Double Displacement Reactions - Worksheet #5: Double-Replacement ... - Free Printable
Educational worksheet: Double Displacement Reactions - Worksheet #5: Double-Replacement .... Download and print for classroom or home learning activities.
PNG
1200×1554
220.3 KB
Free · Personal Use
Quality Assured by Worksheets Library Team
Reviewed for educational accuracy and age-appropriateness
ID: #1374344
⭐
Show Answer Key & Explanations
Step-by-step solution for: Double Displacement Reactions - Worksheet #5: Double-Replacement ...
▼
Show Answer Key & Explanations
Step-by-step solution for: Double Displacement Reactions - Worksheet #5: Double-Replacement ...
Let’s go step by step through each double-replacement reaction. Remember: in these reactions, the positive ions (cations) and negative ions (anions) “switch partners.” Then we check if any product is a gas, water, or precipitate — if not, no reaction occurs (we put an X).
We’ll use common solubility rules:
- Most nitrates, acetates, alkali metal salts, and ammonium salts are soluble.
- Chlorides are soluble except with Ag⁺, Pb²⁺, Hg₂²⁺.
- Sulfides, hydroxides, carbonates, phosphates are often insoluble (except with alkali metals or NH₄⁺).
- Acids + bases → salt + water.
- Acids + sulfides → salt + H₂S gas.
- Acids + carbonates → salt + CO₂ gas + water.
---
1. aluminum iodide + mercury(II) chloride →
Already done:
AlI₃ + HgCl₂ → AlCl₃ + HgI₂
HgI₂ is insoluble (precipitate), so reaction occurs.
✔ Products: aluminum chloride + mercury(II) iodide
---
2. silver nitrate + potassium phosphate →
AgNO₃ + K₃PO₄ → switch partners:
→ Ag₃PO₄ + KNO₃
Check solubility:
- KNO₃ = soluble (all nitrates and alkali metals)
- Ag₃PO₄ = insoluble (silver phosphate is a precipitate)
✔ Reaction occurs.
Products: silver phosphate + potassium nitrate
---
3. copper(II) bromide + aluminum chloride →
CuBr₂ + AlCl₃ → switch:
→ CuCl₂ + AlBr₃
Check solubility:
- CuCl₂ = soluble
- AlBr₃ = soluble
No precipitate, no gas, no water → ✘ No reaction.
Final: X
---
4. calcium acetate + sodium carbonate →
Ca(C₂H₃O₂)₂ + Na₂CO₃ → switch:
→ CaCO₃ + NaC₂H₃O₂
Check:
- NaC₂H₃O₂ = soluble (sodium salt)
- CaCO₃ = insoluble (carbonate of Ca²⁺ is precipitate)
✔ Reaction occurs.
Products: calcium carbonate + sodium acetate
---
5. ammonium chloride + mercury(I) acetate →
NH₄Cl + Hg₂(C₂H₃O₂)₂ → switch:
→ NH₄C₂H₃O₂ + Hg₂Cl₂
Check:
- NH₄C₂H₃O₂ = soluble (ammonium salt)
- Hg₂Cl₂ = insoluble (mercury(I) chloride is a precipitate — also called calomel)
✔ Reaction occurs.
Products: ammonium acetate + mercury(I) chloride
---
6. calcium nitrate + hydrochloric acid →
Ca(NO₃)₂ + HCl → switch:
→ CaCl₂ + HNO₃
Both products are strong electrolytes and soluble:
- CaCl₂ = soluble
- HNO₃ = strong acid, fully dissociated
No precipitate, no gas, no water formed → ✘ No reaction.
Final: X
*(Note: Even though you’re mixing acid and salt, unless it forms weak acid, gas, or precipitate, no net reaction.)*
---
7. iron(II) sulfide + hydrochloric acid →
FeS + HCl → switch:
→ FeCl₂ + H₂S
H₂S is a gas! (rotten egg smell)
✔ Reaction occurs.
Products: iron(II) chloride + hydrogen sulfide gas
---
8. copper(II) hydroxide + acetic acid →
This is acid + base → neutralization → salt + water
Cu(OH)₂ + CH₃COOH → switch:
→ Cu(CH₃COO)₂ + H₂O
Water is formed → ✔ reaction occurs.
Products: copper(II) acetate + water
*(Note: You may need to balance later, but for naming products, this is fine.)*
---
9. calcium hydroxide + phosphoric acid →
Acid + base → salt + water
Ca(OH)₂ + H₃PO₄ → switch:
→ Ca₃(PO₄)₂ + H₂O
Wait — let’s think about charges:
Ca²⁺ and PO₄³⁻ → formula is Ca₃(PO₄)₂
H⁺ and OH⁻ → H₂O
So yes:
3Ca(OH)₂ + 2H₃PO₄ → Ca(PO₄)₂ + 6H₂O
But for product names only:
✔ Products: calcium phosphate + water
Calcium phosphate is insoluble (precipitate), and water is formed → definitely reacts.
---
10. calcium bromide + potassium hydroxide →
CaBr₂ + KOH → switch:
→ Ca(OH)₂ + KBr
Check solubility:
- KBr = soluble
- Ca(OH)₂ = slightly soluble — but technically, it’s considered to form a precipitate in many contexts? Wait...
Actually, Ca(OH)₂ is *slightly* soluble — but in many high school curricula, it’s treated as forming a precipitate when mixed with strong base? Let’s be precise.
Solubility rule: Hydroxides are insoluble except Group 1 and Ba²⁺, Sr²⁺, Ca²⁺ are *marginally* soluble — but often in worksheets like this, if it’s not clearly soluble, they might expect precipitate.
BUT — wait: both reactants are soluble, and products: KBr is soluble, Ca(OH)₂ is sparingly soluble — does that count?
Actually, in most standard double replacement worksheets, if one product is even slightly insoluble, they consider it a precipitate.
However, let’s check real behavior: Mixing CaBr₂ and KOH gives a cloudy solution due to Ca(OH)₂ precipitation.
✔ So reaction occurs.
Products: calcium hydroxide + potassium bromide
*(Some sources say "no reaction" because Ca(OH)₂ is somewhat soluble — but given the context of the worksheet asking to use solubility table, and since Ca(OH)₂ is listed as “slightly soluble” or “insoluble” in many tables, we’ll go with reaction occurring.)*
Wait — let me double-check typical textbook treatment.
In many high school texts, Ca(OH)₂ is considered to form a precipitate when produced in solution from soluble salts. For example, limewater test for CO₂ uses Ca(OH)₂ suspension.
So I’ll go with: ✔ reaction occurs.
Products: calcium hydroxide + potassium bromide
---
Now, compiling final answers for all 10:
1. aluminum chloride + mercury(II) iodide
2. silver phosphate + potassium nitrate
3. X
4. calcium carbonate + sodium acetate
5. ammonium acetate + mercury(I) chloride
6. X
7. iron(II) chloride + hydrogen sulfide
8. copper(II) acetate + water
9. calcium phosphate + water
10. calcium hydroxide + potassium bromide
──────────────────────────────────────
Final Answer:
1. aluminum chloride + mercury(II) iodide
2. silver phosphate + potassium nitrate
3. X
4. calcium carbonate + sodium acetate
5. ammonium acetate + mercury(I) chloride
6. X
7. iron(II) chloride + hydrogen sulfide
8. copper(II) acetate + water
9. calcium phosphate + water
10. calcium hydroxide + potassium bromide
We’ll use common solubility rules:
- Most nitrates, acetates, alkali metal salts, and ammonium salts are soluble.
- Chlorides are soluble except with Ag⁺, Pb²⁺, Hg₂²⁺.
- Sulfides, hydroxides, carbonates, phosphates are often insoluble (except with alkali metals or NH₄⁺).
- Acids + bases → salt + water.
- Acids + sulfides → salt + H₂S gas.
- Acids + carbonates → salt + CO₂ gas + water.
---
1. aluminum iodide + mercury(II) chloride →
Already done:
AlI₃ + HgCl₂ → AlCl₃ + HgI₂
HgI₂ is insoluble (precipitate), so reaction occurs.
✔ Products: aluminum chloride + mercury(II) iodide
---
2. silver nitrate + potassium phosphate →
AgNO₃ + K₃PO₄ → switch partners:
→ Ag₃PO₄ + KNO₃
Check solubility:
- KNO₃ = soluble (all nitrates and alkali metals)
- Ag₃PO₄ = insoluble (silver phosphate is a precipitate)
✔ Reaction occurs.
Products: silver phosphate + potassium nitrate
---
3. copper(II) bromide + aluminum chloride →
CuBr₂ + AlCl₃ → switch:
→ CuCl₂ + AlBr₃
Check solubility:
- CuCl₂ = soluble
- AlBr₃ = soluble
No precipitate, no gas, no water → ✘ No reaction.
Final: X
---
4. calcium acetate + sodium carbonate →
Ca(C₂H₃O₂)₂ + Na₂CO₃ → switch:
→ CaCO₃ + NaC₂H₃O₂
Check:
- NaC₂H₃O₂ = soluble (sodium salt)
- CaCO₃ = insoluble (carbonate of Ca²⁺ is precipitate)
✔ Reaction occurs.
Products: calcium carbonate + sodium acetate
---
5. ammonium chloride + mercury(I) acetate →
NH₄Cl + Hg₂(C₂H₃O₂)₂ → switch:
→ NH₄C₂H₃O₂ + Hg₂Cl₂
Check:
- NH₄C₂H₃O₂ = soluble (ammonium salt)
- Hg₂Cl₂ = insoluble (mercury(I) chloride is a precipitate — also called calomel)
✔ Reaction occurs.
Products: ammonium acetate + mercury(I) chloride
---
6. calcium nitrate + hydrochloric acid →
Ca(NO₃)₂ + HCl → switch:
→ CaCl₂ + HNO₃
Both products are strong electrolytes and soluble:
- CaCl₂ = soluble
- HNO₃ = strong acid, fully dissociated
No precipitate, no gas, no water formed → ✘ No reaction.
Final: X
*(Note: Even though you’re mixing acid and salt, unless it forms weak acid, gas, or precipitate, no net reaction.)*
---
7. iron(II) sulfide + hydrochloric acid →
FeS + HCl → switch:
→ FeCl₂ + H₂S
H₂S is a gas! (rotten egg smell)
✔ Reaction occurs.
Products: iron(II) chloride + hydrogen sulfide gas
---
8. copper(II) hydroxide + acetic acid →
This is acid + base → neutralization → salt + water
Cu(OH)₂ + CH₃COOH → switch:
→ Cu(CH₃COO)₂ + H₂O
Water is formed → ✔ reaction occurs.
Products: copper(II) acetate + water
*(Note: You may need to balance later, but for naming products, this is fine.)*
---
9. calcium hydroxide + phosphoric acid →
Acid + base → salt + water
Ca(OH)₂ + H₃PO₄ → switch:
→ Ca₃(PO₄)₂ + H₂O
Wait — let’s think about charges:
Ca²⁺ and PO₄³⁻ → formula is Ca₃(PO₄)₂
H⁺ and OH⁻ → H₂O
So yes:
3Ca(OH)₂ + 2H₃PO₄ → Ca(PO₄)₂ + 6H₂O
But for product names only:
✔ Products: calcium phosphate + water
Calcium phosphate is insoluble (precipitate), and water is formed → definitely reacts.
---
10. calcium bromide + potassium hydroxide →
CaBr₂ + KOH → switch:
→ Ca(OH)₂ + KBr
Check solubility:
- KBr = soluble
- Ca(OH)₂ = slightly soluble — but technically, it’s considered to form a precipitate in many contexts? Wait...
Actually, Ca(OH)₂ is *slightly* soluble — but in many high school curricula, it’s treated as forming a precipitate when mixed with strong base? Let’s be precise.
Solubility rule: Hydroxides are insoluble except Group 1 and Ba²⁺, Sr²⁺, Ca²⁺ are *marginally* soluble — but often in worksheets like this, if it’s not clearly soluble, they might expect precipitate.
BUT — wait: both reactants are soluble, and products: KBr is soluble, Ca(OH)₂ is sparingly soluble — does that count?
Actually, in most standard double replacement worksheets, if one product is even slightly insoluble, they consider it a precipitate.
However, let’s check real behavior: Mixing CaBr₂ and KOH gives a cloudy solution due to Ca(OH)₂ precipitation.
✔ So reaction occurs.
Products: calcium hydroxide + potassium bromide
*(Some sources say "no reaction" because Ca(OH)₂ is somewhat soluble — but given the context of the worksheet asking to use solubility table, and since Ca(OH)₂ is listed as “slightly soluble” or “insoluble” in many tables, we’ll go with reaction occurring.)*
Wait — let me double-check typical textbook treatment.
In many high school texts, Ca(OH)₂ is considered to form a precipitate when produced in solution from soluble salts. For example, limewater test for CO₂ uses Ca(OH)₂ suspension.
So I’ll go with: ✔ reaction occurs.
Products: calcium hydroxide + potassium bromide
---
Now, compiling final answers for all 10:
1. aluminum chloride + mercury(II) iodide
2. silver phosphate + potassium nitrate
3. X
4. calcium carbonate + sodium acetate
5. ammonium acetate + mercury(I) chloride
6. X
7. iron(II) chloride + hydrogen sulfide
8. copper(II) acetate + water
9. calcium phosphate + water
10. calcium hydroxide + potassium bromide
──────────────────────────────────────
Final Answer:
1. aluminum chloride + mercury(II) iodide
2. silver phosphate + potassium nitrate
3. X
4. calcium carbonate + sodium acetate
5. ammonium acetate + mercury(I) chloride
6. X
7. iron(II) chloride + hydrogen sulfide
8. copper(II) acetate + water
9. calcium phosphate + water
10. calcium hydroxide + potassium bromide
Parent Tip: Review the logic above to help your child master the concept of double displacement reactions worksheet.
