What is the pH of a solution after the addition of 30.0 mL of 0.100 M NaOH to 50.0 mL of 0.10 M HBr?
1 answer:
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Answer: The pH at equivalence point for the given solution is 5.59.
Explanation:
At the equivalence point,
So, first we will calculate the moles of as follows.
= 0.0845 mol
Now, volume of present will be calculated as follows.
Volume =
=
= 0.1891 L
Therefore, the total volume will be the sum of the given volumes as follows.
110 ml + 189.1 ml
= 299.13 ml
or, = 0.2991 L
Now,
= 0.283 M
Chemical equation for this reaction is as follows.
As,
=
=
Now,
=
=
Now, pH will be calculated as follows.
pH =
=
= 5.59
Thus, we can conclude that pH at equivalence point for the given solution is 5.59.
Answer:
"1 M" will be the right solution.
Explanation:
The given values are:
Number of moles,
= 2 moles
Volume of solution,
= 2000 mL
or,
= 2 L
Now,
The molarity of the solution will be:
=
On substituting the values, we get
=
=