Phenolphthalein: Finding concentration with titration

Phenolphthalein (pronounced fe-nul-tha-Leen) is a commonly used indicator. Phenolphthalein is

✓ Clear and colorless in an acid solution

✓ Pink in a basic solution

Chemists use phenolphthalein in a procedure called a titration, in which they determine the concentration of an acid or base by its reaction with a base or acid of known concentration. Here’s how to evaluate an acid solution using titration:

1. Add a couple drops of phenolphthalein to a known

volume of the acid solution you want to test.

Because you’re adding the indicator to an acidic solution, the solution in the flask remains clear and colorless. Suppose, for example, that you want to determine the molar concentration of an HCl solution. First, you place a known volume (say, 25.00 milliliters measured accurately with a pipette) in an Erlenmeyer flask (that’s just a flat-bottomed, conical-shaped flask) and add a couple drops of phenolphthalein solution.

2. Add small, measured amounts of a base of known molarity (concentration) until the solution turns light pink.

Add small amounts of a standardized sodium hydroxide (NaOH) solution of known molarity (for example, 0.100 M) with a buret. (A buret is a graduated glass tube with a small opening and a stopcock valve, which helps you measure precise volumes of solution.) Keep adding base until the solution turns the faintest shade of pink detectable. I call this the endpoint of the titration, the point at which the acid has been exactly neutralized by the base.

3. Write the balanced equation for the reaction.

Here’s the reaction:

HCl(aq) + NaOH(aq) → H₂O(l) + NaCl(aq)

4. Calculate the molarity of the acidic solution.

From the balanced equation, you can see that the acid and base react in a 1:1 mole ratio. So if you can calculate the moles of bases added, you’ll also know the number of moles of HCl present. Suppose that it takes 35.50 milliliters of the 0.100 M NaOH to reach the endpoint of the titration of the 25.00 milliliters of the HCl solution. Knowing the volume of the acid solution then allows you to calculate the molarity (note that you convert the milliliters to liters so that your units cancel nicely):

مواضيع ذات صلة

التفاعل مع اصباغ الازو

تفاعل الجالكونات مع البروم

تفاعل الجالكونات مع الهكسانون الحلقي

تفاعل الجالكونات مع اليوريا ومعوضاته

تفاعل الجالكونات مع البيروكسيدات

تفاعل الجالكون مع الهيدرازين والفنيل هيدرازين

مركبات الجالكون Chalcone Compounds

تفاعل إضافة مايكل

الاضافة الالكتروفيلية الى مركبات الكاربونيل ألفا – بيتا غير المشبعة

تفاعلات تكاثف مركبات الكاربونيل

تحضير مركبات الكاربونيل ألفا – بيتا غيرالمشبعة

مركبات الكاربونيل ألفا – بيتا غير المشبعة