Answer:
5.916x10⁻³ mol OH⁻
Explanation:
The reaction that takes place is:
- H₂SO₄ + 2KOH → K₂SO₄ + 2H₂O
First we <u>calculate the added moles of each reagent</u>, using the <em>given volumes and concentrations</em>:
- H₂SO₄ ⇒ 0.144 M * 27.55 mL = 3.967 mmol H₂SO₄
- KOH ⇒ 0.316 M * 43.84 mL = 13.85 mmol KOH
Now we<u> calculate how many KOH moles reacted with 3.967 mmol H₂SO₄</u>:
- 3.967 mmol H₂SO₄ *
= 7.934 mmol KOH
Finally we calculate how many OH⁻ moles remained after the reaction
- 13.85 mmol - 7.934 mmol = 5.916 mmol OH⁻
- 5.916 mmol / 1000 = 5.916x10⁻³ mol OH⁻
Answer:
When the two atoms are in contact, potassium readily transfers its outer electron to chlorine which readily accepts it, resulting in both atoms achieving a state of eight outermost electrons. With this electron transfer, the ionic bond in KCl is formed.
Density = mass/volume = 316/22.5 = 14.045g/mL.
There can be an electrolytic cell from iron and copper electrodes by connecting a a battery.
<h3>What is a voltaic cell?</h3>
A voltaic cell is a cell that produces energy via a spontaneous chemical reaction. An electrolytic cell produces energy by a nonspontaneous chemical reaction.
Now, we know that we can reverse the electrodes in the voltaic cell and connect a cell. In such case, we can be able to create an electrolytic cell from iron and copper electrodes.
Learn more about electrolytic cell:brainly.com/question/8538807
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