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Ch.4 - Chemical Quantities & Aqueous Reactions
Tro - Chemistry: A Molecular Approach 4th Edition
Tro4th EditionChemistry: A Molecular ApproachISBN: 9780134112831당신이 사용하는 게 아니라요?교과서 변경
모든 교과서Tro 4th EditionCh.4 - Chemical Quantities & Aqueous Reactions문제 80d
4장, 문제 80d

Write balanced complete ionic and net ionic equations for each reaction. d. HC2H3O2(aq) + K2CO3(aq) → H2O(l ) + CO2(g) + KC2H3O2(aq)

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Identify the reactants and products in the given chemical equation: HC2H3O2(aq) + K2CO3(aq) → H2O(l) + CO2(g) + KC2H3O2(aq).
Write the balanced molecular equation for the reaction. Ensure that the number of atoms of each element is the same on both sides of the equation.
Write the complete ionic equation by breaking all the soluble strong electrolytes (aqueous compounds) into their respective ions. Weak acids like HC2H3O2 do not dissociate completely, so they remain in molecular form.
Identify and cancel out the spectator ions, which are ions that appear on both sides of the complete ionic equation without undergoing any change.
Write the net ionic equation by including only the species that undergo a chemical change in the reaction. This equation should show the formation of the products from the reactants without the spectator ions.

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주요 개념

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Complete Ionic Equation

A complete ionic equation represents all the ions present in a solution during a chemical reaction. It shows the reactants and products in their ionic forms, highlighting the dissociation of soluble ionic compounds. This equation is essential for understanding how ions interact in solution and sets the stage for identifying the net ionic equation.
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가이드 코스
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Complete Ionic Equations

Net Ionic Equation

The net ionic equation simplifies the complete ionic equation by removing spectator ions—ions that do not participate in the actual chemical reaction. This equation focuses on the species that undergo a change, providing a clearer picture of the chemical process. It is crucial for understanding the essence of the reaction and the formation of products.
추천 영상:
가이드 코스
00:51
Net Ionic Equations

Acid-Base Reaction

An acid-base reaction involves the transfer of protons (H⁺ ions) between reactants, typically resulting in the formation of water and a salt. In the given reaction, acetic acid (HC2H3O2) acts as an acid, while potassium carbonate (K2CO3) acts as a base. Recognizing this type of reaction is vital for predicting the products and writing the corresponding ionic equations.
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01:09
Acid-Base Reaction
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교과서 질문

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a. K2SO4(aq) + CaI2(aq) → CaSO4(s) + KI(aq)

b. NH4Cl(aq) + NaOH(aq) → H2O(l) + NH3(g) + NaCl(aq)

c. AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

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교과서 질문

Write balanced complete ionic and net ionic equations for each reaction.

c. NaOH(aq) + HC2H3O2(aq) → H2O(l ) + NaC2H3O2(aq)

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교과서 질문

Write balanced complete ionic and net ionic equations for each reaction. a. K2SO4(aq) + CaI2(aq) → CaSO4(s) + KI(aq)

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Write balanced molecular and net ionic equations for the reaction between hydrobromic acid and potassium hydroxide.

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