CHM 230 Exam 3 (copy)

the numerical value of K can be ()

manipulated

Q> K has too much () and goes to the ()

product, left

Q

reactant, right

Q=K is at ()

eqillibrium

the measure of the reactants and products at a given time is ()

Q

K is dependent on ()

temperature

between () and () is where equilibrium is

\+50, -50

acids are compound that () H+

donate

bases are compounds that () H+

accept

a way to represent the amount of free H+ is ()

pH

\-log(h30+) is the …

formula for pH

(H30+) =

10-pH

how many sig figs in pH

2

auto dissociation of water becomes what 2 products

H30, OH

what standard states are not accounted for in K

solid, liquid

Ka >1 is a () acid

strong

Ka

weak

for a strong acid () = ()

HA, H30

Name the 7 strong acids

HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4

Pka= ()

\-log(Ka)

14 = () + ()

pH, pOH

What is the Ka equation

Ka= (A-)(H30+)/(HA)

what is Ka

acid dissociation constant

what number does kw equal

\-1 x 10^-14

The ability to donate H+ is

Ka

As Ka increases so does ()

acid strength

What do you do to solve for pH when given M and ka of a solution?

ice table

when can we take away -x? The formula is (), it is () than 1000

(HA)/(Ka), greater

If the ratio of x to initial molarity is less than ()% the assumption ()

5, works

If the ratio of initial molarity to K is () than 1000 the assumption ()

greater, works

() effects are important

inductive

if the conjugate base is stable () is strong

acid

more oxygens equal more () because the () can spread over multiple sites

resonance, charge

M(OH) and M(OH)2 where M is an () or ()

alkali, alkaline earth metal

There are strong bases that completely () in solution

ionize

there are millions of () bases such as (), ()

weak, amines, anions

weak bases only () ionize in solution by ()

partially, hydrolysis

quantity of OH- is a function of ()

Kb

Kb is the ()

base dissociation constant

Kb is governed by hydrolysis ()

equlibrium

What is the equation to find Kb from Kw and Ka

Kw= Ka x Kb

species that do not change the pH of an aqueous solution are () ions

neutral

() act as bronsted-lowry acids in solution

cations

() act as bronsted-lowry bases in solution

anions

counterions () change pH

dont

examples of neutral counterions for strong acids (6) all anions

B,I,Cl,ClO4,NO3,ClO3

The strong base neutral counterion are also the ()

first column alkaline metals

() base impact pH by ()

weak, equillibrium

weak base equilibria act like () ()

weak acid, equilibria

Kb is the constant to determine

OH-

cations tend to be ()

acidic

anions tend to be ()

basic

A buffer is a solution that resists a () in pH this relates to ( ) lachatelier’s principle

change, self correcting

the equilibrium causes the solution system to shift to use up () H3O+ and OH- as long as HA and A- are ()

added, present

The added acetate ion on the right makes x smaller (assumption) is the () ion effect

common

If A- > HA then ….. the solution is ()

pH> pka, basic

If A- < HA then … the solution is ()

pH

If A- = HA then … the solution is ()

pH=pka, neutral

what is the henderson hasselbach equation used for

calculation for a buffer

what is the henderson hasselbach equation

pH= pka + log (A-/HA)

A- represents the

conjugate base concentration

HA represents the

acid concentration

() acids are capable of dissociating more than one H+

polyprotic

Dissociation of () depends on its concentration because of its dual strong/weak character

H2SO4

the study of how reactions happen is called

kinetics

what are the two factors that kinetics tell us

rates and mechanism of reaction

a reaction () diagram is a kinetic model

coordinate

reactions happen when particles collide with each other is a ()

model

reacting species should need to be () each other

near

collisions are ()

violent

bonds need to be ()/()

formed, broken

collisions impart a lot of () on colliding particles

energy

what are the three requirements that reacting models must have

collision, proper orientation, enough kinetic energy

transition state is where

bonds are formed and broken

insufficient KE to reach the transition state results in () reaction

no

a change in some measurable quantity per unit of time is

rate

what are the units of rate

M/s

High M means that a () of collisions will happen and create a () reaction

lot, faster

low M means much fewer () and a () reaction

collisions, slower

the rate is the () on the graph

slope

reaction () with time

slows

what is the equation of rate

y2-y1/x2-x1

rate of decomposition/consumption is ()

negative

rate of () is positive

production

the rate () for a given reaction relates rate of reaction to the () of reactants

law, reactants

the order of reactant are give by ()

exponents x,y

the overall order of reaction is given by the () of individual orders

sum

if the exponent is higher that means the reaction is more ()

complicated

the rate k is a () constant that encompansses all the parts of () theory that are not included under concentrations

numerical, collision

rate k is () dependent

temperature

the units of k are whatever is necessary to give () M/s in the rate law

rate units

what is unit of k if the overall order is zero

M/s

what is unit of k if the overall order is one

1/s

what is unit of k if the overall order is second

1/M x s

what is unit of k if the overall order is third

1/M2 x s

as order () you add an extra () to the denominator of k

increases, M

the actual of () rate is actually the () to the curve at any time, t

instantaneous, tangent

() rate laws allow us to calculate () quantities for a reaction in proces

integrated

for first order rate of reaction depends only on a () resulting species

single

what is half life

how long for the concentration initially to get 1/2