Standardizing a sodium hydroxide solution lab report

Simply placing your flask onto the balance and then weighing your flask and its contents is not always precise because moisture or other substances on the outside of your flask may result in some error in your measurements.

Finally, It is a good idea to double-check all readings of your buret with your lab partner to ensure accurate results. However by using the formula for determining the molarity of a substance and a simple proportion, it was found that the vinegar used during the experiment was not legal.

Students need training in using burettes correctly, including how to clamp them securely and fill them safely. Aim To calculate the concentration or molarity of sulfuric acid solution by reaction with a basic solution of sodium hydroxide. This solution is then concentrated and crystallised to produce sodium chloride crystals.

Experimental Set-up and Procedure: Data The data recorded on Page consists of two parts: There is no need to dry these items after rinsing. To determine the equivalent mass of an unknown acid. This should produce a white crystalline solid in one or two days. Titration should proceed until the faintest pink persists for 30 sec.

Please give me step by step calculations for standardizing 1N NaOH using potassium phthalate?

Repeat the titration with a second sample of HCl. In conclusion, although there were sources of error, the hypothesis was proven correct by the efficiency of the procedures and the accuracy of the results obtained. This experiment will not be successful if the burettes used have stiff, blocked or leaky stopcocks.

Even though it would take longer to complete the experiment this way, this would help achieve more accurate results. The resulting percentage error out of this deviation is: All waste containing your unknown acid must be disposed of in the hazardous-waste container in the fume hood.

The experiment is most likely to be suited to 14—16 year old students. Another error was caused by the deviation in the mass of KHP. It is a good idea to have a lab partner doublecheck your buret readings in this and subsequent steps.

This might have caused some deviations because the volume of sodium hydroxide added was excess. The acid was added to the flask by slowly opening the stopcock.

Your flasks should be rinsed several times with deionized water before use. If you are unsure whether only a single drop of titrant was dispensed, then you should discard and repeat the trial you are performing or in some cases you may perform a back titration.

Titration of Sulfuric Acid and Sodium Hydroxide One of the most basic experiments taught to everyone in school, the titration between an acid and a base helps us to calculate the concentration of a solution, whose volume is known.

The indicator was used to ensure the titration ended at the right time. Swirl gently to mix. Three ml conical glass flasks.

Obtain a vial containing your solid acid unknown from your instructor. The acidic hydrogen of KPH reacted with the hydroxide in sodium hydroxide to form water that was neutral. Then you removed your first sample and weighed the beaker containing the remainder of the KHP.

In this experiment a pipette is not necessary, as the aim is to neutralise whatever volume of alkali is used, and that can be measured roughly using a measuring cylinder.

Titration Lab: NaOH with Standardized solution of KHP

Explain why the high molar mass of KHP is an advantage to its being used as a primary standard. This flaw was due to allowing excess sodium hydroxide to flow, causing the KHP solution to become pinker than it should have.

Burets should be properly clamped into the buret stand so that they are held in a vertical position. By the weighing by difference method, you also did not have to dry out the Erlenmeyer flasks into which you placed the samples.

If you weighed the samples out by the earlier method, you would have needed to make eight mass determinations mass of empty container, mass of container with sample. Modern burettes with PTFE stopcocks are much easier to use, require no greasing, and do not get blocked. This might have affected the precision and accuracy of the morality and mass measurements.

Refill each of your burets and perform two additional titrations in a similar manner. This flask does not need to be dried because the amount of deionized water inside will not change the number of moles of acid added. The standardization of sodium hydroxide with KPH was done by comparing the amount of sodium hydroxide solution needed to react with a known amount of Potassium hydrogen phthalate.

That is systematic and random.

4: Determining the Equivalent Mass of an Unknown Acid by Titration (Experiment)

Chemistry Lab Report on standardization of acid and bases. 1. Purpose: To prepare standardize solution of sodium hydroxide and to determine the concentration of unknown sulfuric acid solution. TITRATION OF SULPHURIC ACID WITH SODIUM HYDROXIDE Modified: November 3, INTRODUCTION A TITRATION is a process in which a measured amount of a solution is reacted with a known volume of another solution (one of the solutions has an unknown concentration) until a desired end point is reached.

Standardizing A Sodium Hydroxide Solution Lab Report. Abstract.

Standardization of permanganate solution for use in potentiometric titrations

This report is about how to standardize a Sodium Hydroxide (NaOH) solution by titrating it with pure sample of Potassium acid Phthalate (KHC8H4O4).

This experiment has two sections. The first section is to standardize the Sodium Hydroxide by titration. Three sample of – g of solid KHP are place into each of the three. McBride) StandardizationofPotassiumPermanganate However,thisauthorqualifiestheproposedexplanationbythe followingstatements.

A standard solution of known concentration is “titrated against” (reacted with) a solution of unknown concentration.

Titration is the technique to find the concentration of unknown solution by the formula Ma x Va = Mb x Vb to determine the exact concentration of sodium hydroxide solution.

Four lab periods assigned for this experiment. In part I you will prepare an acid (HCl) solution and a base solution and a base (NaOH) solution.

These solutions will be used for all four periods so it is important to keep these solutions. These solutions will be titrated against each other to obtain a base/acid ratio. then report

Standardizing a sodium hydroxide solution lab report
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Titrating sodium hydroxide with hydrochloric acid- Learn Chemistry