Write balanced complete ionic and net ionic equations for each reaction. c. NaOH(aq) + HC 2 H 3 O 2 (aq) → H 2 O(l ) + NaC 2 H 3 O 2 (aq) d. Na 3 PO 4 (aq) + NiCl 2 (aq) → Ni 3 (PO 4 ) 2 (s) + NaCl(aq)

Hi everyone. So we're doing the following reaction below and we have to provide the balance complete and net ionic equations. So we need to first balance this. Um H C H. O two A quiz Plus en a two C. 03 A quiz. And it's gonna yield in A. CH. A quiz. C. 02 gas Plus H 20. Like when we have a hydrogen, a carbon oxygen and a sodium on both sides, We have two hydrogen over here, two carbon over here, flat oxygen. And to study them over here We have three hydrogen over here, two carbon over here, five auction over here, one sodium over here because we have to study on the reaction side, but one on the product side, The most part by two over here get to You can put it to in front of NACH 02 tsunami of four hydrogen and three carbon And seven oxygen over here. If you put a two in front of H C H 02, We're gonna have four hydrogen over here free carbon seven oxygen. So now this is balanced Now we need to write the complete ionic equation by writing all the ions and leave any solid liquid or gas together and do not break them up. I feel like all the equity solutions. Hc H 02 A quiz, it's gonna break up into H plus Equus Plus CHO two minus. Then we have N. A to C. 03. Hey chris I'm just gonna break up into two and a plus a quiz. C. 03 two minus a quiz. Then we have a. H. 02. Equus Gonna break up to any plus a quiz Plus c. h. 0. 2 minus a quiz. So for the complete ionic equation we're gonna have to H plus a quiz Plus two CH. Oh two minus a quiz. Plus to an A. Plus a quiz Plus c. 0. 3 two minus a quiz. And it's going to go to an A. Plus a quiz Plus two c. h. 0. 2 finest quiz C. 02 gas Plus H. 2. 0. Like when and for the net Ionic equation you can get rid of any spectator ions which exist as a reactor in the product any plus and C. H. Oh two minus our our spectator ions. So they're gonna cancel out. So for the net Ionic equation we're gonna have to H plus a quiz Plus c. 0. 3 2 Aquarius and it's gonna yell C. 02. Yes Plus H. 20. Like when thanks for watching my video and I hope it was helpful

Ch.5 - Introduction to Solutions and Aqueous Solutions

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Tro 6th Edition

Ch.5 - Introduction to Solutions and Aqueous Solutions

Problem 55c,d

Chapter 5, Problem 55c,d

Write balanced complete ionic and net ionic equations for each reaction.
c. NaOH(aq) + HC₂H₃O₂(aq) → H₂O(l ) + NaC₂H₃O₂(aq)
d. Na₃PO₄(aq) + NiCl₂(aq) → Ni₃(PO₄)₂(s) + NaCl(aq)

Verified step by step guidance

Identify the states of matter for each compound: NaOH(aq), HC_2H_3O_2(aq), H_2O(l), and NaC_2H_3O_2(aq).

Write the balanced molecular equation: NaOH(aq) + HC_2H_3O_2(aq) → H_2O(l) + NaC_2H_3O_2(aq).

Break down the aqueous compounds into their ions to write the complete ionic equation: Na^+(aq) + OH^-(aq) + HC_2H_3O_2(aq) → H_2O(l) + Na^+(aq) + C_2H_3O_2^-(aq).

Identify the spectator ions, which are ions that appear on both sides of the complete ionic equation without undergoing any change. In this case, Na^+(aq) is the spectator ion.

Write the net ionic equation by removing the spectator ions: OH^-(aq) + HC_2H_3O_2(aq) → H_2O(l) + C_2H_3O_2^-(aq).

Verified Solution

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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 in aqueous solutions. This equation is essential for understanding how ions interact in solution and sets the stage for identifying the net ionic equation.

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.

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, sodium hydroxide (a base) reacts with acetic acid (an acid) to produce water and sodium acetate. Understanding this concept is vital for predicting the products and writing the corresponding ionic equations.

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Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' c. copper(II) nitrate and magnesium sulfide

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Textbook Question

Write a molecular equation for the precipitation reaction that occurs (if any) when each pair of aqueous solutions is mixed. If no reaction occurs, write 'NO REACTION.' a. sodium chloride and lead(II) acetate b. potassium sulfate and strontium iodide c. cesium chloride and calcium sulfide d. chromium(III) nitrate and sodium phosphate

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Textbook Question

Write balanced complete ionic and net ionic equations for each reaction. CaS(aq) + CuCl₂(aq) → CuS(s) + CaCl₂(aq)

Textbook Question

Write balanced complete ionic and net ionic equations for each reaction. d. Na₃PO₄(aq) + NiCl₂(aq) → Ni₃(PO₄)₂(s) + NaCl(aq)

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Textbook Question

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

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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Textbook Question

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

Write balanced complete ionic and net ionic equations for each reaction. c. NaOH(aq) + HC2H3O2(aq) → H2O(l ) + NaC2H3O2(aq)d. Na3PO4(aq) + NiCl2(aq) → Ni3(PO4)2(s) + NaCl(aq)

Verified Solution

Key Concepts

Complete Ionic Equation

Net Ionic Equation

Acid-Base Reaction

Write balanced complete ionic and net ionic equations for each reaction.
c. NaOH(aq) + HC₂H₃O₂(aq) → H₂O(l ) + NaC₂H₃O₂(aq)
d. Na₃PO₄(aq) + NiCl₂(aq) → Ni₃(PO₄)₂(s) + NaCl(aq)