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    calculate the volume of 1.20M hydrochloric acid which is required to neutralise exactly the barium oxide formed by decomposition of 5.00g of barium nitrate. Barium oxide reacts with hydrochloric acid as follows

    Ba0 + 2HCL - BaCl2 + H20
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    Barium nitrate - Ba(NO3)2 - formula weight = 261 g/mol

    Moles = mass / formula weight

    Moles of Ba(NO3)2 in 5.00 g = 5.00 / 261 = 0.0192 mol

    Therefore you form 0.0192 mol of BaO

    As you need 2 HCl to neutralise 1 BaO, you need 0.0192 x 2 = 0.0384 mol of HCl

    Volume = moles / concentration

    Volume of HCl required = 0.0384 / 1.20 = 0.032 dm^3

    = 32 cm^3
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    *sigh*

    Yet another "please do my homework for me"

    number of moles = mass/Mr
    number of moles = concentration x volume (in dm3)

    you need that and a calculator.
 
 
 
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