Question

PLEASE HELP

Titration #1
A total of 25.0 mL of 0.150 M potassium hydroxide (KOH) was required to neutralize 15.0 mL of sulfuric acid (H2SO4) of unknown concentration. What is the concentration of the sulfuric acid?
Balanced Equation:
Acid(unknown) - Solution, Molar Ratio, Volume, Concentration
Base(known) - Solution, Molar Ratio, Volume, Concentration

Answer 1

2KOH + H2SO4 = K2SO4 + 2H20

From the reaction, it can be seen that KOH and H2SO4 have the following amount of substance relationship:

n(KOH):n(H2SO4)=2:1

From the relationship we can determinate required moles of H2SO4:

n(KOH)=c*V=0.15M*0.025L= 0.00375 mole

So,

n(H2SO4)=n(KOH)/2= 0.00375/2= 0.00188 moles

Now, when moles of H2SO4 is known, concentration can be calculated:

c(H2SO4)=n/V= 0.00188mole/0.015L= 0.125M