Assume you dissolve 0.235 g of the weak acid benzoic acid, C 6 H 5 CO 2 H, in en

Question

Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 ? 102 mL of solution and then titrate the solution with 0.158 M NaOH.

What are the concentrations of the following ions at the equivalence point?

Na+, H3O+, OH-
C6H5CO2-

_____________M Na+
_____________M H3O+
_____________M OH-
_____________M C6H5CO2-
What is the pH of the solution?

Assume you dissolve 0.235 g of the weak acid benzoic acid, C6H5CO2H, in enough water to make 1.00 ? 102 mL of solution and then titrate the solution with 0.158 M NaOH. C6H5CO2H(aq) + OH-(aq) C6H5CO2-(aq) + H2O(?) What are the concentrations of the following ions at the equivalence point? Na+, H3O+, OH- C6H5CO2- _____________M Na+ _____________M H3O+ _____________M OH- _____________M C6H5CO2- What is the pH of the solution?

Explanation / Answer

first, calculate the moles of benzoic acid

moles of benzoic acid = 0.235 g / 122.12 g/mol=0.00192 moles

As the relation es 1:1

moles NaOH required = 0.00192

Now, calculate the required volume of NaOH

volume of NaOH = 0.00192 / 0.108 M=0.0178 L

total volume = 0.0178 L + 0.100 L = 0.118 L

Again, as the relation is 1:1, in a complete reaction you

Related Questions

Navigate

• Browse (All)
• Browse A
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.