Answer:
- <em>The net ionic equation is: </em><u>Ag⁺ (aq) + Cl ⁻ (aq) → AgCl (s)</u>
Explanation:
<u>1) Start by writing the total ionic equation:</u>
The total ionic equation shows each aqueous substance in its ionized form, while the solid or liquid substances are shown with their chemical formula.
These are the ionic species:
- AgF (aq) → Ag⁺ (aq) + F⁻ (aq)
- NH₄Cl (aq) → NH₄⁺ (aq) + Cl ⁻ (aq)
- NH₄F(aq) → NH₄⁺ (aq) + F⁻ (aq)
Then, replace each chemical formula in the chemical equation by those ionic forms:
- Ag⁺ (aq) + F⁻ (aq) + NH₄⁺ (aq) + Cl ⁻ (aq) → AgCl (s) + NH₄⁺ (aq) + F⁻ (aq)
That is the total ionic equation.
<u>2) Spectator ions:</u>
The ions that appear in both the reactant side and the product side are considered spectator ions (they do not change), and so they are canceled.
In our total ionic equation they are F⁻ (aq) and NH₄⁺ (aq).
After canceling them, you get the net ionic equation:
<u>3) Net ionic equation:</u>
- Ag⁺ (aq) + Cl ⁻ (aq) → AgCl (s) ← answer
C its Nylon that's the Synthetic polymer that doesnt wear out easily
Answer : The pH of the resulting buffer is, 5.22
Explanation : Given,

First we have to calculate the moles of 

and,

The balanced chemical reaction is:

Moles of HA left = 0.117 mol - 0.08 mol = 0.037 mol
Moles of
= 0.08 mol
The expression used for the calculation of
is,

Now put the value of
in this expression, we get:



Now we have to calculate the pH of buffer.
Using Henderson Hesselbach equation :
![pH=pK_a+\log \frac{[Salt]}{[Acid]}](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%20%5Cfrac%7B%5BSalt%5D%7D%7B%5BAcid%5D%7D)
![pH=pK_a+\log \frac{[A^-]}{[HA]}](https://tex.z-dn.net/?f=pH%3DpK_a%2B%5Clog%20%5Cfrac%7B%5BA%5E-%5D%7D%7B%5BHA%5D%7D)
Now put all the given values in this expression, we get:


Thus, the pH of the resulting buffer is, 5.22
Structure 1 is satisfying octet rule because each atom surrounded by 8 electrons:
The valance electron for oxygen is 6, for sulfur is 6, but for hydrogen is 1. Therefore, the molecule has <span>valance electrons. Sulfur is bonded with 4 oxygen atoms, 4 single bonds, whereas 2 hydrogen atoms are bonded with 2 oxygen atoms.
But the actual structure is 2 but it violates octet rule since S is surrounded in this case with 12 electrons
</span>
Considering the reaction stoichiometry, the quantity of moles of H₂O produced is 3.02 moles.
The balanced reaction is:
CuO + H₂ → Cu + H₂O
By reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of moles of each compound participate in the reaction:
- CuO= 1 mole
- H₂= 1 mole
- Cu= 1 mole
- H₂O= 1 mole
The molar mass of the compounds present in the reaction is:
- CuO= 79.55 g/mole
- H₂= 2 g/mole
- Cu= 63.55 g/mole
- H₂O: 18 g/mole
Then, by reaction stoichiometry (that is, the relationship between the amount of reagents and products in a chemical reaction), the following amounts of mass of each compound participate in the reaction:
- CuO= 1 mole× 79.55 g/mole= 79.55 grams
- H₂= 1 mole× 2 g/mole= 2 grams
- Cu= 1 mole× 63.55 g/mole= 63.55 grams
- H₂O: 1 mole× 18 g/mole= 18 grams
Then, it is possible to determine the moles of H₂O necessary by the following rule of three: If by reaction stoichiometry 79.55 grams of CuO produces 1 mole of H₂O, 240 grams of CuO produces how many moles of H₂O?

<u><em>moles of H₂O= 3.02 moles</em></u>
Finally, the quantity of moles of H₂O produced is 3.02 moles.
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