The net ionic equation: Ag⁺ (aq) + Cl⁻(aq) -> AgCl (s)
<h3>Further explanation </h3>The electrolyte in the solution produces ions.
The equation of a chemical reaction can be expressed in the equation of the ions
For strong electrolytes (the ionization rate = 1) is written in the form of separate ions, while the weak electrolyte (degree of ionization <1) is still written as an un-ionized molecule
In the ion equation, there is an ion spectator that is the ion which does not react because it is present before and after the reaction
When these ions are removed, the ionic equation is called the net ionic equation
For gases and solids including water (H₂O) can be written as an ionized molecule
So only the dissolved compound is ionized ((expressed in symbol aq)
Formation of precipitating compounds that cause reactions can occur from double-replacement reactions
Solubility Rules:
All compounds of Li⁺, Na⁺, K⁺, Rb⁺, Cs⁺, and NH₄⁺
All compounds of NO₃⁻ and C₂H₃O₂⁻
Compounds of Cl⁻, Br⁻, I⁻ except Ag⁺, Hg₂²⁺, Pb²⁺
Compounds of SO₄²⁻ except Hg₂²⁺, Pb²⁺, Sr²⁺, Ba²⁺
Compounds of CO₃²⁻ and PO₄³⁻ except for Compounds of Li +, Na +, K +, Rb +, Cs +, and NH₄ +
Compounds of OH− except Compounds of Li +, Na +, K +, Rb +, Cs +, NH₄⁺, Sr²⁺, and Ba²⁺
The reaction between AgNO₃ (aq) and NaCl (aq)
AgNO₃ (aq) + NaCl (aq) ⇒AgCl (s) + NaNO₃ (aq)
AgCl is an insoluble compound, so reactions can take place and double-replacement reactions occur
Complete ion reaction:
the net ionic equation
Answer: The products formed in this Bronsted-Lowry reaction are and
.
Explanation:
According to Bronsted-Lowry, acids are the species which donate hydrogen ions to another specie in a chemical reaction.
Bases are the species which accept a hydrogen ion upon chemical reaction.
For example,
Here, the products formed in this Bronsted-Lowry reaction are and
.
Thus, we can conclude that the products formed in this Bronsted-Lowry reaction are and
.