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    Asoom's Avatar
    Asoom Posts: 52, Reputation: 1
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    #1

    Apr 20, 2009, 12:58 PM
    Write the balance equation
    I tried to solve my homework , but I face some problem Im not sure about it and another I can't solve it..


    Im not sure about the solve , could you check if it is right or wrong

    1- (Salt + dil. HCl) with Carbonate

    CO3^2- + 2HCl -----> CO2 + H2O+ 2Cl^-


    2- (Solution + HgCl2) with Crbonate

    CO3^2- + HgCl2 -----> HgCO3 + 2Cl^-


    3- (Solution +MgSO4) with Crbonate

    CO3^2- + MgSO4 -----> MgCO3 + SO4^2-


    4- (Salt + dil. HCl) with Bicarbonate

    HCO3^2- + HCl -----> CO2 + H2O+ Cl^-


    5- (Solution +HgCl2) with Bicarbonate

    HCO3^2- + HgCl2 -----> HgCO3 + HCl


    6- (Solution +MgSO4) with Bicarbonate

    HCO3^2- + MgSO4-----> MgCO3+ HSO4


    7- (Salt + dil. HCl) with Nitrite

    NO2^- + HCl -----> HNO3 + Cl


    8- (Solution +AgNO3) with Nitrite

    NO2^- + AgNO3 -----> AgNO2 + NO3



    I can't solve it

    1- (Solution + acidified KMnO4) with Nitrite
    2- (Salt + dil. HCl) with thiosulphate
    3- (Solution +AgNO3) with thiosulphate
    4- (Solution + acidified KMnO4) with thiosulphate
    Perito's Avatar
    Perito Posts: 3,139, Reputation: 150
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    #2

    Apr 20, 2009, 01:37 PM
    1- (Salt + dil. HCl) with Carbonate


    Correct.

    2- (Solution + HgCl2) with Crbonate


    Correct

    3- (Solution +MgSO4) with Crbonate


    Correct

    4- (Salt + dil. HCl) with Bicarbonate


    Almost correct It's HCO3^- not HCO3^2-. There's one negative charge, not 2.

    5- (Solution +HgCl2) with Bicarbonate


    You were missing one chlorine and one negative charge.

    6- (Solution +MgSO4) with Bicarbonate


    Again, bicarbonate has only one charge. Bisulfate also has a -1 charge.

    7- (Salt + dil. HCl) with Nitrite


    You must also make sure the charge is balanced.

    8- (Solution +AgNO3) with Nitrite


    Again, balance charge.


    1- (Solution + acidified KMnO4) with Nitrite
    This is an oxidation-reduction reaction. Nitrite is oxidized, Permanganate is reduced.

    2- (Salt + dil. HCl) with thiosulphate
    Thiosulfate decomposes in acid solution to form SO2 and sulfur.

    3- (Solution +AgNO3) with thiosulphate
    Forms silver thiosulfate.

    4- (Solution + acidified KMnO4) with thiosulphate
    thiosulfate is a reducing agent, permanganate is an oxidizing agent. The thiosulfate will be oxidized, the permanganate will be reduced.

    Try to figure out these last 4 with the hints I've given you.
    Asoom's Avatar
    Asoom Posts: 52, Reputation: 1
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    #3

    Apr 20, 2009, 10:18 PM

    Ok , I will try after my classes finish today

    Thanks a lot
    Asoom's Avatar
    Asoom Posts: 52, Reputation: 1
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    #4

    Apr 21, 2009, 12:32 PM

    1- NO2^- + KMnO4 ------> KNO2 + MnO4

    2- S2O3^2- + 2HCl ------> SO2 + S + Cl^- + H2O

    3- S2O3^2- + 2AgNO3 ------> Ag2S +2NO3


    the last one I can't solve it
    I wait your checking


    (salt + conc H2SO4)

    4I^- + H2SO4 -------> I2 + 2HI + SO4
    could you check also this equation
    Perito's Avatar
    Perito Posts: 3,139, Reputation: 150
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    #5

    Apr 21, 2009, 01:11 PM

    NO2(-) is oxidized to NO3(-). MnO4- is reduced either to MnO2 or to Mn(2+) or occasionally to MnO4(-2). I haven't balanced this and you might need water, acid, or base to do so.
    Permanganate - Wikipedia, the free encyclopedia

    Balancing by half reactions




    Multiply the first equation by 2 and add to the second equation



    That should be balanced.


    looks right.


    I think you just form silver thiosulfate. I don't think the thiosulfate is strong enough to reduce the silver. If it does, it will form metallic silver.

    (salt + conc H2SO4)


    There's no oxidation. Sulfuric acid is not an oxidizer so you can't oxidize I- to I2.
    In fact, you'll have an equilibrium with "bisulfate" and "sulfate":

    Asoom's Avatar
    Asoom Posts: 52, Reputation: 1
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    #6

    Apr 21, 2009, 10:03 PM

    Thanks a lot , your explanation was very strong and clear..

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