The Effect Of Ethanoic Acid On The Reaction Of Oxalic Acid

The error is often caused because of the inability to gather the exact same data consistently. Systematic error is usually constant and due to the environment or to the equipment. Gross error is a human error that usually creates an outlier. Significant figures in this experiment are determined through a variety of rules:

Titration is the slow adding of one solution of a known concentration (called a titrant) to a known volume of another solution of unknown concentration until the reaction reaches neutralization which is indicated by color change (1). We take the solution of known concentration and carefully mix it with unknown concentration until the solution is concentrated. The main goal of this experiment was to prepare a standard solution of oxalic acid and use it to standardize an unknown sodium hydroxide solution. And finally to determine the molar mass of unknown solid acid by titration with standardized NaOH solution. By weighting a sample prepare a solution of an acid of known concentration. Make it up to a known volume in a volumetric flask. We use

was to determine the percentage by mass of acetic acid in vinegar using acid/base titration. The

Table 2: Consists of color extract taken from a red cabbage for a natural indicator. The pH reading that was measured by using the pH meter and the result of the pH reading to determine whether the solution was acidic or basic.

To begin, three sets ofabout 0.3000g of KHP are weighed out on an analytical balance. Put the three sets of KHP into three separate, labeled flasks. All three sets of the KHP is then dissolved with approximately 50mL of deionized water. Next, a buret is used to start the actual titration. Buret is initially filled to 0.00mL mark with the NaOH solution, this is recorded as initial volume. Next, add 2-3 drops of phenolphthalein indicator into each of the three flasks containing KHP. A magnetic stir bar is then added to the first flask, and placed above a stir plate. Everything is positioned under the buret. Stirrer is put on medium speed and the titration can start. Slowly release the NaOH into the KHP flask. As the end point is reached, a pink color will be seen in the flask. When the lightest pink possible remains in the solution for more than 30 seconds titration is complete. The final volume is recorded, and the same steps are taken for the other two sets of KHP solution. Finally, blank titration is completed to determine deviation.

to correct data. The types of error present may be either systematic, human, or random errors.

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

What errors were made in this case? Can you differentiate between latent and active errors?

A: Accuracy is the degree of closeness of measurements of a quantity to the actual (or accepted) value and precision is the degree to which repeated measurements show the same result.

In my opinion, accurate is when you have a measurement and you are more close to the actual value, on the other hand, precision is when you have repeated measurements and they do not have to be close to the real value, for example when you are doing an experiment and you have to do three trials and they are giving you the same result but at the same time, they are far away from the true value.

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

If an experiment contains biological error or systematic errors, they must be considered in addition to the statistical error in order to completely analyze the data.

Precision is the degree of concordance among a number of estimates of the same population (repeatability). It is used to estimate the number of replicate samples required for it to be representative of the population. Precision is defined as Standard Error divided by Mean.

Systematic errors are errors within the equipment such as measuring cylinders which may not be exact or scales which could be damaged and so give incorrect weights. Random errors are those made by human errors such as having parallax errors distorting measurements, temperatures in the room affecting results or slow reaction times when stopping a stop watch or placing things in solutions. Systematic and random errors can be reduced by many repeats of the whole experiment and then averaging the results and also, decreasing as many variables as possible by using precise

In this lab a acid-base indicator phenolphthalein was used to determine endpoint of a reaction HCl(aq) and KOH(aq). At the end point all of the HCl(aq) would have reacted with KOH(aq), and the pH becomes 7. The phenolphthalein would changed colours from colourless to pink indication when enough KOH(aq) was added. The purpose of numerous trials was to use the average volume of the 3 trials with similar measurements.