Question

Calculate the volume in mL of a 1.420M NaOH soution required to titrate the following solutions:

a) 25.00mL of a 2.430M HCl solution

b) 25.00mL of a 4.500M H2SO4 solution

(can you please show all the steps and work needed to solve this problem, thank you!)

Answer 1

a)

we have the Balanced chemical equation as:

NaOH + HCl ---> NaCl + H2O

Here:

M(HCl)=2.43 M

M(NaOH)=1.42 M

V(HCl)=25.0 mL

According to balanced reaction:

1*number of mol of NaOH =1*number of mol of HCl

1*M(HCl)*V(HCl) =1*M(NaOH)*V(NaOH)

1*2.43 M *25.0 mL = 1*1.42M *V(NaOH)

V(NaOH) = 42.78 mL

Answer: 42.78 mL

b)

we have the Balanced chemical equation as:

2 H2SO4 + NaOH ---> Na2SO4 + 2 H2O

Here:

M(H2SO4)=4.5 M

M(NaOH)=1.42 M

V(H2SO4)=25.0 mL

According to balanced reaction:

1*number of mol of H2SO4 =2*number of mol of NaOH

1*M(H2SO4)*V(H2SO4) =2*M(NaOH)*V(NaOH)

1*4.5 M *25.0 mL = 2*1.42M *V(NaOH)

V(NaOH) = 39.61 mL

Answer: 39.61 mL