The titration of 20.0 mL of an unknown concentration #H_2SO_4# solution requires 83.6 mL of 0.12 M #LiOH# solution. What is the concentration of the #H_2SO_4# solution (in M)?

1 Answer
Jun 10, 2016

Answer:

#(C_M)_(H_2SO_4) = 0.25 \ mol.L^-1#

Explanation:

Write a balanced chemical equation for the neutralization reaction to figure out the mole relationship between the sulfuric acid and lithium hydroxide.

#H_2SO_4 + 2LiOH -> Li_2SO_4 + 2H_2O#

#n_(H_2SO_4) = 1/2 \ n_(LiOH)#

#underbrace((C_MxxV))_("number of moles of "H_2SO_4) = 1/2\ \ \ \ \ \ xxunderbrace((C_MxxV))_("number of moles of "LiOH)#

Note that #C_M# is the molar concentration and #V#is the volume of solution.

#(C_MxxV)_(H_2SO_4) = 1/2( C_MxxV)_(LiOH)#

#(C_M)_(H_2SO_4) = (C_MxxV)_(LiOH)/( 2* V_(H_2SO_4)#

#(C_M)_(H_2SO_4) = (0.12 \ mol.L^-1xx 83.6 \ mL)/( 2xx20.0 \ mL)#

#(C_M)_(H_2SO_4) = (0.12 \ mol.L^-1xx 83.6 \ cancel (mL))/( 2xx20.0 \ cancel(mL))#

#(C_M)_(H_2SO_4) = 0.25 \ mol.L^-1#