Answer:
A. To focus on only those ions that form the precipitate
Explanation:
Net ionic equations cancel out the ions that appear on both sides of the reaction because they essentially don't participate in the reaction. This is very useful when dealing with redox reactions because are complicated enough without spectator ions being in the way, so they help focus on those ions that actually form the precipitate.
Key Terms
- Spectator Ions: an ion that does not take part in the chemical reaction.
- Net ionic equations: a equation where ions that appear on both sides are canceled out.
- Redox reaction: an oxidation-reduction reaction.
The pH of a buffer solution containing acid of pKa 7.5 will be 8.1.
The pH of a solution indicates its acidity or basicity. A pH below 7 is acidic, while pH above 7 is basic. 7 is considered as the neutral value.
A buffer is a solution that has the ability to resist the change in pH when an acid or a base is added to it. The natural example of buffer is blood.
According to the question, pKa of acid = 7.5
If concentration of base is x then, concentration of acid will be x/4.
According to the Henderson–Hasselbalch equation,
pH = pKa + log [A⁻] / [HA]
pH = 7.5 + log [
]
pH = 7.5 + log 4 ⇒ 7.5 + 0.602
pH = 8.1
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Idk i’m on that question now
Answer:
Explanation:
Incorrect name correct name
a) calcium dichloride calcium chloride
b) copper(II) oxide copper(I) oxide
c) stannous tetrafluoride stannic fluoride
d) hydrogen chloride acid hydrochloric acid
