A student titrates a 25 mL of an unknown concentration of HCl with 35 mL of a 0.890 M solution of KOH to reach the equivalence point. What is the pH of the HCl solution? Paired item 1)

Question

A student titrates a 25 mL of an unknown concentration of HCl with 35 mL of a 0.890 M solution of KOH to reach the equivalence point. What is the pH of the HCl solution?  Paired item 1)

Quizplus · Accepted Answer

The equivalence point is reached when the moles of acid and base are equal. Therefore, the moles of HCl are equal to the moles of KOH:```moles of HCl = moles of KOHMoles of HCl = (0.890 M) * (0.035 L) = 0.03115 mol```The concentration of HCl can be calculated by dividing the moles of HCl by the volume of the HCl solution:```Concentration of HCl = moles of HCl / volume of HCl solutionConcentration of HCl = 0.03115 mol / 0.025 L = 1.246 M```The pH of the HCl solution can be calculated using the following equation:```pH = -log[H+]```The concentration of H+ ions in the HCl solution is equal to the concentration of HCl:```[H+] = 1.246 M```Therefore, the pH of the HCl solution is:```pH = -log(1.246) = 0.10```

A Student Titrates a 25 ML of an Unknown Concentration