A-Level Chemistry 1B Precipitation_1

What is a precipitation reaction?

• a) A reaction that occurs between two gases

• b) A reaction that occurs in solid-state only

• c) A reaction that occurs in aqueous solutions where two ionic bonds combine forming insoluble salts

• d) A reaction that occurs in organic solvents

One way to test for carbon dioxide gas that's ​ (a)   is that we bubble it through lime water. ​ (b)   is an aqueous solution of calcium hydroxide ​ (c)  

So here i'm breathing through this tube and you see the bubbles coming up through the ​ (d)   solution. So let's see if i can do this all in one breathe

• co2
• lime water
• Ca(OH)2.
• calcium hydroxide
• Oxygen

if I can have this carbon dioxide and calcium hydroxide react to form that ​ (a)   . if you look at the reaction, you can see we have​ (b)   ) + Ca(OH)2 (aq) →​ (c)   +H2O that's the precipitate, and eventually that's what will change the solution to the ​ (d)   and

that's the test for ​ (e)   .

• milky white precipitate
• CaCO2 (g
• CaCO3 (s)
• milky white color
• carbon dioxide

Lead Nitrate and Potassium Iodide Precipitate reaction; gold rain experiment involves the​ (a)   between lead nitrate (Pb(NO3)2) and ​ (b)   , which results in the formation of a ​ (c)   . The term "gold rain" is often used to describe the appearance of the ​ (d)   , which has a ​ (e)   .

When lead nitrate and potassium iodide are mixed together, a double displacement reaction occurs. The lead ions (Pb2+) from lead nitrate react with the iodide ions (I-) from potassium iodide to form lead iodide (PbI2), which is insoluble in water and precipitates out. The balanced chemical equation for the reaction is as follows:

Pb(NO3)2 + 2KI → PbI2 + 2KNO3

The golden-yellow precipitate of lead iodide gives the appearance of "gold rain" when it forms in the solution. This reaction is often used as a demonstration in chemistry experiments to observe the formation of a colored precipitate.

• reaction
• potassium iodide (KI)
• precipitate
• resulting precipitate
• golden-yellow color

Lead Nitrate and Potassium Iodide Precipitate reaction; gold rain experiment involves the reaction between lead nitrate (Pb(NO3)2) and potassium iodide (KI), which results in the formation of a precipitate. The term "gold rain" is often used to describe the appearance of the resulting precipitate, which has a golden-yellow color.

When ​ (a)   and potassium iodide are mixed together, a ​ (b)   occurs. The ​ (c)   (Pb2+) from lead nitrate react with the ​ (d)   (I-) from potassium iodide to form​ (e)   (PbI2), which is insoluble in water and precipitates out. The balanced chemical equation for the reaction is as follows:

Pb(NO3)2 + 2KI → PbI2 + 2KNO3

The golden-yellow precipitate of lead iodide gives the appearance of "gold rain" when it forms in the solution. This reaction is often used as a demonstration in chemistry experiments to observe the formation of a colored precipitate.

• lead nitrate
• double displacement reaction
• lead ions
• iodide ions
• lead iodide

Lead Nitrate and Potassium Iodide Precipitate reaction; gold rain experiment; involves the reaction between lead nitrate (Pb(NO3)2) and potassium iodide (KI), which results in the formation of a precipitate. The term "gold rain" is often used to describe the appearance of the resulting precipitate, which has a golden-yellow color.

When lead nitrate and potassium iodide are mixed together, a double displacement reaction occurs. The lead ions (Pb2+) from lead nitrate react with the iodide ions (I-) from potassium iodide to form lead iodide (PbI2), which is insoluble in water and ​ (a)   . The balanced chemical equation for the reaction is as follows:

​ (b)   + 2KI → PbI2 + 2KNO3

The golden-yellow precipitate of​ (c)   gives the appearance of "gold rain" when it forms in the solution. This reaction is often used as a demonstration in chemistry experiments to observe the formation of a ​ (d)   .

• precipitates out
• Pb(NO3)2
• lead iodide
• colored precipitate

One way to test for ​ (a)   gas that's Co2 is we bubble it through ​ (b)   . Lime water is an ​ (c)   of calcium hydroxide ​ (d)   . So here I'm breathing through this tube and you see the ​ (e)   coming up through the calcium hydroxide solution. So let's see if I can do this all in one breath. If I can have this carbon dioxide and calcium hydroxide react to form that milky white precipitate.

• carbon dioxide
• lime water
• aqueous solution
• Ca(OH)2
• bubbles

So here i'm breathing through this tube

and you see the bubbles coming up through the ​ (a)   . So let's see if I can do this all in one breath. If I can have this ​ (b)  

and calcium hydroxide​ (c)   to form that ​ (d)   .

• calcium hydroxide solution
• carbon dioxide
• reacts
• milky white precipitate

If you look at the ​ (a)   you can see we have: ​ (b)   +Ca(OH)2 ⟶> CaCO3 + H2O and in the products we have ​ (c)   (solid calcium carbonate) that's the ​ (d)   and eventually, that's what will change the ​ (e)   to the milky white color and that's the test for carbon dioxide.

• reactants
• CO2
• CaCO3
• precipitate
• solution

you can see that initially we had a liquid that was clear. So we're starting to see that ​ (a)   that​ (b)   that is precipitating out. And here just right here is when I would say we definitively have passed the test for ​ (c)   We have that milky white precipitate this is Dr B with a test for​ (d)   using lime water. Thanks for watching.

• milky white precipitate
• calcium carbonate solid
• carbon dioxide gas.
• CO2 (carbon dioxide) gas