How many grams of dry NHạ Cl need to be added to 2.00 L of a 0.100 M solution of ammonia, NHa, to prepare a buffer solution that has a pH of 8.98? K for ammonia is 1.8 x 10 Express your answer with the appropriate units.
Reactive Intermediates
In chemistry, reactive intermediates are termed as short-lived, highly reactive atoms with high energy. They rapidly transform into stable particles during a chemical reaction. In specific cases, by means of matrix isolation and at low-temperature reactive intermediates can be isolated.
Hydride Shift
A hydride shift is a rearrangement of a hydrogen atom in a carbocation that occurs to make the molecule more stable. In organic chemistry, rearrangement of the carbocation is very easily seen. This rearrangement can be because of the movement of a carbocation to attain stability in the compound. Such structural reorganization movement is called a shift within molecules. After the shifting of carbocation over the different carbon then they form structural isomers of the previous existing molecule.
Vinylic Carbocation
A carbocation where the positive charge is on the alkene carbon is known as the vinyl carbocation or vinyl cation. The empirical formula for vinyl cation is C2H3+. In the vinyl carbocation, the positive charge is on the carbon atom with the double bond therefore it is sp hybridized. It is known to be a part of various reactions, for example, electrophilic addition of alkynes and solvolysis as well. It plays the role of a reactive intermediate in these reactions.
Cycloheptatrienyl Cation
It is an aromatic carbocation having a general formula, [C7 H7]+. It is also known as the aromatic tropylium ion. Its name is derived from the molecule tropine, which is a seven membered carbon atom ring. Cycloheptatriene or tropylidene was first synthesized from tropine.
Stability of Vinyl Carbocation
Carbocations are positively charged carbon atoms. It is also known as a carbonium ion.
![V.E. CHEM 02 Spring 2021
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<Ch 18 Part 1 Buffers, Titrations, Solubility
Question 4
Just as pH is the negative logarithm of
H,O+1. pK, is the negative logarithm of
K..
- Part A
pK =-log K,
Acetic acid has a K, of 1.8 x 10-5. Three acetic acid/acetate buffer solutions, A B, and C, were made using varying concentrations:
The Henderson-Hasselbalch equation is used to
calculate the pH of buffer solutions:
A [acetic acid] ten times greater than (acetate).
B. acetate ten times greater than [acetic acid), and
c. Jacetate = [acetic acid].
base)
pH = pK, +log
scid)
Match each buffer to the expected pH.
Notice that the pH of a buffer has a value
close to the pK, of the acid, differing only by
the logarithm of the concentration ratio
(basel/lacád). The Henderson-Hasselbalch
equation in tems of pOH and pK is similar.
Drag the appropriate items to their respective bins.
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POH = pK +log
%3D
base)
pH = 3.74
pH= 4.74
PH = 5.74
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