I don't know man hahahaha
Answer:
The chemical formula for ammonium hypochlorite is NH4ClO.
The chemical formula for ammonium nitrate is NH4NO3.
Explanation:
These two are correct
Na₂CO₃(s) → 2Na⁺(aq) + CO₃²⁻(aq)
The sodium carbonate formed from a strong base and a weak acid. Hydrolysis is subjected to the anion of a weak acid.
CO₃²⁻ + H₂O ⇄ HCO₃⁻ + OH⁻
HCO₃⁻ + H₂O ⇄ H₂CO₃ + OH⁻
pH>7 alkaline solution
2Na⁺ + CO₃²⁻ + 2H₂O ⇄ 2Na⁺ + 2OH⁻ + H₂CO₃
Answer:
C.0.28 V
Explanation:
Using the standard cell potential we can find the standard cell potential for a voltaic cell as follows:
The most positive potential is the potential that will be more easily reduced. The other reaction will be the oxidized one. That means for the reactions:
Cu²⁺ + 2e⁻ → Cu E° = 0.52V
Ag⁺ + 1e⁻ → Ag E° = 0.80V
As the Cu will be oxidized:
Cu → Cu²⁺ + 2e⁻
The cell potential is:
E°Cell = E°cathode(reduced) - E°cathode(oxidized)
E°cell = 0.80V - (0.52V)
E°cell = 1.32V
Right answer is:
<h3>C.0.28 V
</h3>
<h3 />
Explanation:
Let us assume that mass of nickel(II) iodide is 2.90 g, volume is 150.ml, and concentration is 0.70 M.
When
is added into the solution then it will not affect the
concentration.
![NiI_{2} \rightarrow Ni^{2+} + 2I^{-}](https://tex.z-dn.net/?f=NiI_%7B2%7D%20%5Crightarrow%20Ni%5E%7B2%2B%7D%20%2B%202I%5E%7B-%7D)
Moles of
= ![\frac{mass}{\text{molar mass of nickel iodide}}](https://tex.z-dn.net/?f=%5Cfrac%7Bmass%7D%7B%5Ctext%7Bmolar%20mass%20of%20nickel%20iodide%7D%7D)
=
= 0.00928 mol
Moles of
= ![2 \times moles of NiI_{2}](https://tex.z-dn.net/?f=2%20%5Ctimes%20moles%20of%20NiI_%7B2%7D)
= ![2 \times 0.00928](https://tex.z-dn.net/?f=2%20%5Ctimes%200.00928)
= 0.01856 mol
Molarity of
= ![\frac{moles of I^{-}}{\text{volume of solution}}](https://tex.z-dn.net/?f=%5Cfrac%7Bmoles%20of%20I%5E%7B-%7D%7D%7B%5Ctext%7Bvolume%20of%20solution%7D%7D)
= ![\frac{0.01856}{0.150}](https://tex.z-dn.net/?f=%5Cfrac%7B0.01856%7D%7B0.150%7D)
= 0.124 M
Thus, we can conclude that final molarity of iodide anion in the solution is 0.124 M.