A compound with molecular formula C6H15N exhibits a singlet at d 0.9 (1H), a triplet at d 1.10 (3H), a singlet at d1.15 (9H), an
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Answer:
pH = 3.513
Explanation:
Hello there!
In this case, since this titration is carried out via the following neutralization reaction:
We can see the 1:1 mole ratio of the acid to the base and also to the resulting acidic salt as it comes from the strong HCl and the weak hydroxylamine. Thus, we first compute the required volume of HCl as shown below:
Now, we can see that the moles of acid, base and acidic salt are all:
And therefore the concentration of the salt at the equivalence point is:
Next, for the calculation of the pH, we need to write the ionization of the weak part of the salt as it is able to form some hydroxylamine as it is the weak base:
Whereas the equilibrium expression is:
Whereas Ka is computed by considering Kw and Kb of hydroxylamine:
So we can write:
And neglect the x on bottom to obtain:
And since x=[H3O+] we obtain the following pH:
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Answer : The value of of the reaction is 10.5 and the reaction is product favored.
Explanation : Given,
Moles of at equilibrium = 0.0406 mole
Moles of at equilibrium = 0.170 mole
Moles of at equilibrium = 0.302 mole
Volume of solution = 2.00 L
First we have to calculate the concentration of at equilibrium.
Now we have to calculate the value of equilibrium constant.
The balanced equilibrium reaction is,
The expression of equilibrium constant for the reaction will be:
Now put all the values in this expression, we get :
Therefore, the value of of the reaction is, 10.5
There are 3 conditions:
When ; the reaction is product favored.
When ; the reaction is reactant favored.
When ; the reaction is in equilibrium.
As the value of . So, the reaction is product favored.