Predict the products of each reaction and write balanced...

Key Concepts

Double Displacement Reactions

Double displacement reactions involve the exchange of ions between two reactants to form two new compounds. This type of reaction is common among ionic compounds dissolved in water, where the cations and anions recombine into potentially new products through the swapping process. It is an important concept because it provides a framework for predicting reaction outcomes in aqueous solutions.

Precipitation Reactions

Precipitation reactions occur when two aqueous ionic compounds react and form an insoluble compound, known as the precipitate. In these reactions, solubility rules are used to determine which combinations of ions will yield a compound that does not remain in solution. This concept is crucial for understanding why certain products separate from the solution, leading to a visible change.

Acid-Base Reactions

Acid-base reactions involve the donation of protons (H? ions) from an acid to a base, often resulting in the formation of water and a salt. When acids react with carbonate or sulfide compounds, additional reaction pathways such as gas evolution (for example, CO? formation) may occur. This concept helps in predicting the products and understanding the driving forces behind the reaction.

Complete Ionic Equations

Complete ionic equations represent all of the soluble ionic compounds in their dissociated form as separate ions. This format provides a detailed picture of the reaction in aqueous solutions by breaking down compounds into their constituent ions, while maintaining the conservation of mass and charge.

Net Ionic Equations

Net ionic equations simplify complete ionic equations by removing species that appear on both sides of the equation, known as spectator ions. This process highlights the actual chemical change taking place during the reaction and provides clarity on the essential reactive species.

Balancing Chemical Equations

Balancing chemical equations is the process of ensuring that the number of atoms for each element, as well as the overall charge, is the same on both sides of the reaction. This reflects the law of conservation of mass and charge, which is fundamental in accurately representing any chemical reaction.

Transcript

00:02 This question asks you to write the balanced complete ionic and net ionic equations.

00:09 If no reaction occurs, you simply indicate no reaction.

00:13 The first one is ammonium sulfate.

00:17 Ammonium has a 1 plus charge.

00:24 Sulfate has a 2 minus charge, so we're going to need two ammoniums for every sulfate.

00:30 According to solubility rules, this is aqueous.

00:32 It reacts with barium nitrate.

00:37 Barium, an alkaline earth metal, has a 2 plus charge.

00:40 Nitrate has a 1 -minus charge.

00:42 So we need 2 nitrates.

00:44 According to solubility rules, it's also aqueous.

00:48 This will then form barium sulfate when the cat -ion switch places.

00:54 Most sulfates are soluble, but barium is an exception, so it's insoluble and a solid.

01:02 Barium 2 plus sulfate 2 minus one of each of them ammonium has a 1 plus charge it's going to combine with nitrate with a 1 minus charge so we just need one of each of them but now to balance them two ammoniums two nitrates we put a 2 right there then we'll separate everything that's soluble the ammonium sulfate separates into two ammoniums 1 sulfate barium nitrate 1 barium 2 nitrates barium sulfate is soluble, so it's going to stay as a, i'm sorry, insoluble, so it stays as a solid.

01:44 And then the ammonium nitrate, because there are two of them, gives us two ammoniums and two nitrates.

01:52 We'll recognize that the ammoniums are commentable sides as spectator ions, as are the nitrates.

02:00 So this is our complete ionic equation.

02:04 When we remove the spectator ions, we have the net ionic equation.

02:12 Next, we have hydrochloric acid.

02:15 Hydrochloric acid is h -c -l, h with a 1 -plus charge, and chloride with a 1 -1 -minus.

02:20 Just requires one of each of them.

02:23 Then we have that reacting with lithium -carbonate.

02:26 Lithium has a 1 -plus charge.

02:28 Carbonate has a 2 -minus, so we need 2 -1 -6 -so we need 2 -3 for every carbonate.

02:32 According to solubility rules, both of these are soluble.

02:35 So when an acid reacts with a carbonate containing salt, we end up getting carbon dioxide in water and another salt.

02:45 The salt that would form when the cation of the carbonate combines with the anion of the acid, lithium chloride.

02:53 Lithium has a one plus charge, chloride has a one minus, so we just need one of each of them.

03:00 But because we have two lithiums here, we're going to need to put a two in front of the lithium, giving us two chlorides.

03:06 We're going to need to put a two in front of the hcl.

03:09 Now what we're going to do is pull apart the hcl into two hydrogens and two chlorides, and we'll still have the lithium separated into two lithiums and one carbonate.

03:21 Then we'll have our carbon dioxide and water, and the two lithium chlorides will produce two lithium ions and two chloride anions.

03:32 We recognize that the lithium ions, the two of them, and the two chlorides are common to both sides.

03:37 So here's our complete ionic equation.

03:40 We remove the spectator ions, and we have the net ionic equation.

03:45 Two hydrogens react with one carbonate to produce carbon dioxide and water.

03:51 Next we have sulfuric acid reacting with strontium nitrate.

03:56 Sulfuric acid has sulfate, which has a two minus charge and two hydrogens, each with a one plus charge.

04:03 Strontium, an alkaline earth metal, has a two plus charge...

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