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Sodium oxide, reacts with water to give NaOH. A) Write a balance equation? B)What is the pH of the solution prepared by allowing 1.55 g of Na2O to react with 500.0 ml of water? (assume there is no volume change) C) How many milliliters of 0.0100M HCL are needed to neutralize the NaOH prepared in(b)

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    Na2O + HOH ==> 2NaOH

    B. There is a long way and a short way of doing this. The long way is to make a stoichiometry problem out of it, convert g Na2O to moles, calculate moles NaOH formed, then use M = moles/L.
    A shorter way is to forget about stoichiometry and reason it out.
    moles Na2O = 1.55 g/molar mass Na2O = ??
    moles NaOH = 2*moles Na2O
    M = moles/L
    M NaOH = molarity of OH^-
    Then pOH = -log(OH^-) and
    pH + pOH = pKw = 14
    Solve for pH.

    C. Use
    mL acid x M acid = mL base x M base.
    Solve for the unknown, mL acid.

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