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32 Cards in this Set

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This law describes the state of equilibrium
Law of mass action
at equilibrium,the ratio of the rate of the forward reaction to the reverse ration equals to this
Log 10 or 1
equilibrium constants is expressed in this unit
no unit
If two reactions are at equilibrium with each other, then the equilibrium constants of the forward reaction (K) and the of the reverse reaction (K') have the following relationship
KK' = 1
In a chemical reactor, this reaction has not yet reached equilibrium- the reactants are still being converted into the products. Here, this relationship holds for the reation quotient (Q) and equilibrium constant (K)
Q<K
in Haber process, ammonia is synthesized from nitrogen and hydrogen. the application of higher pressure to this system will shift the position of the equilibrium in the following manner
To the right
photosynthesis is an example of an endothermic chemical reaction. in this process, plants use the energy form the sun to convert carbon dioxide and water into glucose and oxygen. this reaction requires 15 MJ of energy (sunlight) for every kg of glucose that is produces. increase the temperature of the system will shift the position of equilibrium in the direction of
to the right
when pH of a dilute solution increases from 3 to 5, its molar hydrogen ion concentration undergoes this change
100 fold decrease
which of the following acid is not a strong acid:
HF HBr HI
HF
in acetate buffer, the buffer action is provided by acetate ions and this chemical species
acetic acid
the pH of a buffer is dependent on many factors.
- temperature
- ionic strength
- concentrations of the acid and base
The pH of a monoprotic weak acid becomes equal to its pKa, when the ratio of the concentrations of its dissociated and undissociated forms satisfies this relationship
r = 1
When AgNO3, is used to titrate unknown concentration of KBr, what is the relationship between the concentration of Ag+ and that of Br- in the solution at equivalent point
the [Ag+] at equivalent point is independent on the initial [Br-]
This base can serve as a secondary standard for the titration of a weak acid
NaOH
In a titration experiment, as solution of arsenous acid (H3AsO3) was titration with iodine. In this process arenous acid was converted in to arsenic acid (H3As3O4). this is an example of this type of titration
Redox reaction
In a titration experiment, a compound with a physical property that changes abruptly when the titration is close to completion is known as this
Indicator
A titration experiment is assumed to have reached this point when the quantity of titrant added is the exact amount necessary for stoichometric reaction with the target analyte.
equivalence point
An anlytical experiment in which the titration procedure is carried out with the matrix that does not contain the target analyte is called this
blank titration
a highly pure and stable chemical reagent which can be weighed out and used directly to provide a known number of moles is called
primary standard
this base represents a primary standard for the titration of an acid
Na2CO3
A graduated tube used in a titration experiment to dispense known volume of a titrant is known as this
buret
when a weak acid is titrated with a strong base, the titration curve contains this many inflection points
2
what factors is the pH of a buffer dependent on
- temperature
- ionic strength
- relative concentrations of conjugated acid and base
This acid represents a secondary standard for the titration of a weak base
HCl
If the equilibrium constant for one reaction is K, the equilibrium constant K' of the new react if it is doubled will have following relationship
K' = K^2
when pH is a dilute solution increases from 10-11 its molar hydroxide ion concentration undergoes this change
10 fold increase.
In a buffer, the buffer action is provided by H2PO4- and this chemical species
H3PO4 and/or HPO4^2-
Glucose in a sample was reacted with glucose oxidase and then hydrogen peroxide was titrated with permangante. what type of titration is this
Indirect titration because it requires 2 steps
In the dissociation of a monohydroxy weak base B in aqueous solution which assumption leads to the statement of [OH-] =[BH+]
The condtribution of [OH-] from water autoprotolysis can be ignored
The first derivative of titration curve indicates
The position of equivalence point, where the first derivative reaches maximum.
Increase of volume of this system wills hift the position of equilibrium in the following manner
to the left
which addition will increase the solubility of MgF2 in water
add HNO3