Investigating The Concentration Of A Hydrochloric Acid A Solution Using Acid ‚Äê Base Titration

We know that that the end point of the titration is reached when, after drop after careful drop of NaOH, the solution in the flask retains its pale pink color while swirling for about 30

2. To titrate a hydrochloric acid solution of “known” concentration with standardized 0.5M sodium hydroxide.

Chemistry 102 is the study of kinetics – equilibrium constant. When it comes to the study of acid-base, equilibrium constant plays an important role that tells how much of the H+ ion will be released into the solution. In this lab, the method of titrimetry was performed to determine the equivalent mass and dissociation constant of an unknown weak monoprotic acid. For a monoprotic acid, it is known that pH = pKa + log (Base/Acid). When a solution has the same amount of conjugate base and bronsted lowry acid, log (Base/Acid) = 0 and pH = pKa. By recording the pH value throughout the titration process and determining the pH at half- equivalence point, the value of Ka can be easily calculated. In this experiment, the standardized NaOH solution has a concentration of 0.09834 M. The satisfactory sample size of known B was 0.2117 g. The average equivalent mass of the unknown sample was found to be 85.01 g, pKa was found to be 4.69, which was also its pH at half-equivalence point and Ka was found to be 2.0439×〖10〗^(-5). The error was 1.255% for equivalent mass and 0.11% for Ka. In other word, the experiment was very precise and accurate; the identity of the unknown sample was determined to be trans-crotonic by the method of titrimetry.

ii. The second part of the titration series involves titration of NaOH with Hydrochloric acid (HCL). Again, three reps of titration and a blank titration have to be completed. A volumetric pipet is used to measure 10.00mL of HCL into three labeled conical flasks. Then the flasks are filled with deionized water until about the 50mL mark. A buret is

Titration is a lab method that used to determine a quantitative analysis which used to know the concentration of a drug or compound, and this process happen by use a reagent which is known its concentration and its volume to calculate the another concentration or volume, this reagent called titrant and it may be acid or base. There are many types of titration to determine different orders of drugs and compounds like (acid base titration- Redox titration- Gas phase titration- Complexometric titration- Zeta potential titration). The most common method for quantitative analysis is acid- base titration and redox titration. 1- Acid base titration is the method which depends on the naturalization between acid and base in the flask then changes the color of ph. indicator (ph.ph or methyl orange) till reach the endpoint. 2- Redox titration is the method which relies on reduction-oxidation reaction between titrant and sample and we use a redox indicator toll reach the indicator. 3- Gas phase titration this method of quantitative analysis is occurs in gas phase. 4- Complexometric titration is depend on form a complex between titrant and sample in which we are used a complexometric indicator which this indicator form a weak complex with sample, then the titration happen till reach the endpoint. 5- Zeta potential titration we use this

The purpose of this experiment was to determine the pKa of the bromothymol blue (indicator) through absorption spectroscopy. Bromothymol blue being a monoprotic acid base indicator, displays different colors at different pH because of the differences in the ratio of the conjugated acid and base form. The fraction of conjugate acid and base was interpolated for the solutions through the acquired absorbance spectrum of the bromothymol blue at various pH. The rearranged form of Henderson Hasselbalch equation was graphed as a function of pH to determine the pKa of the indicator.

During a titration the pH of the solution will be monitored using a pH meter from that we get a titration curve. The titration curve is then used to determine the equivalent molecular weight and Ka value of the unknown weak acid, from that we are

In Part 1, ~0.30g of KHP is dissolved in 25.00 mL of water, and titrated with NaOH. The volume of NaOH added to reach the endpoint is recorded and corrected (Table 1). The number of moles of NaOH reacted in trial 1 and trial 2 are 0.001534 mol and 0.001433 mol (Equation 1). The concentration of NaOH in trial 1 and trial 2 are 0.07331 M and 0.06628 M (Equation2). The average concentration of NaOH is 0.06979 M (Equation 3). The average deviation is 0.003515 M (Equation 4). In Part 2, ~0.13g of Na2CO3 is dissolved in 25.00 mL of water, and titrated with HCl. The volume of HCl added to reach the endpoint is recorded and corrected (Table 2). The number of moles of HCl reacted in trial 1 and trial 2 are 0.001225mol and 0.001253mol (Equation 5). The concentration of HCl in trial 1 and trial 2 are 0.03298M and 0. 0.03477M (Equation 6). The average concentration of HCl is

By using acid-base titration, we determined the suitability of phenolphthalein and methyl red as acid base indicators. We found that the equivalence point of the titration of hydrochloric acid with sodium hydroxide was not within the ph range of phenolphthalein's color range. The titration of acetic acid with sodium hydroxide resulted in an equivalence point out of the range of methyl red. And the titration of ammonia with hydrochloric acid had an equivalence point that was also out of the range of phenolphthalein.. The methyl red indicator and the phenolphthalein indicator were unsuitable because their pH ranges for their color changes did not cover the equivalence points of the trials in which they were used. However, the

First, three titration curves and three second derivative curves were created to determine the average pH at the half-equivalence point from the acetic acid titrations. Titration curves were used as visuals to portray buffer capacity. The graphs and a table, Table 1, that showcased the values collected were created and included below. The flat region, the middle part, of Figures 1, 2 and 3, showed the zone at which the addition of a base or acid did not cause changes in pH. Once surpassed, the pH increased rapidly when a small amount of base, NaOH, was added to the buffer solution. Using the figures below and

The purpose of this lab was to use process titration to find concentration of an aqueous solution of Hcl(aq) , using KOH(aq) as the titrant.

An acid-base titration is the determination of the concentration of an acid or base by exactly neutralizing the acid/base with an acid or base of known concentration. This allows for quantitative analysis of the concentration of an unknown acid

Determination of Concentration of Hydrochloric Acid and Phosphoric Acid in an Unknown HCl – H3PO4 Mixture through Use of Potentiometric Titrations

For this experiment, a pH meter was used so this part of the experiment began with the calibration of the pH meter with specified buffers. The buret was then filled with the standard HCl solution and a set-up for titration was prepared. 200g of the carbonate-bicarbonate solid sample was weighed and dissolved in 100 mL of distilled water. The sample solution was then transferred into a 250-ml volumetric flask and was diluted to the 250-mL mark. The flask was inverted several times for uniform mixing. A 50-mL aliquot of the sample solution was measured and placed unto a beaker. 3 drops of the phenolphthalein indicator was added to the solution in the beaker. The electrode of the pH meter was then immersed in the beaker and the solution containing the carbonate-bicarbonate mixture was titrated with the standard HCl solution to the phenolphthalein endpoint. Readings of the pH were taken at an interval of 0.5 mL addition of the titrant. After the first endpoint is obtained, 3 drops of the methyl orange was added to the same solution and was titrated with the standard acid until the formation of an orange-colored solution. Readings of the pH were also taken at 0.5 mL addition of the titrant.

It took an average of 14.5 mL acid titrant (HCl) to make the pink solution colorless or to reach the phenolphthalein endpoint while 36.85 mL of the titrant was used to reach the methyl orange endpoint.