which equations represent precipitation reactions?
□ na₂s + febr₂ → 2nabr + fes
□ mgso₄ + cacl₂ → mgcl₂ + caso₄
□ lioh + nh₄i → lii + nh₄oh
□ 2nacl + k₂s → na₂s + 2kcl
□ agno₃ + nacl → agcl + nano₃

Question

Accepted Answer

To determine which equations represent precipitation reactions, we need to recall that a precipitation reaction is a type of double - displacement reaction where an insoluble solid (precipitate) is formed from the reaction of two aqueous solutions. We can use the solubility rules to identify if a precipitate is formed.

### Step 1: Analyze $Na_{2}S + FeBr_{2}\to2NaBr + FeS$
- Sodium sulfide ($Na_{2}S$) and iron(II) bromide ($FeBr_{2}$) are both soluble in water (since most sodium salts and most bromide salts are soluble).
- The product iron(II) sulfide ($FeS$) is insoluble in water (sulfides of transition metals are generally insoluble). So, a precipitate ($FeS$) is formed. This is a precipitation reaction.

### Step 2: Analyze $MgSO_{4}+CaCl_{2}\to MgCl_{2}+CaSO_{4}$
- Magnesium sulfate ($MgSO_{4}$) and calcium chloride ($CaCl_{2}$) are soluble in water (most sulfate salts and most chloride salts are soluble).
- The product calcium sulfate ($CaSO_{4}$) has limited solubility in water (it is considered slightly soluble or insoluble in many cases, and will precipitate out). So, this is a precipitation reaction.

### Step 3: Analyze $LiOH + NH_{4}I\to LiI+NH_{4}OH$
- Lithium hydroxide ($LiOH$) and ammonium iodide ($NH_{4}I$) are soluble.
- The product ammonium hydroxide ($NH_{4}OH$) is unstable and decomposes into $NH_{3}$ and $H_{2}O$, and lithium iodide ($LiI$) is soluble. There is no precipitate formed. This is not a precipitation reaction.

### Step 4: Analyze $2NaCl + K_{2}S\to Na_{2}S + 2KCl$
- Sodium chloride ($NaCl$) and potassium sulfide ($K_{2}S$) are soluble.
- The products sodium sulfide ($Na_{2}S$) and potassium chloride ($KCl$) are also soluble (sodium salts and potassium salts are generally soluble). There is no precipitate formed. This is not a precipitation reaction.

### Step 5: Analyze $AgNO_{3}+NaCl\to AgCl + NaNO_{3}$
- Silver nitrate ($AgNO_{3}$) and sodium chloride ($NaCl$) are soluble.
- The product silver chloride ($AgCl$) is insoluble in water (chlorides of silver, lead, and mercury(I) are insoluble). So, a precipitate ($AgCl$) is formed. This is a precipitation reaction.

# Answer:
The equations that represent precipitation reactions are:
- $Na_{2}S + FeBr_{2}\to2NaBr + FeS$
- $MgSO_{4}+CaCl_{2}\to MgCl_{2}+CaSO_{4}$
- $AgNO_{3}+NaCl\to AgCl + NaNO_{3}$

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Question

Explanation:

Step 1: Analyze \(Na_{2}S + FeBr_{2}\to2NaBr + FeS\)

Step 2: Analyze \(MgSO_{4}+CaCl_{2}\to MgCl_{2}+CaSO_{4}\)

Step 3: Analyze \(LiOH + NH_{4}I\to LiI+NH_{4}OH\)

Step 4: Analyze \(2NaCl + K_{2}S\to Na_{2}S + 2KCl\)

Step 5: Analyze \(AgNO_{3}+NaCl\to AgCl + NaNO_{3}\)

Answer: