not yet at equillibrium, and is considered unsaturated? Is dissolution or precipitation more thermodynamically favorable at this time?
When a salt's IP is less than the Salts' Ksp
Dissolution is thermodynamic favorable
163
When is the solution considered supersaturated? How is a supersaturated solution created?
When the Ion product is greater than Ksp then the solution is considered super saturated
By dissolving solute into a hot solvent and then slowly cooling the solution
Precipitation is more thermodynamically favorable
164
When is the solution considered saturated?
If the calculate IP is equal to the known Ksp
The solution is in equillibrium
165
What is molar solubility?
The molarity of a solute in a saturated solution
166
The dissolution of the of the original solution is termed _____ and the subsequent formation of the complex ion in solution is termed _______
Ksp
Kf (the formation or stability constant of the complex in solution)
167
What is the rate limiting step for complex ion formation?
The initial dissolution of the metal ion
168
Why do complex ions form?
To become more soluble in solution
169
What are colligative properties?
Physical properties of solutions that are dependent not he concentration of dissolved particles but not on the chemical identity of the dissolved particles
Ex: vapor pressure depression, freezing point depression, boiling point elevation, and osmotic pressure are usually associated with dilute solutions
170
What is the common ion effect? What effect does it have on the dissociation reaction??
It decreases the solubility of a compound in a solution that already contains one of the ions in the compound.
The presence of that ion in solution shifts the dissociation reaction to the left decreasing its dissociation
171
What are pH and pOH of a solution given by?
pH= -log[H+] = log 1/[H+}
pOH= -log[OH-] = log 1/[OH-]
172
What is the relationship of pH and pOH
As pH increases, pOH decreases by the same amount
An inverse relationship
173
What does a pH greater than 7 or a pOH less than 7 indicate?
What does a pH less than 7 or a pOH greater than 7 indicate?
Indicates a relative excess of OH ions and the solution is basic
Indicates a relative excess of H+ ions and the solution is acidic
174
pH is 7 is neutral is applicable only if the temperature is _________
25 degrees Celsius or 298K
175
What is an acid equivalent? A base equivalent? And what is polyvalent?
Acid equivalent: equal to one mole of H+ (or H30+) ions
Base equivalent: equal to one mole of OH-
Some acids and bases are polyvalent so each mole of the acid or base liberates more than one acid or base equivalent
176
One mole of H2SO4 produces how many acid equivalents?
Two (2moles of H3O+)
177
What two measurements are useful for acid-base chemistry?
Normality and gram equivalent weight
178
What is gram equivalent weight? What is the gram equivalent weight of H2SO4?
The mass of a compound that produces one equivalent (one mole of charge)
H2SO4 has a molar mass of 98 g/mol. It Is a divlaent acid so each mole of the acid compound yields two acid equivalents. The gram equivalent weight is 98/2 = 49 grams.
The complete dissociation of 49 grams of H2SO4 will yield one acid equivalent (1 mole of H3O+)
179
What are the common polyvalent acids? Common polyvalent bases?
Common polyvalent acids: H2SO4, H3PO4 and H2CO3
Common polyvalent bases: Al(OH)3, Ca(OH)2, Mg(oH)2
180
How do indicators work in titrations to determine the equivalence point of the acid-base titration ?
Indicators are weak organic acids or bases that have different colors in their protonated state and deprotonated states. They need to be weak or else the indicator would be titration first
The point at which the indicator changes to its final color is NOT the equivalence point but rather the ENDPOINT
181
When a strong acid and a strong base are titration the equivalence point of the titration will be what?
7 (for monovalent species)
182
What is the equivalence point of a weak acid and strong base titration such as CH3COOH with NaOH.
A pH greater than 7
183
What is the difference in titration curves for a strong acid with a strong base compared to a weak acid with a strong base?
The PH curve for the strong acid/strong base titration shows a steeper, more sudden rise ath the equivalence point.
In the weak acid/ strong base titration the pH changes more gradually early on in the titration and has less of a sudden rise at the equivalence point
184
What does the pH titration curve look like for a weak base titrand and strong acid titrant ?
An inversion of the curve for a weak acid titrand and a strong base titrant
The intial pH will be in the basic range and will demonstrate a gradual drop in pH with the addition of a strong acid
The equivalence point wil be in the acidic pH range
185
With polyvalent acids and bases, when is the equivalence point recognized?
There are multiple equivalence points as the H+ ions are removed, a rapid pH change is observed near the equivalence point (the point between regions 4 and 5) as acid is added
