Question
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)
Answers
DrBob222
A.
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.
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.
Anonymous
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