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ACID-BASE TITRATION I. Objective Students can acquire knowledge and ability in determining concentration of the solution by divalen acid-base titration (H 2SO 4) by using phenoltalein indicator (PP). Theory According to Br o nsted and Lowry, an acid is a species which donates a proton, H +, and a base is a species which accepts a proton in a proton-transfer reaction. For example, in the following acid-base reaction: H 2SO 4 (aq) + 2NaOH (aq) → 2H 2O (l) + 2Na + (aq) + SO 4 2 – (aq) H 2SO 4 (aq) is an acid which donates a proton, H +, to the base NaOH (aq).
This reaction is often called a neutralization reaction. An acid-base titration is a procedure for determining the concentration of an acid (or a base) in a solution by measuring the volume of base (or acid) of a known concentration that completely reacts with it. The solution of accurately known concentration is called the standard solution (titrant), it contains a definite number of gram-equivalents per liter.
Standard solution is usually added from a graduated vessel called a burette. The process of adding titrant until the reaction just complete is termed a titration and the substance to be determined is titrated (analyte). The point at which the reaction is complete is called the equivalence point or the theoretical (or stoichiometric) end point. This point must be detectable by some change unmistakable to the eye and this can be done by adding an auxiliary reagent, known as an indicator which should give a clear visual change (color change) in the liquid being titrated. In order to perform a titration procedure a reaction must fulfill the following condition. It must be simple reaction, which can be expressed by a chemical reaction. The substance to be determined should react completely with the titrant in stoichiometric or equivalent proportions.
The reaction should be practically instantaneous or proceed with very great speed. There must be a marked change in some physical or chemical property (as color change) of the solution at the equivalence point. An indicator should be available which, by a change in physical properties (Color), should sharply define the end point of the reaction. If no visible indicator is available for the detection of the equivalence point, the latter can often be determined by other method as potentiometer or conduct metric or spectrophotometer titration. Titration can be used for many types of reactions: a. Neutralization (reaction of acid with base.). Precipitation reaction.
Oxidation – reduction reactions d. Complex formation reactions. Materials and equipments v Materials NaOH solution 0,1 N H 2SO 4 solution x N P henolphthalein Indicator (PP) v Equipments Burette 50 mL 1 pcs Erlenmeyer flask 250 mL 2 pcs Drooping Pipette 2 pcs Graduated Glass Cylinder 50 mL 2 pcs Stirring Stick 1 pcs Funnel 1 pcs Volumetric Pipette 10 mL 1 pcs Stand, retort and klem (stative) 1 set IV. Procedure. Equipments are set for titration process.
Burette is washed up with aquades and the tap’s leakage is checked accuracy. Burette is washed up with some titrant (NaOH 0,1 N).
Titrant (NaOH 0,1 N) are entered into burette using funnel to zero numeral. 10 mL titrated (H 2SO 4) are entered into Erlenmeyer flask. Titrated are added phenoltalein indicator (PP) around 1-2 crop.
Titra tion is done by drooping titrant into titrat ed bit by bit from buret te. Titra tion are stopped until the titrated’s color changed. T itran t volumes are written down. 5-9 procedure are repeated 3 times. Average titrant’s volume that used are calculated. Unknown concentration of solution are calculated. Observe result Observe table of H 2SO 4 solution.
Repeating Volume Titrat e Volume (H 2SO 4) Titran t Volume (NaOH 0,1 N) 1 10 mL 9,6 mL 2 10 mL 9,1 mL 3 10 mL 9,4 mL Average Volume 10 mL 9,4 mL VI. Discussion The experiment that we did is name alkalimetri titration because it is done to determine concentration of acid solution (H 2SO 4) by using base standard solution (NaOH 0,1 M). The titrated in this experiment is H 2SO 4 x M around 10 mL. PP indicator is added to differentiate acid solution with base solution s o that by adding 2 drops PP indicator in H 2SO 4 x M make the H 2SO 4 x M solution still uncolored. Then in the titrated is titr ationed by NaOH 0,1 M solution.
This procedure is repeated 3 times. End point indication of titration is the changed of titrated color from uncolored into red when the volume of NaOH 0,1 M solution is used around 9,6 mL;9,1 mL; and 9,4 mL each other.
Next, will be done a calculation of concentration based on the theory and the experiment’s result. For H 2SO 4 Tirtation with NaOH as titrant: Rea ction between H 2SO 4 and NaOH is: Rea ction: H 2SO 4 (aq) + 2NaOH (aq) Na 2SO 4 (aq) + 2H 2O (l) From reaction above we can know that the ratio of mol between H 2SO 4 and NaOH is 1:2. So, to calculate concentration of H 2SO 4 solution based on the experiment’s result, we can use the equation below.
Mmol ion H + = mmol ion OH – Ma. Vb Information: Ma = acid molarity H XA Mb = strong base molarity L(OH) n Va = acid volume Vb = base volume X = acid valence n = base valence According to The Theory: To determine NaOH solution’s volume that needed: T itra nt ( NaOH ) that used: 0,1 N same as 0,1 M ( because it is monovalen). Titrated ( H 2SO 4 ) that used: 0,1 N same as 0,05 M ( because it is divalen). This concentration is acquired based on the calculation H 2SO 4 concentration that made by group 2 and laboratory assistant. 2.10 mL = 0,1 M. Vb 1 mL = 0,1. Vb Vb = 1 mL / 0,1 = 10 mL So, to calculate H 2SO 4 0,05 M need 10 mL NaOH 0,1 N ( based on the th eor y ) Based on the experiment’s result: Experiment I ( needed NaOH around 0,96 mL) Ma.
10 ml = 0,1 M. 20 ml = 0,96 mmol Ma = 0,96 mmol/20 ml = 0,048 M Experiment II ( needed NaOH around 0,91 mL) Ma. 10 ml = 0,1 M. 20 ml = 0,91 mmol Ma = 0,91 mmol/20 ml = 0,0455 M Experiment III ( needed NaOH around 0,94 mL) Ma. 10 ml = 0,1 M. 20 ml = 0,94 mmol Ma = 0,94 mmol/20 ml = 0,047 M Calculate using average volume: Ma.
10 ml = 0,1 M.