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32 Cards in this Set
- Front
- Back
This law describes the state of equilibrium
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Law of mass action
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at equilibrium,the ratio of the rate of the forward reaction to the reverse ration equals to this
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Log 10 or 1
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equilibrium constants is expressed in this unit
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no unit
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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
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KK' = 1
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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)
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Q<K
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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
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To the right
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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
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to the right
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when pH of a dilute solution increases from 3 to 5, its molar hydrogen ion concentration undergoes this change
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100 fold decrease
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which of the following acid is not a strong acid:
HF HBr HI |
HF
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in acetate buffer, the buffer action is provided by acetate ions and this chemical species
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acetic acid
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the pH of a buffer is dependent on many factors.
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- temperature
- ionic strength - concentrations of the acid and base |
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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
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r = 1
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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
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the [Ag+] at equivalent point is independent on the initial [Br-]
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This base can serve as a secondary standard for the titration of a weak acid
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NaOH
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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
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Redox reaction
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In a titration experiment, a compound with a physical property that changes abruptly when the titration is close to completion is known as this
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Indicator
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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.
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equivalence point
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An anlytical experiment in which the titration procedure is carried out with the matrix that does not contain the target analyte is called this
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blank titration
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a highly pure and stable chemical reagent which can be weighed out and used directly to provide a known number of moles is called
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primary standard
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this base represents a primary standard for the titration of an acid
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Na2CO3
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A graduated tube used in a titration experiment to dispense known volume of a titrant is known as this
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buret
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when a weak acid is titrated with a strong base, the titration curve contains this many inflection points
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2
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what factors is the pH of a buffer dependent on
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- temperature
- ionic strength - relative concentrations of conjugated acid and base |
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This acid represents a secondary standard for the titration of a weak base
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HCl
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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
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K' = K^2
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when pH is a dilute solution increases from 10-11 its molar hydroxide ion concentration undergoes this change
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10 fold increase.
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In a buffer, the buffer action is provided by H2PO4- and this chemical species
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H3PO4 and/or HPO4^2-
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Glucose in a sample was reacted with glucose oxidase and then hydrogen peroxide was titrated with permangante. what type of titration is this
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Indirect titration because it requires 2 steps
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In the dissociation of a monohydroxy weak base B in aqueous solution which assumption leads to the statement of [OH-] =[BH+]
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The condtribution of [OH-] from water autoprotolysis can be ignored
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The first derivative of titration curve indicates
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The position of equivalence point, where the first derivative reaches maximum.
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Increase of volume of this system wills hift the position of equilibrium in the following manner
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to the left
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which addition will increase the solubility of MgF2 in water
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add HNO3
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