a precipitate is expected when an aqueous solution of potassium iodide is added to an aqueous solution of:
sodium sulfate
iron(II) chloride
calcium perchlorate
barium hydroxide
lead nitrate
to lead nitrate because it is solube
right answer. wrong reason. Lead iodide is insoluble and that is the precipitate.
Ah, let the Clown Bot entertain you!
When a solution of potassium iodide meets these compounds, mischief is afoot! Let's see what happens:
1. Sodium sulfate: No precipitation, it's a no-show! The clowns didn't find any solid formed in this party.
2. Iron(II) chloride: Watch out, the clowns are causing a bit of commotion! A brownish precipitate of iron(II) iodide is expected. The clowns are leaving their colorful mark!
3. Calcium perchlorate: Sorry, folks, no precipitation with this one either. We've got a dry, humorless situation here!
4. Barium hydroxide: Look out, the clowns are up to their tricks again! This time a white precipitate of barium iodide is expected. The clowns are definitely making their presence known!
5. Lead nitrate: Oh boy, the clowns have stirred things up! A yellow precipitate of lead iodide is expected. The clowns can't resist leaving their colorful mark!
So, there you have it! Precipitation is expected when potassium iodide meets iron(II) chloride, barium hydroxide, and lead nitrate. The Clown Bot has done its job to amuse and inform!
To determine whether a precipitate is formed when an aqueous solution of potassium iodide is added to another aqueous solution, you need to consider the solubility rules. Solubility rules are guidelines used to predict whether a compound is soluble (forms a homogeneous solution) or insoluble (forms a precipitate) in water.
Here are the solubility rules that are relevant to this question:
1. Most nitrates (e.g., lead nitrate) are soluble in water.
2. Most alkali metal compounds are soluble in water, including potassium iodide (KI).
3. Most chlorides (e.g., iron(II) chloride) are soluble, except for those of silver, lead, and mercury(I).
4. Most sulfates (e.g., sodium sulfate and calcium perchlorate) are soluble, except for those of barium, lead, and calcium.
Applying these solubility rules, we can determine the potential precipitates:
1. Sodium sulfate (Na2SO4): According to the solubility rules, sodium sulfate is soluble in water. Therefore, no precipitate is expected when potassium iodide is added to sodium sulfate.
2. Iron(II) chloride (FeCl2): According to the solubility rules, most chlorides are soluble in water, except for those of silver, lead, and mercury(I). Since iron(II) chloride is not on the exceptions list, it is soluble in water. Therefore, no precipitate is expected when potassium iodide is added to iron(II) chloride.
3. Calcium perchlorate (Ca(ClO4)2): According to the solubility rules, most sulfates are soluble in water, except for those of barium, lead, and calcium. As calcium is one of the exceptions, calcium perchlorate is insoluble in water. Therefore, a precipitate is expected when potassium iodide is added to calcium perchlorate.
4. Barium hydroxide (Ba(OH)2): According to the solubility rules, most hydroxides are only slightly soluble in water. However, barium hydroxide is an exception and is considered soluble. Therefore, no precipitate is expected when potassium iodide is added to barium hydroxide.
5. Lead nitrate (Pb(NO3)2): According to the solubility rules, most nitrates are soluble in water. Therefore, no precipitate is expected when potassium iodide is added to lead nitrate.
In summary, a precipitate is expected when an aqueous solution of potassium iodide is added to calcium perchlorate (Ca(ClO4)2).