All the equations represent a double replacement reaction . Therefore the products would get formed by exchange of either positive ions or negative ions.
#5
Lead (II) acetate + Sodium Hydroxide solution
CME : Pb(C2H3O2)2 (aq) + 2 NaOH (aq) ----------------> Pb(OH)2 (s) + 2 NaC2H3O2 (aq) ...........[Using solubility rules, we can predict that Pb(OH)2 would be solid ]
To balance the equation, we add 2 before NaC2H3O2 and NaOH
CIE : for complete ionic equation, we will separate those substance which are in (aq) state
Pb+2 (aq) + 2 C2H3O2 -1 (aq) + 2 Na + (aq) + 2 OH - (aq) ----------> Pb(OH)2 (s) + 2 Na + (aq) + 2 C2H3O2 - (aq)
NIE : For net ionic equation, we will cancel out the common ions on both sides
Pb +2 (aq) + 2 OH- (aq) -------------------> Pb(OH)2 (s)
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#6
Lead (II) acetate + Aq. ammonia solution
Aq. ammonia solution is NH3 in water which can also be written as NH4OH
NH3 + H2O <------> NH4OH (aq)
CME : Pb(C2H3O2)2 (aq) + 2 NH4OH (aq) ----------------> Pb(OH)2 (s) + 2 NH4C2H3O2 (aq) ..........[Using solubility rules, we can predict that Pb(OH)2 would be solid ]
To balance the equation, we add 2 before NH4C2H3O2 and NH4OH
CIE : for complete ionic equation, we will separate those substance which are in (aq) state
Pb+2 (aq) + 2 C2H3O2-1 (aq) + 2 NH4+ (aq) + 2 OH - (aq) -------> Pb(OH)2 (s) + 2 NH4+ (aq) + 2 C2H3O2 - (aq)
NIE : For net ionic equation, we will cancel out the common ions on both sides
Pb+2 (aq) + 2 OH - (aq) --------> Pb(OH)2 (s)
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#7
Cobalt (II) nitrate solution + Sodium carbonate solution
CME : Co(NO3)2 (aq) + Na2CO3 (aq) ----------------> CoCO3 (s) + 2 NaNO3(aq) ........[Using solubility rules, we can predict that CoCO3 would be solid ]
To balance the equation, we add 2 before NaNO3
CIE : for complete ionic equation, we will separate those substance which are in (aq) state
Co +2 (aq) + 2 NO3 - (aq) + 2 Na + (aq) + CO3 -2 (aq) ----------------> CoCO3 (s) + 2 Na + (aq) + 2 NO3 - (aq)
NIE : For net ionic equation, we will cancel out the common ions on both sides
Co +2 (aq) + CO3-2(aq) ----------------> CoCO3 (s)
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#8
Cobalt (II) nitrate solution + Sulfuric acid solution
CME : Co(NO3)2 (aq) + H2SO4 (aq) ----------------> CoSO4 (s) + 2 HNO3(aq) ........[Using solubility rules, we can predict that CoSO4 would be solid ]
To balance the equation, we add 2 before HNO3
CIE : for complete ionic equation, we will separate those substance which are in (aq) state
Co +2 (aq) + 2 NO3 - (aq) + 2 H + (aq) + SO4 -2 (aq) ----------------> CoSO4 (s) + 2 Na + (aq) + 2 NO3 - (aq)
NIE : For net ionic equation, we will cancel out the common ions on both sides
Co +2 (aq) + SO4 -2(aq) ----------------> CoSO4 (s)
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#9
Cobalt (II) nitrate solution + Aq. ammonia solution.
As described earlier, aq. ammonia is NH4OH (aq)
CME : Co(NO3)2 (aq) + 2 NH4OH (aq) ----------------> Co(OH)2 (s) + 2 NH4NO3(aq) .......[Using solubility rules, we can predict that Co(OH)2 would be solid ]
To balance above equation, we add 2 before NH4OH and NH4NO3
CIE : for complete ionic equation, we will separate those substance which are in (aq) state
Co +2 (aq) + 2 NO3 - (aq) + 2 NH4+ (aq) + 2 OH - (aq) ---------> Co(OH)2 (s) + 2 NH4+ (aq) + 2 NO3 - (aq)
NIE : For net ionic equation, we will cancel out the common ions on both sides
Co +2 (aq) + 2 OH - (aq) --------------> Co(OH)2 (s)
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#10
Ammonium acetate solution + Sodium hydroxide solution
In this reaction NH4OH is formed as one of the products . NH4OH is very unstable and dissociates into NH3 gas and water . The reaction is written below.
CME : NH4C2H3O2 (aq) + NaOH (aq) --------------> NH3 (g) + H2O (l) + NaC2H3O2 (aq)
CIE : for complete ionic equation, we will separate those substance which are in (aq) state
NH4 + (aq) + C2H3O2 - (aq) + Na + (aq) + OH - (aq) --------> NH3(g) + H2O (l) + Na + (aq) C2H3O2 - (aq)
NIE : For net ionic equation, we will cancel out the common ions on both sides
NH4 +(aq) + OH -(aq) --------> NH3(g) + H2O (l)
Lead(II) acetate + sodium hydroxide solution Lead(II) acetate + aqueous ammonia solution Cobalt(II) nitrate solution +...
A solution contains 1.95×10-2 M nickel(II) nitrate and 1.95×10-2 M cobalt(II) acetate. Solid sodium carbonate is added slowly to this mixture. What is the concentration of cobalt(II) ion when nickel ion begins to precipitate?
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Write formula for compounds
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cobalt(II) acetate. A solution contains 7.85X10M calcium nitrate and 8.21x10M Solid sodium sulfide is added slowly to this mixture. What is the concentration of cobalt(II)ion when calcium ion begins to precipitate? [Co2+]=1 M Submit Answer Retry Entire Group 9 more group attempts remaining