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Ionization of Weak Bases Video Lecture | Physical Chemistry for NEET
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FAQs on Ionization of Weak Bases Video Lecture - Physical Chemistry for NEET
| 1. What is ionization of weak bases? |  |
Ans. Ionization of weak bases refers to the process in which a weak base, such as ammonia or water, accepts a proton (H+) from a strong acid, resulting in the formation of a conjugate acid and a hydroxide ion (OH-). This process occurs to a lesser extent compared to strong bases and is characterized by an incomplete dissociation in water.
| 2. How does the ionization of weak bases differ from strong bases? | |
Ans. The ionization of weak bases differs from strong bases in terms of the extent of dissociation. While strong bases completely dissociate in water, weak bases only partially dissociate, resulting in a lower concentration of hydroxide ions (OH-) in the solution. This lower concentration of hydroxide ions makes weak bases less alkaline compared to strong bases.
| 3. What factors influence the degree of ionization of weak bases? | |
Ans. Several factors influence the degree of ionization of weak bases. These factors include the concentration of the weak base, temperature, presence of other ions or molecules in the solution, and the nature of the weak base itself. Higher concentrations, higher temperatures, and absence of competing ions or molecules generally favor a higher degree of ionization.
| 4. Can you provide an example of a weak base and its ionization equation? | |
Ans. Ammonia (NH3) is an example of a weak base. Its ionization equation in water can be represented as follows:
NH3 + H2O ⇌ NH4+ + OH-
In this equation, ammonia accepts a proton from water to form the ammonium ion (NH4+) and hydroxide ion (OH-). The equilibrium symbol (⇌) indicates that the reaction is reversible, and the degree of ionization depends on the relative concentrations of the reactants and products.
| 5. How does the ionization of weak bases affect their pH? | |
Ans. The ionization of weak bases results in the formation of hydroxide ions (OH-), which can increase the concentration of hydroxide ions in the solution. This increased concentration of hydroxide ions leads to an increase in pH, making the solution more basic. However, since weak bases only partially ionize, the increase in pH is generally less pronounced compared to strong bases.
Text Transcript from Video
welcome to electron line and now let's
take a look at weak bases and their
associated ionization constants so just
like with acids a strong base completely
ionizes in water so when we have for
example sodium hydroxide we put that in
an aqueous solution we find out that you
completely ionizes into sodium ions and
hydroxide ions one hundred percent or
very nearly so but weak bases only
partially ionized for example when we
take ammonia which is a weak base and we
dissolve it in water we have a partial
ionization process where some of it
turns into the ammonium ion and some but
then with associated hydroxide ion as
well and we have an OOP this is wrong
here this should be k so be the count
the ionization constant for basis can
then be defined by the concentration of
the hydroxide ion times the
concentration of the associated or
conjugate acid / the final concentration
of the base then if we want to find the
pH of the solution we can find the Poh
of the solution by taking minus the log
of the final concentration of the
hydroxide ion which comes from right
here final concentration then we can
find the pH by taking 14 minus the Poh
and if you want to find the percent
ionization we take the concentration of
the hydroxide ion divided by the council
should the initial concentration of the
base times a hundred percent so looks
very similar than what we do with assets
except the only difference here is that
we have the Associated ionization
constant for the base and then of course
we can calculate the Poh which then we
have to find the pH doing this small
step right there but other than that
it's the very same process on the next
video will show you an example of how to
find the final concentration and the
percentile is a shin of a weak base
take a look at weak bases and their
associated ionization constants so just
like with acids a strong base completely
ionizes in water so when we have for
example sodium hydroxide we put that in
an aqueous solution we find out that you
completely ionizes into sodium ions and
hydroxide ions one hundred percent or
very nearly so but weak bases only
partially ionized for example when we
take ammonia which is a weak base and we
dissolve it in water we have a partial
ionization process where some of it
turns into the ammonium ion and some but
then with associated hydroxide ion as
well and we have an OOP this is wrong
here this should be k so be the count
the ionization constant for basis can
then be defined by the concentration of
the hydroxide ion times the
concentration of the associated or
conjugate acid / the final concentration
of the base then if we want to find the
pH of the solution we can find the Poh
of the solution by taking minus the log
of the final concentration of the
hydroxide ion which comes from right
here final concentration then we can
find the pH by taking 14 minus the Poh
and if you want to find the percent
ionization we take the concentration of
the hydroxide ion divided by the council
should the initial concentration of the
base times a hundred percent so looks
very similar than what we do with assets
except the only difference here is that
we have the Associated ionization
constant for the base and then of course
we can calculate the Poh which then we
have to find the pH doing this small
step right there but other than that
it's the very same process on the next
video will show you an example of how to
find the final concentration and the
percentile is a shin of a weak base
About this Video
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Dec 26, 2024 Last updated |
Video Description: Ionization of Weak Bases for NEET 2024 is part of Physical Chemistry for NEET preparation.
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