In a titration of a sample of vinegar, you find that it requires 11.10 mL of 0.748 M NaOH to neutralize a 10.0 mL of sulfuric acid (H2SO4)
a) write the balanced equation
b) what is the concentration of the sulfuric acid solution?
c) label acid and base as strong or weak

Question

In a titration of a sample of vinegar, you find that it requires 11.10 mL of 0.748 M NaOH to neutralize a 10.0 mL of sulfuric acid (H2SO4)
a) write the balanced equation
b) what is the concentration of the sulfuric acid solution?
c) label acid and base as strong or weak

abb0t · Answer

2 NaOH + H$_2$SO$_4$ $\rightarrow$ Na$_2$SO$_4$ + 2 H$_2$O 

Now, to find the concentraton, I'm assuming they want to know the concentration at equivalence point (the point its "neutralized", use $\sf \color{blue}{M_1V_1=M_2V_2}$

where M$_1$ = initial concentration, and V$_1$ = starting volume, same for the other two, is final. You're solving for $\sf \color{red}{M_2}$. 

Both are very strong acid/bases.

cometailcane · Answer

Thank you!