ml of t0.00M HCl solution in a small beaker is titrated with 0.10M NaOH solution

Question

ml of t0.00M HCl solution in a small beaker is titrated with 0.10M NaOH solution a) Write the acid-base reaction that occurs during the titration. b) Calculate the value of the equilibrium constant for the titration reaction in from a buret. All experiments are carried out at 25°C. 2a. Is it reasonable to assume that this titration reaction goes essentially to completion? Explain. c) Predict the pH of the solution at the equivalence point of the titration (acidic, basic or neutral). Explain your reasoning

Explanation / Answer

a)

HCl + NaOH = NaCl + H2O

this is already balanced

b)

if essentially goes to completion

K = [NaCl]/([HCl][NaOH])

[NaCl] >> [HCl] and [NaOH]

K = infinite

c)

find pH in equilibirum,

storng acid + strong base

will always have pH = 7

since it is neutralized, expect no hydrolysis or side reaction

Related Questions

Navigate

• Browse (All)
• Browse M
• Subjects

---

---

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