Answer:
i don't thing i understand the question.
Explanation:
Answer:
Butanoic acid present in solution
Explanation:
In this case, we have a buffer solution of butanoic acid and sodium butanoate. In other words a reaction like this:
HC₄H₇O₂ + H₂O <------> C₄H₇O₂⁻ + H₃O⁺ Ka = 1.5x10⁻⁵
The low value of Ka means that this is a weak acid. So, after this, the NaOH is added to the solution.
The NaOH is a really strong base, so we might expect that the pH of the solution increase drastically, however this do not occur.
The reason for this is because the first thing to happen in this reaction is an acid base reaction.
The NaOH react with the butanoic acid still present in solution, because is a weak acid, so in solution, this acid is not completely dissociated into it's respective ions. So the butanoic acid reacts with the NaOH and the products:
HC₄H₇O₂ + NaOH <------> Na⁺C₄H₇O₂⁻ + H₂O
So, because of this, the pH increase but not much.
Answer:
Hi there!
I believe you are looking for the conjugate ACID of PH3 and in this case, the conjugate acid is PH4+
Answer:
Redox but not combustion
Explanation:
2K(s) + 2H₂O(l) → 2KOH(aq) + H₂(g)
This is a redox reaction, because the oxidation number of K increases from 0 to +1, while that of H decreases from +1 to 0.
It is not a combustion reaction, because combustion is the reaction
with O₂.
The equation for the combustion of potassium would be
4K(s) + O₂(g) ⟶ 2K₂O(s)
