300 mLs of a 2% NaOH (sodium hydroxide, a base) solution are mixed with 200 mLs of a 1% H2SO4 (sulfuric acid) solution.
NaOH + H2SO4 ----> H2O + Na2SO4
a) who is the limiting reagent?
b) who is the leftover reagent, and how much is left over (in moles)
c) how much products (water and salt) are made (in moles)
d) estimate the pH after the reaction is done
e) the molarity of the salt (Na2SO4) in the final solution
I am stumped by this question. How to solve it without knowing the density of each solution, and that varies by temperature?
I balanced the equation
2 NaOH + H2SO4 → 2 H2O + Na2SO4
molar masses:
NaOH: 39.997 g/mol
H2SO4: 98.07848 g/mol
H2O: 18.01528 g/mol
Na2SO4 : 142.04213856 g/mol