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This question asks you to write balanced net ionic equations for the following reactions that occur in aqueous solution.
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And if no reaction occurs, meaning no precipitate form is based on the solubility rules as a product, then you should indicate.
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To write the balanced net ionic equation, it's best to first write the complete formula equation.
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Balance it.
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Then pull everything apart that is soluble into its ions and get the complete ionic equation.
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Cancel the spectator ions, and what is left is the net ionic equation.
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Let's begin.
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A is sodium sulfate reacting with potassium chloride.
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When the cation switch places, we will get potassium sulfate, which is soluble, according to the solubility rules.
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Sulfates are soluble, and salts contain potassium are soluble, and sodium chloride.
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And sodium chloride, which is also soluble.
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Any salt containing sodium or any salt containing chloride is soluble, according to the solubility rules.
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Yes, there are a couple exceptions for chloride, which sodium chloride is not, and there's a couple exceptions for sulfate, which potassium sulfate is not.
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So this is no reaction, no precipitate will form.
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The next one is potassium sulfide reacting with calcium nitrate.
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Potassium has a plus one charge.
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Sulfide has a two minus charge, so we need two potassium for every sulfide.
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Calcium has a two plus charge.
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Nitrate has a one minus charge, so we need two nitrates for every calcium.
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When the cat ion switch places, calcium still has a two plus charge.
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Sulfide with a two minus charge requires just one of each of them for.
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Calcium sulfide.
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According to the solubility rules, all sulfides are insoluble, so this is our precipitate.
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The sulfide would not be insoluble if it contains an alkaline metal, such as potassium or sodium, or ammonium.
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That's why this is soluble.
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Then the other product would be potassium nitrate.
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Potassium has a plus one charge.
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Nitrate has a one minus charge, so we just need one of each of them.
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And according to the solubility rules, all salts containing potassium and nitrate or and or nitrate are soluble, so this is aqueous.
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Now we need to balance the reaction.
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We have two potassiums here.
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So we need to put a two here to get two potassium.
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That also gives us two nitrates.
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We already have two nitrates.
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So now it's balanced.
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Calcium sulfide being our precipitant.
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We'll then pull apart everything that is.
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Soluble into its ions.
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Potassium sulfide has two potassium and one sulfide, so we'll get two potassium and one sulfide.
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Calcium nitrate has one calcium and two nitrates, so we'll get one calcium and two nitrates.
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We'll keep calcium sulfide together as a solid, and then we have two potassium nitrates, so we'll get two potassiums and two nitrates.
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Hopefully you can see then that potassium and nitrate are our spectator ions, which cancel from both sides of the complete ionic equation.
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And what is left is the net ionic equation.
03:53
One calcium 2 plus combines with 1 sulfide 2 minus to produce calcium sulfide.
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Next we have sodium hydroxide reacting with silver nitrate.
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Sodium has a plus 1 charge.
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Hydroxide has a 1 minus charge, so we need just one of each of them.
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Silver has a plus 1 charge, nitrate has a 1 minus charge.
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So we need just one of each of them.
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Then when the cat -ion switch places, we will get sodium hydroxide, according to the silhou, i'm sorry, silver hydroxide.
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According to the solubility rules, all hydroxides are insoluble, except those with the alkali metals or ammonium.
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So silver hydroxide is insoluble and is our precipitate solid.
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The other product would be sodium nitrate.
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According to the solubility rules all sodium salts and all nitrate salts are soluble, so this is aqueous.
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Now we need to balance it.
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Turns out we just have one of each of everything on both sides, so it's already balanced.
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We'll pull apart our sodium hydroxide into one sodium and one hydroxide, our silver nitrate into one silver and one nitrate...