What is the pH of a solution that has a hydronium ion concentration 100 times less than a solution with a pH of 6 explain your r
1 answer:
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Explanation:
It is given that the total volume is (10 mL + 60 mL) = 70 mL.
Also, it is known that =
Where, = total volume
= initial volume
Therefore, new concentration of =
=
= 0.43 M
New concentration of NaOH =
=
= 0.14 M
So, the given reaction will be as follows.
Initial: 0.43 0.14 0
Change: -0.14 -0.14 0.14
Equilibrium: 0.29 0 0.14
As it is known that value of = 4.74
Therefore, according to Henderson-Hasselbalch equation calculate the pH as follows.
pH =
=
= 4.74 + (-0.316)
= 4.42
Therefore, we can conclude that the pH of given reaction is 4.42.
"The ability of a base to react with a soluble metal salt" demonstrates characteristic of a base.
<u>Answer:</u> Option D
<u>Explanation:</u>
As the sodium hydroxide react with only with some metals. It is a very strong basic compound with a intense solubility in water and hygroscopic in nature. The ability of base is reflected from its potential to react with metals. In the given reaction:
is an acidic property showing salt which is added with sodium hydroxide and this reaction result into a pale blue precipitate of basic copper hydroxide & sodium sulphate which is neutral salt. The reaction is a double displacement and precipitation reaction.