Write balanced complete ionic and net ionic equations for each reaction. 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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Ch.5 - Introduction to Solutions and Aqueous Solutions

Problem 55d

Chapter 5, Problem 55d

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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Identify the reactants and products in the given chemical equation: Na_3PO_4(aq) + NiCl_2(aq) → Ni_3(PO_4)_2(s) + NaCl(aq).

Write the balanced molecular equation for the reaction: 2 Na_3PO_4(aq) + 3 NiCl_2(aq) → Ni_3(PO_4)_2(s) + 6 NaCl(aq).

Write the complete ionic equation by breaking all the soluble ionic compounds into their respective ions: 6 Na^+(aq) + 2 PO_4^{3-}(aq) + 3 Ni^{2+}(aq) + 6 Cl^-(aq) → Ni_3(PO_4)_2(s) + 6 Na^+(aq) + 6 Cl^-(aq).

Identify and cancel out the spectator ions that appear on both sides of the complete ionic equation: Na^+(aq) and Cl^-(aq).

Write the net ionic equation by including only the ions and compounds that participate in the reaction: 2 PO_4^{3-}(aq) + 3 Ni^{2+}(aq) → Ni_3(PO_4)_2(s).

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Key Concepts

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

Ionic Compounds and Solubility

Ionic compounds consist of positively and negatively charged ions. Their solubility in water is determined by the strength of the ionic bonds and the interactions with water molecules. For example, sodium phosphate (Na3PO4) and nickel(II) chloride (NiCl2) are soluble in water, dissociating into their respective ions, which is crucial for writing complete ionic equations.

Complete Ionic Equations

A complete ionic equation shows all the ions present in a reaction, including spectator ions that do not participate in the actual chemical change. In the given reaction, the complete ionic equation would include all ions from the reactants and products, allowing for a clear visualization of the species involved before simplification to the net ionic equation.

Net Ionic Equations

A net ionic equation represents only the species that undergo a chemical change during the reaction, omitting spectator ions. This simplification highlights the actual reaction taking place, such as the formation of solid nickel(II) phosphate (Ni3(PO4)2) from the ions in solution, providing a clearer understanding of the chemical process.

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Net Ionic Equations

Related Practice

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

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.

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

d. Na₃PO₄(aq) + NiCl₂(aq) → Ni₃(PO₄)₂(s) + NaCl(aq)

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)

Textbook Question

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

Textbook Question

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

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

Verified video answer for a similar problem:

Key Concepts

Ionic Compounds and Solubility

Complete Ionic Equations

Net Ionic Equations

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