Answer:
[tex]\% HClO_4=5.65\%[/tex]
Explanation:
Hello,
In this case, since the reaction between barium hydroxide and perchloric acid is:
[tex]2HClO_4+Ba(OH)_2\rightarrow Ba(ClO_4)_2+2H_2O[/tex]
It means there is a 2:1 mole ratio between the acid and the base; thus we compute the moles of barium hydroxide that are reacting:
[tex]n_{Ba(OH)_2}=0.0107L*0.338 mol/L=0.00363molBa(OH)_2[/tex]
Now, we compute the mass of perchloric acid (molar mass = 100.46 g/mol) by considering that 2:1 mole ratio:
[tex]m_{HClO_4}=0.00363molBa(OH)_2*\frac{2molHClO_4}{1molBa(OH)_2} *\frac{100.45gHClO_4}{1molHClO_4} =0.729gHClO_4[/tex]
Finally, the percent of perchloric acid in such sample is:
[tex]\% HClO_4=\frac{0.729g}{12.9g} *100\%\\\\\% HClO_4=5.65\%[/tex]
Best regards!
