QUESTION IMAGE
Question
analysis and conclusions
- for each case in which you found a reaction occurred, write the correct formula for the substance formed. in those cases where no reaction occurred, mark nr (no reaction)
- for each formula write the correct chemical name for the compound formed. in those cases where no reaction occurred, mark nr (no reaction).
Step1: Recall solubility rules
Use solubility rules to determine if a reaction occurs and the product formed. For example, when a metal - ion reacts with an anion, if the resulting compound is insoluble, a reaction occurs.
Step2: Analyze each combination
For $Co(NO_3)_2$ and $K_3PO_4$
The reaction is $3Co(NO_3)_2 + 2K_3PO_4=Co_3(PO_4)_2\downarrow+6KNO_3$. The product is $Co_3(PO_4)_2$ (cobalt(II) phosphate).
For $Co(NO_3)_2$ and $KOH$
$Co(NO_3)_2 + 2KOH = Co(OH)_2\downarrow+2KNO_3$. The product is $Co(OH)_2$ (cobalt(II) hydroxide).
For $Co(NO_3)_2$ and $K_4Fe(CN)_6$
$3Co(NO_3)_2+2K_4Fe(CN)_6 = Co_3[Fe(CN)_6]_2\downarrow + 6KNO_3$. The product is $Co_3[Fe(CN)_6]_2$ (cobalt(II) hexacyanoferrate(II)).
For $Co(NO_3)_2$ and $K_2CO_3$
$Co(NO_3)_2+K_2CO_3 = CoCO_3\downarrow+2KNO_3$. The product is $CoCO_3$ (cobalt(II) carbonate).
For $Co(NO_3)_2$ and $KI$
$Co(NO_3)_2 + 2KI=CoI_2 + 2KNO_3$. Since $CoI_2$ is soluble, NR (no reaction).
For $Co(NO_3)_2$ and $K_2C_2O_4$
$Co(NO_3)_2+K_2C_2O_4 = CoC_2O_4\downarrow+2KNO_3$. The product is $CoC_2O_4$ (cobalt(II) oxalate).
Repeat this process for all the metal - ion and anion combinations.
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| $K_3PO_4$ | $KOH$ | $K_4Fe(CN)_6$ | $K_2CO_3$ | $KI$ | $K_2C_2O_4$ | |
|---|---|---|---|---|---|---|
| $Pb(NO_3)_2$ | $Pb_3(PO_4)_2$ | $Pb(OH)_2$ | $Pb_2[Fe(CN)_6]$ | $PbCO_3$ | $PbI_2$ | $PbC_2O_4$ |
| $CuSO_4$ | $Cu_3(PO_4)_2$ | $Cu(OH)_2$ | $Cu_2[Fe(CN)_6]$ | $CuCO_3$ | $CuI$ (with oxidation - reduction side - reaction possible, but mainly NR) | $CuC_2O_4$ |
| $Fe(NO_3)_3$ | $FePO_4$ | $Fe(OH)_3$ | $Fe_4[Fe(CN)_6]_3$ | $Fe_2(CO_3)_3$ | NR | $Fe_2(C_2O_4)_3$ |
| $Ni(NO_3)_2$ | $Ni_3(PO_4)_2$ | $Ni(OH)_2$ | $Ni_2[Fe(CN)_6]$ | $NiCO_3$ | NR | $NiC_2O_4$ |
| $Sr(NO_3)_2$ | $Sr_3(PO_4)_2$ | $Sr(OH)_2$ (soluble in large amounts of water, but may precipitate in concentrated solutions) | $Sr_2[Fe(CN)_6]$ | $SrCO_3$ | NR | $SrC_2O_4$ |
| $AgNO_3$ | $Ag_3PO_4$ | $AgOH$ (which decomposes to $Ag_2O$) | $Ag_4[Fe(CN)_6]$ | $Ag_2CO_3$ | $AgI$ | $Ag_2C_2O_4$ |
| $K_3PO_4$ | $KOH$ | $K_4Fe(CN)_6$ | $K_2CO_3$ | $KI$ | $K_2C_2O_4$ | |
|---|---|---|---|---|---|---|
| $Pb(NO_3)_2$ | Lead(II) phosphate | Lead(II) hydroxide | Lead(II) hexacyanoferrate(II) | Lead(II) carbonate | Lead(II) iodide | Lead(II) oxalate |
| $CuSO_4$ | Copper(II) phosphate | Copper(II) hydroxide | Copper(II) hexacyanoferrate(II) | Copper(II) carbonate | NR | Copper(II) oxalate |
| $Fe(NO_3)_3$ | Iron(III) phosphate | Iron(III) hydroxide | Iron(III) hexacyanoferrate(II) | Iron(III) carbonate | NR | Iron(III) oxalate |
| $Ni(NO_3)_2$ | Nickel(II) phosphate | Nickel(II) hydroxide | Nickel(II) hexacyanoferrate(II) | Nickel(II) carbonate | NR | Nickel(II) oxalate |
| $Sr(NO_3)_2$ | Strontium phosphate | Strontium hydroxide | Strontium hexacyanoferrate(II) | Strontium carbonate | NR | Strontium oxalate |
| $AgNO_3$ | Silver phosphate | Silver oxide (from decomposition of $AgOH$) | Silver hexacyanoferrate(II) | Silver carbonate | Silver iodide | Silver oxalate |