A double replacement reaction occurs when aqueous potassium iodide and aqueous mercury (I) nitrate are mixed. What is the correct balanced chemical equation for this reaction? (1 point) KI(aq) + HgNO3 (aq) yields KHg(aq) + INO3(s) KI(aq) + HgINO3 (aq) yields KNO3 (aq) + Hg(s) KI2 (aq) + HgNO3 (aq) yields KNO3 (aq) + HgI2 (s) KI(aq) + Hg2NO3 (aq) yields KNO3(aq) + Hg2I(s)

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A double replacement reaction occurs when aqueous potassium iodide and aqueous mercury (I) nitrate are mixed. What is the correct balanced chemical equation for this reaction? (1 point) KI(aq) + HgNO3 (aq) yields KHg(aq) + INO3(s) KI(aq) + HgINO3 (aq) yields KNO3 (aq) + Hg(s) KI2 (aq) + HgNO3 (aq) yields KNO3 (aq) + HgI2 (s) KI(aq) + Hg2NO3 (aq) yields KNO3(aq) + Hg2I(s)

Chemistry
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i think it is the third option
I feel like it should be this but its not one of your options: KI(aq) + HgNO3(aq) → KNO3(aq) + HgI(s) But it could be option two if you just have the I in the wrong spot for some reason

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hmm. i'm confused on this one
K has a charge of +1, I has a charge of -1, Hg will have a charge of +1 as it specified it in the question and NO3 has a charge of -1. So there should be no 2s involved anywhere in the formula K can't bond with Hg and NO3 can't bond with I
is the first option possible?
KHg i dont think exist
I searched it up to see if someone else has ever asked this question on anything and they answered with the first one but I really don't think thats right K and Hg don't bond normally and NO3 and I don't normally bond either
i think i should go with the third one
I eliminated a and b out
C makes the most sense. The true answer isnt here tho.
Ya what @sweetburger says makes sense even though overall it doesn't make sense either lol
Lol thanks you guys! :) :DD

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