Respuesta :
Answer:
Net ionic equation for the reaction between MgCl₂ and NaOH in water:
[tex]\rm Mg^{2+}\; (aq) + 2\; OH^{-}\; (aq) \to Mg(OH)_2\;(s)[/tex].
Net ionic equation for the reaction between MgSO₄ and BaCl₂ in water:
[tex]\rm {Ba}^{2+}\; (aq) + {SO_4}^{2-}\;(aq) \to BaSO_4\; (s)[/tex].
Explanation:
Start by finding the chemical equations for each reaction:
MgCl₂ reacts with NaOH to form Mg(OH)₂ and NaCl. This reaction is a double decomposition reaction (a.k.a. double replacement reaction, salt metathesis reaction.) This reaction is feasible because one of the products, Mg(OH)₂, is weakly soluble in water and exists as a solid precipitate.
[tex]\rm MgCl_2\; (aq) + 2\; NaOH\; (aq)\to Mg(OH)_2 \; (s) + 2\; NaCl\; (aq)[/tex].
MgSO₄ reacts with BaCl₂ in a double decomposition reaction to produce BaSO₄ and MgCl₂. Similarly, the solid product BaSO₄ makes this reaction is feasible.
[tex]\rm MgSO_4\; (aq) + BaCl_2\; (aq) \to BaSO_4\; (s) + MgCl_2\; (aq)[/tex].
How to rewrite a chemical equation to produce a net ionic equation?
- Rewrite all reactants and products that ionizes completely in the solution as ions.
- Eliminate ions that exist on both sides of the equation to produce a net ionic equation.
Typical classes of chemicals that ionize completely in water:
- Soluble salts,
- Strong acids, and
- Strong bases.
Keep the formula of salts that are not soluble in water, weak acids, weak bases, and water unchanged.
Take the first reaction as an example, note the coefficients:
- MgCl₂ is a salt and is soluble in water. Each unit of MgCl₂ can be written as [tex]\rm Mg^{2+}[/tex] and [tex]\rm 2\; Cl^{-}[/tex].
- NaOH is a strong base. Each unit of NaOH can be written as [tex]\rm Na^{+}[/tex] and [tex]\rm OH^{-}[/tex].
- Mg(OH)₂ is a weak base and should not be written.
- NaCl is a salt and is soluble in water. Each unit of NaCl can be written as [tex]\rm Na^{+}[/tex] and [tex]\rm Cl^{-}[/tex].
[tex]\rm Mg^{2+} + 2\; Cl^{-} + 2\; Na^{+} + 2\; OH^{-} \to Mg(OH)_2\;(s) + 2\; Na^{+} + 2\; Cl^{-}[/tex].
Ions on both sides of the equation:
- [tex]\rm 2\; Cl^{-}[/tex], and
- [tex]\rm 2\; Na^{+}[/tex].
Add the state symbols:
[tex]\rm Mg^{2+}\; (aq) + 2\; OH^{-}\; (aq) \to Mg(OH)_2\;(s)[/tex].
For the second reaction:
[tex]\rm MgSO_4\; (aq) + BaCl_2\; (aq) \to BaSO_4\; (s) + MgCl_2\; (aq)[/tex].
[tex]\rm Mg^{2+} + 2\; {SO_4}^{2-} + Ba^{2+} + 2\; Cl^{-} \to BaSO_4\; (s) + Mg^{2+} + 2\; Cl^{-}[/tex].
[tex]\rm Ba^{2+}\; (aq) + {SO_4}^{2-}\; (aq) \to BaSO_4\; (s)[/tex].
The net ionic equation of the reaction
a. Mg²⁺ (aq) + 2OH⁻ (aq) ---> MgOH₂ (s)
b. Ba²⁺(aq) + SO₄²⁻(aq) ----> BaSO₄(s)
Further explanation
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:
• 1. soluble compound
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⁺
• 2. insoluble compounds
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 of MgCl₂ with NaOH:
MgCl₂ (aq) + 2NaOH (aq) -> Mg(OH)₂ (s) + 2NaCl (aq)
complete ion reaction:
Mg²⁺ (aq) + 2Cl⁻ (aq) + 2Na⁺ (aq) + 2OH⁻ (aq) -> Mg(OH)₂ + 2Na⁺ (aq) + 2Cl⁻(aq)
net ionic equation: Mg²⁺ (aq) + 2OH⁻ (aq) ---> MgOH₂ (s)
the reaction of MgSO₄ with BaCl₂
MgSO₄ (aq) + BaCl₂ (aq) -> BaSO₄ (s) + MgCl₂ (aq)
Complete ion reaction:
[tex]\rm Mg^{2+}(aq)+SO_4^{2-}(aq)+Ba^{2+}(aq)+2Cl^-(aq)\to BaSO_4(s)+Mg^{2+}(aq)+2Cl^-(aq)\\\\net\:ionic\:equation:Ba^{2+}(aq)+SO_4^{2-}(aq)\to BaSO_4(s)[/tex]
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Keywords: the net ionic equation, spectator ions, molecular equation,full ionic equation
