The purpose of acid base laboratory experiment was to determine equivalance points. pKa points softe

4. softener to experience how to titrate acid-base
The purpose of acid base laboratory experiment was to determine equivalance points. pKa points softener for a strong acid. HCl, titrated with a strong base, NaOH using a drop approach softener in order to determine completely accurate data. The pH is measured every time 1ml of NaOH added. The pKa of acetic softener acid theoretically is at 4.76. Using a concentration of 0.1M NaOH, we had the largest NaOH volume softener before the largest pH increase at 19.00ml. For the largest NaOH volume after the largest softener pH increases we used 20.00ml of base.  The pKa of amino glicine acid theoretically is at 2.53(carboxylic) and 9.78(amino). This means that the graph of titration of amino glicine acid having two  inflection  point in which this acid can be attached to two different group of carboxylic and amino. However, from this experiment, the first inflection point are skip and only one inflection point or midpoint can be seen.  Using a concentration of 0.1M NaOH, there is no point that we can observed the pH increase drastically. The pH started to be constant at pH 9.83. Unlike other labs, this lab allowed for the most precise titration results possible. The reason for this is that separate drops were entered softener one at a time and their volume was computed in order to add to the total. softener However, due to the fact of adding drops one at a time, time became an issue while completing the experiment. One titration took nearly 30 minutes in order to complete flawlessly.
  An acid-base titration is a neutralization reaction that is performed in the lab in the purpose of to determine an unknown concentration of acid or base. The general purpose of a titration is to determine the amount of particular substance in a sample. Weak acid is different from strong acid as it cannot dissociate completely in the water. Due to this, H + concentration in weak acid depends on the coefficient of equilibrium. When a weak acid is titrated with a strong base, or weak base is titrated with a strong acid, the titration curve is unique for the weak acid or the weak base. Hence, a titration curve can be used to determine the ionization constants for weak acids and weak bases. softener
2
4.34
9.71
18
5.61
11.53
12.15 softener
12.36
12.51
In this experiment, a solution of acetic acid which is a weak acid has been titrated with a 0.1 M solution of NaOH solution. During the titration, the concentration of acid will be decreasing because of the reaction with the increment softener of NaOH. Also, since the conjugate base of the weak acetic acid was the product of this reaction, the concentration softener of base will be increasing at the end of the experiment. The quantities of both acid and base concentrations became equal at some point. The equality occurred halfway to the equivalence point which means half of the weak acid has been converted into its conjugate softener base, so the molar quantities will be identical at this point.
  softener Acetic acid is a monoprotic since it has only has 1 reflection point or 1 pKa point. By analyzing the graph of acetic softener acid, at the half way point (or also known as inflection point or pK a point),   the pH turns out to be 4.76 as 13.50 ml NaOH has been added. Hence, the pK a for the acetic acid must also be 4.76 (by applying the Henderson-Hasselbalch equation, pH= pK a ). The acid ionization constant, K a , can be calculated;
            softener       = 1.74 x 10 -5 The equivalent point is a midpoint of the vertical line. However, in this graph, the equivalent point was not reach yet since the experiment softener was stop after 26 ml of NaOH was added. By looking at the actual graph of acetic acid, the equivalent point was marked as 27.02 ml of NaOH has been added into the weak acid solution.  
             Titration curves softener are obtained when the pH of given volume of a sample solution varies after successive addition of acid or alkali. The curves are usually plots of pH against the volume of titrant added or more correctly against the number of equivalents added per mole of the sample. This curve empirically defines several characteristics (the precise number of each characteristic depends on the nature of the acid being titrated: 
           Amino Acids are Weak Polyprotic Acids.    They are present softener as zwitter ions at neutral pH and are amphoteric molecules that can be titrated with both acid and alkali. All of the amino acids have an acidic group (COOH) and a basic group (NH2) attached to the α carbon, and also they contain ionizable groups that act as weak acids or bases, giving off or taking on protons when the pH is altered. The strong positive charge on the amino group induces a tendency softener for the carboxylic softener acid group to lose a proton , so amino acids are considered to be strong acids. Some ami