Question

1. What volume of each of the following acids will react completely with 70.00 mL of 0.200 M NaOH  ?

a) 0.250 M HCL

b) 0.200 M HNO3

c) 0.100 M HC2H3O2 (1 acidic hydrogen)

2. A 22.26-mL sample of hydrochloric acid solution requires 35.00 mL of 0.115 M sodium hydroxide for complete neutralization. What is the concentration of the original hydrochloric acid solution?

Answer 1

1)

a)

Balanced chemical equation is:

NaOH + HCl ---> NaCl + H2O

Here:

M(NaOH)=0.2 M

M(HCl)=0.25 M

V(NaOH)=70.0 mL

According to balanced reaction:

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

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

1*0.2 M *70.0 mL = 1*0.25M *V(HCl)

V(HCl) = 56.0 mL

Answer: 56.0 mL

b)

Balanced chemical equation is:

NaOH + HNO3 ---> NaNO3 + H2O

Here:

M(NaOH)=0.2 M

M(HNO3)=0.2 M

V(NaOH)=70.0 mL

According to balanced reaction:

1*number of mol of NaOH =1*number of mol of HNO3

1*M(NaOH)*V(NaOH) =1*M(HNO3)*V(HNO3)

1*0.2 M *70.0 mL = 1*0.2M *V(HNO3)

V(HNO3) = 70.0 mL

Answer: 70.0 mL

c)

Balanced chemical equation is:

NaOH + HC2H3O2 ---> NaC2H3O2 + H2O

Here:

M(NaOH)=0.2 M

M(HC2H3O2)=0.1 M

V(NaOH)=70.0 mL

According to balanced reaction:

1*number of mol of NaOH =1*number of mol of HC2H3O2

1*M(NaOH)*V(NaOH) =1*M(HC2H3O2)*V(HC2H3O2)

1*0.2 M *70.0 mL = 1*0.1M *V(HC2H3O2)

V(HC2H3O2) = 140 mL

Answer: 140 mL

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