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Data of HCl Trial 1: volume of HCl =0.82l Volume of NaOH =22.1ml Trial 2: volume of HCl=0.821ml Volume of NaOH = 22.2ml Trial 3: volume of HCl= 0.821ml Volume NaOH = 22.7ml 1) calculate the molarity of HCl for each trial and find the average molarity.

Data of HCl Trial 1: volume of HCl =0.82l Volume of NaOH =22.1ml Trial 2: volume of HCl=0.821ml Volume of NaOH = 22.2ml Trial 3: volume of HCl= 0.821ml Volume NaOH = 22.7ml 1) calculate the molarity of HCl for each trial and find the average molarity.

Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Data of HCl Trial 1: volume of HCl =0.82l Volume of NaOH =22.1ml Trial 2: volume of HCl=0.821ml Volume of NaOH = 22.2ml Trial 3: volume of HCl= 0.821ml Volume NaOH = 22.7ml 1) calculate the molarity of HCl for each trial and find the average molarity.
Procedure: A-Preparation of 100 mL of 0.10M HCI aisi You need to calculate the volume of concentrated HCI you need to take and dilute it with Water to make 100 mL of 0.10 M HCl. (density of concentrated HCl = 1.20 g/ml, mass percent = 37% by mass) B-Preparation of 200 mL of 0.10 M NAOH You need to calculate the mass of NaOH that you need to weigh and dissolve in 200 mL of water to make 200 mL of 0.10 M NaOH. Hint: NaOH pellets should be weighed on a watch glass, mix it well with water. (Caution: NaOH is very corrosive, do not spill and if you do, wash it off immediately with an excess of water.) C- Standardization of ~0.10M NaOH “Determining the concentration of NaOH" 1- Weigh duplicate samples of 0.50-0.60 g of previously dried standard KHP into 125 or 250- ml flasks. Dissolve each sample in ~25.0- ml in distilled water. 2 - Add 2-4 drops of phenolphthalein indicator. Titrate it with NaOH until the first appearance of a permanent, pink color. 3- If runs do not agree to about two parts per thousand, repeat for the third time and calculate the average of the two closest results. D- Standardization of HCl "Determining the concentration of HCl" 1- Use the NaOH solution that you prepared to determine the concentration of HC. 2- Add 2-4 drops of phenolphthalein indicator to a 25.0 mL of the previously prepared HCl and titrate with the NaOH solution until the first appearance of a permanent pink color. 3- 3- If runs do not agree to about two parts per thousand, repeat for the third time and calculate the average of the two closest results.
Transcribed Image Text:Procedure: A-Preparation of 100 mL of 0.10M HCI aisi You need to calculate the volume of concentrated HCI you need to take and dilute it with Water to make 100 mL of 0.10 M HCl. (density of concentrated HCl = 1.20 g/ml, mass percent = 37% by mass) B-Preparation of 200 mL of 0.10 M NAOH You need to calculate the mass of NaOH that you need to weigh and dissolve in 200 mL of water to make 200 mL of 0.10 M NaOH. Hint: NaOH pellets should be weighed on a watch glass, mix it well with water. (Caution: NaOH is very corrosive, do not spill and if you do, wash it off immediately with an excess of water.) C- Standardization of ~0.10M NaOH “Determining the concentration of NaOH" 1- Weigh duplicate samples of 0.50-0.60 g of previously dried standard KHP into 125 or 250- ml flasks. Dissolve each sample in ~25.0- ml in distilled water. 2 - Add 2-4 drops of phenolphthalein indicator. Titrate it with NaOH until the first appearance of a permanent, pink color. 3- If runs do not agree to about two parts per thousand, repeat for the third time and calculate the average of the two closest results. D- Standardization of HCl "Determining the concentration of HCl" 1- Use the NaOH solution that you prepared to determine the concentration of HC. 2- Add 2-4 drops of phenolphthalein indicator to a 25.0 mL of the previously prepared HCl and titrate with the NaOH solution until the first appearance of a permanent pink color. 3- 3- If runs do not agree to about two parts per thousand, repeat for the third time and calculate the average of the two closest results.
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