Math

QuestionWhich of the following would be a precipitate when the following aqueous solutions are mixed: Pb(NO3)2\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2} and KI INO3\mathrm{INO}_{3} PbI2\mathrm{PbI}_{2} KNO3\mathrm{KNO}_{3} PbK2\mathrm{PbK}_{2}

Studdy Solution

STEP 1

1. We are dealing with an aqueous reaction between Pb(NO3)2\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2} and KI\mathrm{KI}.
2. We need to identify the precipitate formed from the reaction.
3. We assume knowledge of solubility rules to determine the precipitate.

STEP 2

1. Write the balanced chemical equation for the reaction.
2. Apply solubility rules to determine which products, if any, are insoluble.
3. Identify the precipitate from the reaction.

STEP 3

Write the balanced chemical equation for the reaction:
Pb(NO3)2(aq)+2KI(aq)PbI2(s)+2KNO3(aq)\mathrm{Pb}\left(\mathrm{NO}_{3}\right)_{2} (aq) + 2\mathrm{KI} (aq) \rightarrow \mathrm{PbI}_{2} (s) + 2\mathrm{KNO}_{3} (aq)

STEP 4

Apply solubility rules to determine which products are insoluble:
- PbI2\mathrm{PbI}_{2} is generally insoluble in water. - KNO3\mathrm{KNO}_{3} is soluble in water.

STEP 5

Identify the precipitate from the reaction:
Since PbI2\mathrm{PbI}_{2} is insoluble in water, it will precipitate out of solution.
The precipitate formed is:
PbI2 \boxed{\mathrm{PbI}_{2}}

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