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DochEvi [55]
2 years ago
12

What is the ionic equation for HC2H3O2(aq)+NH4OH(aq)=NH4C2H3O2(aq)+H2O

Chemistry
1 answer:
kondaur [170]2 years ago
5 0

Answer:

Ionic equation:

H⁺(aq)  + C₂H₃O₂⁻ (aq) + NH₄⁺(aq)  + OH⁻(aq)     →    NH₄⁺(aq)  + C₂H₃O₂⁻ (aq) +  H₂O(l)

Explanation:

Chemical equation:

HC₂H₃O₂(aq) + NH₄OH(aq) → NH₄C₂H₃O₂(aq) + H₂O(l)

Ionic equation:

H⁺(aq)  + C₂H₃O₂⁻ (aq) + NH₄⁺(aq)  + OH⁻(aq)     →    NH₄⁺(aq)  + C₂H₃O₂⁻ (aq) +  H₂O(l)

Net ionic equation:

H⁺(aq)  + OH⁻(aq)     →     H₂O(l)

The C₂H₃O₂⁻ (aq) and NH₄⁺(aq) and are spectator ions that's why these are not written in net ionic equation. The water can not be splitted into ions because it is present in liquid form.

Spectator ions:

These ions are same in both side of chemical reaction. These ions are cancel out. Their presence can not effect the equilibrium of reaction that's why these ions are omitted in net ionic equation.  

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Sergeu [11.5K]

Answer:

.0556 L

Explanation:

First, convert the 1.35 M to 1.35 mol/L in order for the units to correctly cancel out.

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2 years ago
What type of organic compound has the empirical formula CH2O and can serve as energy storage or the starting material for fats a
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3 years ago
Calculate the Molarity when a 6.11 mL solution of 0.1 H2SO4 is diluted with 105.12 mL of water
barxatty [35]

Molarity after dilution : 0.0058 M

<h3>Further explanation </h3>

The number of moles before and after dilution is the same  

The dilution formula

 M₁V₁=M₂V₂

M₁ = Molarity of the solution before dilution  

V₁ = volume of the solution before dilution  

M₂ = Molarity of the solution after dilution  

V₂ = Molarity volume of the solution after dilution

M₁=0.1 M

V₁=6.11

V₂=105.12

\tt M_2=\dfrac{M_1.V_1}{V_2}=\dfrac{0.1\times 6.11}{105.12}=0.0058~M

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