How do you write a complete balanced reaction of aqueous lead (II) nitrate, $P b {(N O_{3})}_{2}$ $Pb(NO_3)_2$ , and aqueous potassium chloride, $K C L$ $KCL$ ?

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How do you write a complete balanced reaction of aqueous lead (II) nitrate, $P b {(N O_{3})}_{2}$ $Pb(NO_3)_2$ , and aqueous potassium chloride, $K C L$ $KCL$ ?

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Answer 1 · 2015-12-01T16:25:05

$P b {(N O_{3})}_{2} (a q) + 2 K C l (a q) \to P b C l_{2} (s) ⏐ ↓ + 2 K N O_{3} (a q)$ $Pb(NO_3)_2(aq) + 2KCl(aq) rarr PbCl_2(s)darr + 2KNO_3(aq)$

Explanation:

How did I know that $P b C l_{2}$ $PbCl_2$ was insoluble? Chemistry is an experimental science and this is something that you must learn. All halides are soluble, EXCEPT for lead(II) chloride, mercurous chloride ( $H g_{2} C l_{2}$ $Hg_2Cl_2$ ), and silver chloride, $A g C l$ $AgCl$ .

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How do you write a complete balanced reaction of aqueous lead (II) nitrate, $P b {(N O_{3})}_{2}$ $Pb(NO_3)_2$ , and aqueous potassium chloride, $K C L$ $KCL$ ?

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How do you write a complete balanced reaction of aqueous lead (II) nitrate, Pb(NO_3)_2Pb(NO3)2Pb(NO_3)_2, and aqueous potassium chloride, KCLKCLKCL?

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How do you write a complete balanced reaction of aqueous lead (II) nitrate, $P b {(N O_{3})}_{2}$ $Pb(NO_3)_2$ , and aqueous potassium chloride, $K C L$ $KCL$ ?