If the volume of the vinegar used is 8.05 mL, the molarity of acetic acid is 1.02 mmol / 8.05 mL = 0.127 M. In this experiment, a carefully measured volume of vinegar (V analyte) is placed into a beaker and the mass determined. To determine the concentration of an unknown acid. Acid-Base Titration Lab April 18 2017 I. Titration Curves of Strong and Weak Acids and Bases Goals To calibrate a pH probe. To become familiar with acid-base titration curves. a) List the diagrams by letter in the order these mixtures would appear during the titration, beginning with the earliest and ending with the final mixture. C. It was used as a catalyst for the acid-base neutralization reaction. Write your answer with the correct number of significant figures. As a result, you will have a lower than actual concentration of the hydrochloric acid, meaning a larger percent error Determination of sodium hydroxide concentration is about as often discussed as hydrochloric acid titration - both acid and base are strong, so calculation of titration curve and equivalence point are pretty straightforward. This result is expected because a combination of strong acids and strong bases should result in a neutral at the equivalence point. Table 4 shows data for the titration of a 25.0-mL sample of 0.100 M hydrochloric acid with 0.100 M sodium hydroxide. It is the same idea with the transferring of the acid. If 25.31 mL of 0.0500 M NaOH solution are required to reach the equivalence point of an acid-base titration of 40.0 mL of 7-Up, how many moles of NaOH were required? A titration is a process used to determine the volume of a solution needed to react with a given amount of another substance. Purpose Be able to titrate a measured volume of HCl with a solution of NaOH of The values of the pH measured after successive additions of small amounts of NaOH are listed in the first column of this table, and are graphed in Figure 1, in a form that is called a titration curve. B. In this experiment, you will titrate hydrochloric acid solution, HCl, with a basic sodium hydroxide solution, NaOH. Stage 1 Using a small funnel, pour a few cubic centimetres of 0.4 M hydrochloric acid into the burette, with the tap open and a beaker under the open tap. To carry out an accurate titration using dilute hydrochloric acid, dilute sodium hydroxide solution, and phenolphthalein indicator. D. It was used to identify when the solution passed the equivalence point. Equipment and Materials 0.10 M ammonium hydroxide solution, 0.10 M sodium hydroxide solution, 0.0074 M hydrochloric acid Answer: Based on the data, the strong acid/strong base combination of hydrochloric acid and sodium hydroxide had the neutral pH at the equivalence point, being 7.11. With the residual water in the beaker, you are diluting the standardized sodium hydroxide solution. general remarks. Apparatus for titrating sodium hydroxide with hydrochloric acid to produce sodium chloride. View Acid Base Titration Lab.docx from CHE 2240 at St. John's University. The simplest acid-base reactions are those of a strong acid with a strong base. The concentration of the NaOH solution is given and you will determine the unknown concentration of the HCl. Using the values above, if titration requires 1.02 mmol of NaOH to reach the endpoint, the sample must also contain 1.02 mmol of acetic acid. titration of hydrochloric acid with sodium hydroxide as titrant. A. 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