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Nikitich [7]
2 years ago
6

Which of the following types of equations will include spectator ions

Chemistry
2 answers:
krek1111 [17]2 years ago
6 0

Answer:- B) Full ionic equation

Explanations:- A molecular equation does not have ions. It is the non charge form of the elements of compounds. When we write the full or total ionic equation for the molecular equation then ions are written for the aqueous species. The ions present on both sides(reactant and product sides) in a full ionic equation are known as spectator ions or common ions. These ions are canceled to get the net ionic equation. For example, reaction of aqueous solution of silver nitrate with aqueous solution of barium chloride to form aqueous solution of barium nitrate and a precipitate of silver chloride.

Balanced molecular equation:-

BaCl_2(aq)+2AgNO_3(aq)\rightarrow Ba(NO_3)_2(aq)+2AgCl(s)

Full ionic equation:-

Ba^+^2(aq)+2Cl^-(aq)+2Ag^+(aq)+2NO_3^-(aq)\rightarrow Ba^+^2(aq)+2NO_3^-(aq)+2AgCl(s)

If we look at the above full ionic equation then barium ion and nitrate ions are the spectator ions are they are present on both sides.

So, while writing the net ionic equation, these spectator ions are canceled.

Net ionic equation:-

2Cl^-(aq)+2Ag^+(aq)\rightarrow2AgCl(s)

So, it is also clear from the above example that it's the full ionic equation that include spectator ions.

algol [13]2 years ago
5 0

B.<u> Full ionic equation</u> will include spectator ions

<h3>Further explanation </h3>

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 spectator ion 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)

For example Reaction between :

K₃PO₄(aq) + FeCl₃(aq)

Reactions that occur:

K₃PO₄(aq) + FeCl₃(aq) ⇒ 3KCl(aq) + FePO₄(s)

this reaction is called  Molecular equation

FePO₄(s) solid form that does not decompose in the form of ions

So the ionic equation becomes:

  • 3K+(aq) + PO₄³⁻(aq) + Fe³⁺(aq) + 3Cl⁻(aq) ⇒ 3K⁺(aq) + 3Cl⁻(aq) + FePO₄(s)

this reaction is called Full ionic equation

There is spectator ions that is 3K⁺(aq) and 3Cl⁻(aq) , so that if it is removed a net ionic equation will be formed:

  • PO₄³⁻(aq) + Fe³⁺(aq) ⇒ FePO₄(s)

this reaction is called Net ionic equation

<h3>Learn more </h3>

the net ionic equation

brainly.com/question/8885824

brainly.com/question/11854070

brainly.com/question/10280219

brainly.com/question/9830467

Keywords: the net ionic equation, spectator ions, molecular equation,full ionic equation, net ionic equation

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The concentration of diluted solution is 0.16 M

<u>Explanation:</u>

As, the number of moles of diluted solution and concentrated solution will be same.

So, the equation used to calculate concentration will be:

M_1V_1=M_2V_2

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M_1\text{ and }V_1 are the molarity and volume of the concentrated HCl solution

M_2\text{ and }V_2 are the molarity and volume of diluted HCl solution

We are given:

M_1=0.35M\\V_1=400mL\\M_2=?M\\V_2=(500+400)mL=900mL

Putting values in above equation, we get:

0.35\times 400=M_2\times 900\\\\M_2=\frac{0.35\times 400}{900}=0.16M

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Choose the correct net ionic equation for the reaction (if a reaction occurs) between CaCl2 and AgNO3: Group of answer choices
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Answer:

2Ag⁺(aq) + 2Cl⁻(aq) -> 2AgCl(s)

Explanation:

Silver nitrate and calcium chloride will react in a double displacement reaction (which has to produce a precipitate, a gas, or water to have a reaction).

This reaction will produce a silver chloride precipitate and a solution of calcium nitrate.

The reaction will be 2AgNO3(aq) + CaCl2(aq) -> 2AgCl(s) + Ca(NO3)2(aq)

To write a net ionic equation:

1. Write the balanced molecular equation.

   2AgNO3 + CaCl2 -> 2AgCl(ppt) + Ca(NO3)2

2. Write the balanced complete ionic equation.

To write the complete ionic equation:

- Start with a balanced molecular equation.

2AgNO3(aq) + CaCl2(aq) -> 2AgCl(s) + Ca(NO3)2(aq)

- Break all soluble strong electrolytes (compounds with (aq) beside them) into their ions

       indicate the correct formula and charge of each ion

       indicate the correct number of each ion

       write (aq) after each ion

- Bring down all compounds with (s), (l), or (g) unchanged.

2Ag⁺(aq) + 2NO³⁻(aq) + Ca²⁺(aq) + 2Cl⁻(aq) -> 2AgCl(s) + Ca²⁺(aq) + 2NO³⁻(aq)

3. Cross out the spectator ions that are present. Spectator ions are ions that are present in the reaction mixture but do not participate in it. You can recognize spectator ions by looking for ions that are present on both sides of the equation.

4. Write the "leftovers" as the net ionic equation.

2Ag⁺(aq) + 2Cl⁻(aq) -> 2AgCl(s)

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