Give an example of a double replacement reaction.?
help me ill appreciate it,thanks
Answer:
NaCl + KNO3 --> NaNO3+ KCl
During double replacement, the cations and anions of two different compounds switch places.
K2SO4 +2 NaNO3 >> Na2SO4 + 2 KNO3
2KCl + Li2SO4 >> K2SO4 + 2 LiCl
3NaBr + K3PO4 >> Na3PO4 + 3 KBr
3 CaS + 2 K3PO4 >> Ca3(PO4)2 + 3 K2S
2 AgNO3 + Na2SO4 >> Ag2SO4 + 2 NaNO3
CuSO4 + ZnCl 2 -->CuCl2 + ZnSO4
A typical double replacement reaction can occur when two ionic compounds are mixed together.� In water these ionic compounds split apart into their respective anions and cations.� The cations now have an opportunity to swap anions.� A reaction occurs if , by swapping anions, a product is formed that cannot split apart into anions and cations.� Look at the following example:� the reaction of silver nitrate and potassium chloride.�� The silver, nitrate, potassium and chloride ions all begin in solution.� When a silver ion combines with a chloride ion, it leaves the solution and becomes a solid.� This drives the reaction to completion!!!
AgNO3(aq) + KCl(aq)� ‑‑‑‑>� AgCl(s) + KNO3(aq)
The reaction must be driven by one of three driving forces:� Formation of a solid, formation of a gas or formation of a weakly‑ionizing compound such as water.� Lets look to see what happens when the driving forces are not there.�
NaNO3(aq) + KCl(aq)� ‑‑X‑‑>� NaCl(aq) + KNO3(aq)
Nothing happens!!� Without a driving force there is no change in the solution so we say no reaction has taken place.� Note that even though we can write an equation for the reaction, no reaction takes place without a driving force!!
How can we tell if an ionic compound will be soluble in water?� There are a series of guidelines in your book.� On the next page I provide you with another presentation of these same rules:
Solubility Rules
1.� All compounds containing Na+, K+,� or NH4+ ions are soluble in water.
2. �All nitrates (NO3‑) are soluble in water.
3.� Most chlorides (Cl‑ ), and sulfates (SO42‑) are soluble.� Some important exceptions are silver chloride (AgCl), barium sulfate (BaSO4), and lead sulfate (PbSO4) which are insoluble.
4.� Most carbonates (CO32‑), phosphates (PO43‑), sulfides (S2‑), and hydroxides (OH‑) are insoluble in water.� Important exceptions are those of Na+, K+,� and NH4+, as well as barium hydroxide, Ba(OH)2.�
������������������������������...
How do you know if a gas will form?� If H2CO3 is formed it will form a gas by decomposing to H2O and CO2.� You will see that in this lab.� Other compounds that release water or a gas are
NH4OH and H2SO3.
When an strong acid and a strong base react, in an aqueous solutions, they produce a salt and water.� This is an example of a double displacement reaction where the driving force is the formation of the covalent compound water.� Often, the only way to tell if one of these reactions has occurred is by looking for the formation of heat or by using an acid/base indicator to tell if the base has neutralized the acid.� If you do not see a reaction occurring you may wish to ask your instructor for an appropriate indicator.�� (How can you tell what the color of the indicator will be in an acidic solution and a basic solution?� Answer:� Test the solutions individually.)�
Procedure
There are ten stations.� Please use the standard procedure at each station.
I.� Reacting CuSO4 solution with NaOH solution.
II.� Reacting Na2CO3 solution with HCl solution.
III.� Reacting KCl solution with Na2CO3 solution.
IV.� Reacting Na2SO4 solution with BaCl2 solution.
V.� Reacting NaOH solution with HCl solution.� (Use phenolphthalein indicator)
VI.� Reacting Na2CO3 solution with CaCl2 solution.
VII.� Reacting Ni(NO3)2 solution with NaOH solution.
VIII. Reacting Na2SO4 solution with Cu(N03)2 solution.
IX.� Reacting KOH solution with MgCl2 solution.
X.� Reacting NaHCO3 solution with HNO3 solution.
Standard procedure
1.�������� Transfer 10‑15 drops of one solution into test tube.� Record in your notebook a description of the appearance of the first solution.
2.�������� Record in your notebook your description of the second solution.
3.�������� Using a Beral pipet, add 10‑15 drops of the second solution to the test tube.� Record in your notebook your description of the appearance of the reaction mixture.� Dispose of waste appropriately,�
4.�������� a.� Write in your notebook a complete, molecular equation, including states.
b.� Write in your notebook the driving force and make sure that the equation is balanced.
Purpose:� To observe double replacement reactions
Procedure:� As stated in lab handout and as presented by the instructor.� All reagents had a concentration of 1 M.
Conclusion:� In all of the double replacement reactions where a chemical reaction took place, the reaction was driven by one of these driving forces: formation of a gas, formation of a solid,� formation of a water, or the reaction in which a strong acid reacts to form a weaker acid.
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Answer:
NaCl + KNO3 --> NaNO3+ KCl
During double replacement, the cations and anions of two different compounds switch places.
K2SO4 +2 NaNO3 >> Na2SO4 + 2 KNO3
2KCl + Li2SO4 >> K2SO4 + 2 LiCl
3NaBr + K3PO4 >> Na3PO4 + 3 KBr
3 CaS + 2 K3PO4 >> Ca3(PO4)2 + 3 K2S
2 AgNO3 + Na2SO4 >> Ag2SO4 + 2 NaNO3
CuSO4 + ZnCl 2 -->CuCl2 + ZnSO4
A typical double replacement reaction can occur when two ionic compounds are mixed together.� In water these ionic compounds split apart into their respective anions and cations.� The cations now have an opportunity to swap anions.� A reaction occurs if , by swapping anions, a product is formed that cannot split apart into anions and cations.� Look at the following example:� the reaction of silver nitrate and potassium chloride.�� The silver, nitrate, potassium and chloride ions all begin in solution.� When a silver ion combines with a chloride ion, it leaves the solution and becomes a solid.� This drives the reaction to completion!!!
AgNO3(aq) + KCl(aq)� ‑‑‑‑>� AgCl(s) + KNO3(aq)
The reaction must be driven by one of three driving forces:� Formation of a solid, formation of a gas or formation of a weakly‑ionizing compound such as water.� Lets look to see what happens when the driving forces are not there.�
NaNO3(aq) + KCl(aq)� ‑‑X‑‑>� NaCl(aq) + KNO3(aq)
Nothing happens!!� Without a driving force there is no change in the solution so we say no reaction has taken place.� Note that even though we can write an equation for the reaction, no reaction takes place without a driving force!!
How can we tell if an ionic compound will be soluble in water?� There are a series of guidelines in your book.� On the next page I provide you with another presentation of these same rules:
Solubility Rules
1.� All compounds containing Na+, K+,� or NH4+ ions are soluble in water.
2. �All nitrates (NO3‑) are soluble in water.
3.� Most chlorides (Cl‑ ), and sulfates (SO42‑) are soluble.� Some important exceptions are silver chloride (AgCl), barium sulfate (BaSO4), and lead sulfate (PbSO4) which are insoluble.
4.� Most carbonates (CO32‑), phosphates (PO43‑), sulfides (S2‑), and hydroxides (OH‑) are insoluble in water.� Important exceptions are those of Na+, K+,� and NH4+, as well as barium hydroxide, Ba(OH)2.�
������������������������������...
How do you know if a gas will form?� If H2CO3 is formed it will form a gas by decomposing to H2O and CO2.� You will see that in this lab.� Other compounds that release water or a gas are
NH4OH and H2SO3.
When an strong acid and a strong base react, in an aqueous solutions, they produce a salt and water.� This is an example of a double displacement reaction where the driving force is the formation of the covalent compound water.� Often, the only way to tell if one of these reactions has occurred is by looking for the formation of heat or by using an acid/base indicator to tell if the base has neutralized the acid.� If you do not see a reaction occurring you may wish to ask your instructor for an appropriate indicator.�� (How can you tell what the color of the indicator will be in an acidic solution and a basic solution?� Answer:� Test the solutions individually.)�
Procedure
There are ten stations.� Please use the standard procedure at each station.
I.� Reacting CuSO4 solution with NaOH solution.
II.� Reacting Na2CO3 solution with HCl solution.
III.� Reacting KCl solution with Na2CO3 solution.
IV.� Reacting Na2SO4 solution with BaCl2 solution.
V.� Reacting NaOH solution with HCl solution.� (Use phenolphthalein indicator)
VI.� Reacting Na2CO3 solution with CaCl2 solution.
VII.� Reacting Ni(NO3)2 solution with NaOH solution.
VIII. Reacting Na2SO4 solution with Cu(N03)2 solution.
IX.� Reacting KOH solution with MgCl2 solution.
X.� Reacting NaHCO3 solution with HNO3 solution.
Standard procedure
1.�������� Transfer 10‑15 drops of one solution into test tube.� Record in your notebook a description of the appearance of the first solution.
2.�������� Record in your notebook your description of the second solution.
3.�������� Using a Beral pipet, add 10‑15 drops of the second solution to the test tube.� Record in your notebook your description of the appearance of the reaction mixture.� Dispose of waste appropriately,�
4.�������� a.� Write in your notebook a complete, molecular equation, including states.
b.� Write in your notebook the driving force and make sure that the equation is balanced.
Purpose:� To observe double replacement reactions
Procedure:� As stated in lab handout and as presented by the instructor.� All reagents had a concentration of 1 M.
Conclusion:� In all of the double replacement reactions where a chemical reaction took place, the reaction was driven by one of these driving forces: formation of a gas, formation of a solid,� formation of a water, or the reaction in which a strong acid reacts to form a weaker acid.
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