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eistein+newton+gallileo=_me

  • 4 years ago

how many litres of 0.500M HCL(aq) are needed to react completely with 0.100 mol of Pb(NO3)2, forming a precipitate of PbCl2(s)...please explain

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  1. sgeos
    • 4 years ago
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    Start by balancing your equation. (Note that the H and Pb switch places.)\[2HCl(aq)+Pb(NO_3)_2(aq) \rightarrow PbCl_2(s)+2HNO_3(aq)\] From there, figure out how many mol of HCl you need to react completely with 0.100 mol of Pb(NO3)2. After that, figure out how many liters of solution that works out to at 0.500M HCl.

  2. eistein+newton+gallileo=_me
    • 4 years ago
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    lol i tried that and it failed

  3. sgeos
    • 4 years ago
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    Where did you go wrong?

  4. hakkunamatata
    • 4 years ago
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    1M of HCl can react with0.5M of Pb(NO3)2 to produce 0.5M of PbCl2 1 L of HCl contains 0.5 M, 2 L of HCl contains 1M of HCl 1 M of HCl react with 0.5M of Pb(NO3)2 How many Mole of HCl needed to react with 0.1 M of Pb(NO3)2 to complete the reaction= 1/5Mof HCl =0.2 M of HCl 0.2M of HCl in how many Litres of HCl=0.4 litre not sure..........of ans.........hope it is true....

  5. sgeos
    • 4 years ago
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    That looks right to me.

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