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How many milliliter of 0.150 M H2SO4 (sulfuric acid) are required to react with 1.87 g of sodium hydrogen carbonate, NaHCO3, according to the following equation?

H2SO4 + 2NaHCO3 --> Na2SO4 + 2H2O + 2CO2

dont understand this am i suppose to change 1.87 into Molarity for liters or something?? never learned how to do that
thanks for the comments in advance

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3 answers
  1. A step by step procedure for working these problems.
    http://www.jiskha.com/science/chemistry/stoichiometry.html

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  2. @DrBob222 the link you provided doesnt do a good job in explaining how to convert grams into liters/Molarity
    if you can do u think u can go into a little more detail on showing me what to do with the 1.87 sodium hydrogen carbonate?
    thanks

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  3. Grams don't convert to liters or to molarity.. Grams converts to moles. moles = grams/molar mass. Then you use the equation to convert moles of one material to moles of the other. If you have M and L, then moles = M x L.
    So just follow the steps.
    Convert 1.87 grams NaHCO3 to moles. moles = grams/molar mass.
    2. You have moles NaHCO3, now convert that to moles H2SO4 using the coefficients in the balanced equation.
    3. Now you have moles H2SO4. M x L = moles. You have moles and M from the problem, solve for L and convert to mL.

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