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Choose the correct products for the double replacement reaction below. Click here to access the solubility rules to determine which product, if any, forms a solid precipitate in the reaction.

PbCl2 + MgSO4Upper C subscript 3 upper H subscript 8 plus upper O subscript 2 right arrow. ?

Pb + O2 + MgCl

PbMg + ClSO4
PbSO4 + MgCl2

Pb(SO4)2 + MgCl
Which product in the reaction forms a precipitate?
PbSO4

MgCl2

PbMg

no precipitate formed

Choose the correct products for the double replacement reaction below Click here to access the solubility rules to determine which product if any forms a solid class=


Answer :

elvokipkorir

Answer:

Overall equation:

PbCl2 + MgSO4 => PbSO4 + MgCl2

Products:

PbSO4 + MgCl2

PbSO4 is a white precipitate (solid)

Explanation:

The reaction between PbCl2 and MgSO4 yields PbSO4 and MgCl2. PbSO4 is evidenced by formation of a white precipitate in the product side. The white precipitate is therefore, PbSO4. MgCl2 Formed is in aqueous state.

PbCl2(aq) + MgSO4(aq) => PbSO4 (s) + MgCl2(aq)

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