Balance the equation for the following precipitation...

Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species $(\mathrm{s}, \ell, \mathrm{aq}, \text { or } \mathrm{g})$ $$\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow \mathrm{NiCO}_{3}+\mathrm{NaNO}_{3}$$

Balance the equation for the following precipitation reaction, and then write the net ionic equation. Indicate the state of each species $(\mathrm{s}, \ell, \mathrm{aq}, \text { or } \mathrm{g})$
$$\mathrm{Ni}\left(\mathrm{NO}_{3}\right)_{2}+\mathrm{Na}_{2} \mathrm{CO}_{3} \rightarrow \mathrm{NiCO}_{3}+\mathrm{NaNO}_{3}$$

Key Concepts

Solubility Rules

These rules help predict whether an ionic compound will dissolve in water. They are essential for determining which products in a reaction will remain in solution and which will form a precipitate, thereby guiding the construction of both full ionic and net ionic equations.

States of Matter

Indicating the physical states (solid, liquid, aqueous, gas) in a chemical equation is important for understanding the behavior of substances during a reaction. It communicates whether a substance is in solution, precipitated out, in a gaseous state, or in a pure solid or liquid state.

Balancing Chemical Equations

This concept involves ensuring that the number of atoms for each element is the same on both sides of a chemical equation. It is based on the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. Balancing equations often requires adjusting coefficients to achieve equal numbers of atoms for all elements involved.

Precipitation Reactions

Precipitation reactions are a type of double replacement reaction where two aqueous solutions combine and form an insoluble solid called a precipitate. Understanding these reactions requires knowing which combinations of ions will result in an insoluble compound based on solubility rules.

Net Ionic Equations

Net ionic equations remove the spectator ions from the full ionic equation to focus on the species that actually participate in the reaction. They highlight the chemical change by showing only the ions or molecules directly involved in forming the precipitate or other product.

Transcript

00:01 Hello everyone and thanks for joining me for a look at complete and net ionic equations.

00:06 For this problem, we're going to be given an unbalanced precipitation reaction.

00:14 Our job will be to balance the equation, assign states, then write the complete and net ionic equations.

00:35 And i'm going to go to the next page while we get ready to begin.

00:39 Okay, the equation we are given, the balanced chemical reaction, is nickel -2 nitrate, and we always start with aqueous, reacts with sodium carbonate, to produce, our products are nickel -2 carbonate and sodium -nitrate.

01:19 Now we have to figure out the states for our two products, and we know that, both alkali metals and nitrates are aqueous.

01:29 So this one is absolutely aqueous.

01:35 That's an aqueous.

01:37 And we know that most of our carbonates are insoluble, and this is an insoluble carbonate.

01:43 So here is our chemical equation, and now we need to balance it.

01:47 So i'm just going to do a quick look here and balance this by inspection.

01:52 Here i have two sodium, two nitrates, so i can look quickly, and if i put a two right here, i'm done.

02:01 There's our balanced chemical equation.

02:03 Part one, done.

02:05 We've got our states assigned, so that's done.

02:10 Now, let's write our complete ionic equation.

02:14 In order to do that, we're going to split all of our aqueous.