Expt:Titrating sodium hydroxide with hydrochloric acid
From Learn Chemistry Wiki
In this experiment sodium hydroxide is neutralised with hydrochloric acid to produce the soluble salt sodium chloride in solution. This solution is then concentrated and crystallised to produce sodium chloride crystals.
Apparatus and chemicals
- Eye protection
Each working group requires:
- Burette (30 cm3 or 50 cm3) (see note 1)
- Conical flask (100 cm3)
- Beaker (100 cm3)
- Pipette (20 or 25 cm3) with pipette filler
- Stirring rod
- Small (filter) funnel (about 4 cm diameter)
- Burette stand and clamp (see note 2)
- White tile (optional) (see note 3)
- Bunsen burner with heat resistant mat
- Pipeclay triangle (see note 4)
- Evaporating basin (at least 50 cm3 capacity)
- Crystallising dish
- Access to:
- Microscope or hand lens suitable for examining crystals in the crystallising dish
- Sodium hydroxide solution, 0.4 mol dm-3 (see note 5) (Irritant at this concentration), about 100 cm3 in a labelled and stoppered bottle
- Dilute hydrochloric acid, 0.4 mol dm-3 (Low hazard at this concentration), about 100 cm3 in a labelled and stoppered bottle
- Methyl orange indicator solution (Low hazard at this concentration) (or alternative) in small dropper bottle
Sodium hydroxide (Irritant at concentration used) Refer to CLEAPSS® Hazcard 91, Recipe card 65 Dilute hydrochloric acid (Low hazard at concentration used) Refer to CLEAPSS® Hazcard 47A and Recipe card 31 Methyl orange indicator solution (The solid is Toxic but not the solution) Refer to CLEAPSS® Hazcard 32 and Recipe card 33
- If your school still uses burettes with glass stopcocks, consult the CLEAPSS® Laboratory handbook, section 10.10.1, for their care and maintenance. This experiment will not be successful if the burettes used have stiff, blocked or leaky stopcocks. Modern burettes with PTFE stopcocks are much easier to use, require no greasing, and do not get blocked. Burettes with pinchcocks of any type are not recommended; while cheap, they also are prone to leakage, especially in the hands of student beginners.
- Burette stands and clamps are designed to prevent crushing of the burette by overtightening,
which may happen if standard jaw clamps are used.
- The optional white tile is to go under the titration flask, but white paper can be used instead.
- Ceramic gauzes can be used instead of pipeclay triangles, but the evaporation then takes longer.
- The concentrations of the solutions do not need to be made up to a high degree of accuracy, but they should be reasonably close to the same concentration as each other, and less than 0.5 mol dm-3.
- The evaporation and crystallisation stages may be incomplete in the lesson time. The crystallisation dishes need to be set aside for crystallisation to take place slowly. However, the dishes should not be allowed to dry out completely, as this spoils the quality of the crystals. With occasional checks, it should be possible to decide when to decant surplus solution from each dish to leave good crystals for the students to inspect in the following lesson.
HEALTH & SAFETY: Wear eye protection
a Using a small funnel, pour a few cubic centimetres of 0.4 mol dm-3 hydrochloric acid into the burette, with the tap open and a beaker under the open tap. Once the tip of the burette is full of solution, close the tap and add more solution up to the zero mark. (Do not re-use the acid in the beaker – this should be rinsed down the sink.)
b Use a pipette with pipette filler to transfer 25 (or 20) cm3 of 0.4 mol dm-3 sodium hydroxide solution to the conical flask, and add two drops of methyl orange indicator. Swirl gently to mix. Place the flask on a white tile or piece of clean white paper under the burette tap.
c Add the hydrochloric acid to the sodium hydroxide solution in small volumes, swirling gently after each addition. Continue until the solution just turns from yellow-orange to red and record the reading on the burette at this point. This coloured solution should now be rinsed down the sink.
a Refill the burette to the zero mark. Carefully add the same volume of fresh hydrochloric acid as you used in (c) to another 25 (or 20) cm3 of sodium hydroxide solution, to produce a neutral solution, but this time without any indicator.
a Pour this solution into an evaporating basin. Reduce the volume of the solution to about half by heating on a pipeclay triangle or ceramic gauze over a low to medium Bunsen burner flame. The solution spits near the end and you get less crystals. Do not boil dry. You may need to evaporate the solution in, say, 20 cm3 portions to avoid over-filling the evaporating basin. Do not attempt to lift the hot basin off the tripod – allow to cool first, and then pour into a crystallising dish.
b Leave the concentrated solution to evaporate further in the crystallising dish. This should produce a white crystalline solid in one or two days.
c Examine the crystals under a microscope.
1. What substances have been formed in this reaction? Write a word equation and a symbol equation.
2. Why must you use another 25 cm3 of sodium hydroxide solution, rather than making your crystals from the solution in Stage 1?
3. What shape are the crystals?
This experiment has been reproduced from Practical Chemistry:
This website has a wealth of information on sodium chloride as a mineral (Website accessed January 2011):