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2 answers:
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The question is incomplete, here is the complete question:
Consider the following reaction:
In the first 15.0 s of the reaction, 1.9×10⁻² mol of O₂ is produced in a reaction vessel with a volume of 0.480 L . What is the average rate of the reaction over this time interval?
<u>Answer:</u> The average rate of appearance of oxygen gas is
<u>Explanation:</u>
We are given:
Moles of oxygen gas =
Volume of solution = 0.480 L
Molarity is calculated by using the equation:
So,
The given chemical reaction follows:
The average rate of the reaction for appearance of is given as:
Or,
where,
= final concentration of oxygen gas = 0.0396 M
= initial concentration of oxygen gas = 0 M
= final time = 15.0 s
= initial time = 0 s
Putting values in above equation, we get:
Hence, the average rate of appearance of oxygen gas is
Answer:
The pH at the equivalence point is lower than 7
Explanation:
Given the titration involves a strong acid and a weak base
An example is the reaction between ammonia and hydrochloric acid in the aqueous phase
The pH of the base will ordinarily start high and drop rapidly with the additions of acid. As the equivalence point is approached, the pH will change more gradually, until finally one drop will cause a rapid pH transition through the equivalence point.
If a chemical indicator is used—methyl orange would be a good choice in this case—it changes from its basic to its acidic colour.
In strong acid-weak base titrations, the pH at the equivalence point is not 7 but below it. This is due to the production of a conjugate acid during the titration; it will react with water to produce hydronium ions.
