How many milliliters of a 0.2075 M NaOH solution are needed to completely neutralize 18.00 mL of 0.3198 M H2SO4?

Question

marmar10 · Answer

i keep getting 27.74 mL but its not right -_-

marmar10 · Answer

@Cuanchi

anonymous · Answer

Show me the balanced equation please.

marmar10 · Answer

NaOH + H2SO4 = H2O + Na2SO4 i think this is right

marmar10 · Answer

@Hoslos

anonymous · Answer

An equation is balanced when the total number of atoms of every element is the same on both sides of the equation, that is$$2NaOH + H _{2}SO _{4}\rightarrow Na _{2}SO _{4}+2H _{2}O$$

marmar10 · Answer

oh wow sorry i didnt balance it haha wow im tired. Ill try and see if i can get the right answer now

marmar10 · Answer

i got it now haha :') its 55.48 mL

anonymous · Answer

This type of exercises are solved by first balancing equations so that you find ratios and proportions.
As you can see, the molar or volume ratio of sodium hydroxide to sulphuric acid is 2:1.
First, find the number of moles from the limiting reagent, which is sulphuric acid.
$$mol=\frac{ concentration*volume }{ 1000 }$$
$$mol=\frac{ 0.3198*18 }{ 1000 }=0.005mol$$

anonymous · Answer

For NaOH, the mol has to be doubled , giving 0.01mol.
Using the same formula of mol for NaOH and making v the subject you get$$volume=1000mol/concentration=\frac{ 1000*0.01 }{ 0.2075 }=48.19ml$$