What halide salts are insoluble?
This illustrates a general phenomenon of aqueous solubility......
And we must able to reproduce the reactions.....
In all cases both charge and mass are conserved, as they must be if we are to represent chemical reality.
In the case of the silver halides, in particular, this reaction gives silver chloride as a very curdy white solid from aqueous solution; silver bromide as a cream solid; and silver iodide as a yellow solid.
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Here's what I got.
Start by writing the chemical formulas of the reactants and of the products.
#"lead(II) nitrate " -> " Pb"("NO"_3)_2# #"potassium iodide " -> " KI"# #"lead(II) iodide " -> " PbI"_2# #"potassium nitrate " -> " KNO"_3# Now, your reaction takes place in aqueous solutions. Three of the four chemical species involved in the reaction will be in the aqueous state,
#"(aq)"# , and one, potassium iodide, will be in the solid state,#"(s)"# .The unbalanced chemical equation looks like this
#"Pb"("NO"_ 3)_ (2(aq)) + "KI"_ ((aq)) -> "PbI"_ (2(s)) darr + "KNO"_ (3(aq))# To balance this chemical equation, multiply the potassium iodide by
#2# and the potassium nitrate by#2# .You will end up with
#"Pb"("NO"_ 3)_ (2(aq)) + 2"KI"_ ((aq)) -> "PbI"_ (2(s)) darr + 2"KNO"_ (3(aq))# If you want, you can write the complete ionic equation by breaking up the soluble compounds, i.e. the ones that are in the aqueous state, into their respective cations and anions
#"Pb"_ ((aq))^(2+) + 2"NO"_ (3(aq))^(-) + 2"K"_ ((aq))^(+) + 2"I"_ ((aq))^(-) -> "PbI"_ (2(s)) darr + 2"K"_ ((aq))^(+) + 2"NO"_ (3(aq))^(-)# If you eliminate the spectator ions, i.e. the ions that are present on both sides of the equation
#"Pb"_ ((aq))^(2+) + color(red)(cancel(color(black)(2"NO"_ (3(aq))^(-)))) + color(red)(cancel(color(black)(2"K"_ ((aq))^(+)))) + 2"I"_ ((aq))^(-) -> "PbI"_ (2(s)) darr + color(red)(cancel(color(black)(2"K"_ ((aq))^(+)))) + color(red)(cancel(color(black)(2"NO"_ (3(aq))^(-))))# you will get the net ionic equation
#"Pb"_ ((aq))^(2+) + 2"I"_ ((aq))^(-) -> "PbI"_ (2(s)) darr# Lead(II) iodide is a yellow insoluble solid that precipitates out of the solution.
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Silver chloride (AgCl), lead(II) chloride (PbCl2), and mercury(I) chloride (Hg2Cl2) are examples of insoluble halide salts.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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