Hi, please help me complete trial 1, step-by-step. The lab is Acid-Base Titrations.

We mixed roughly 1 g of KHP and 10 mL water in a flask. Added drops of phenolphthalein indicator. Then titrated NaOH into flask containing KHP and H2O until it reached equivalence point.

Thank you

Part I. Standardization of NaOH solution: Trial #2 Trial #1 Measurements 0.470 g Mass of weighing paper 1.480 g Mass of weighing paper KHP Mass of KHP 1.01 g of moles of KHP 43 mL Initial buret reading 31 mL Final buret reading Volume of NaOH 12 mL of moles of NaOH Concentration of N Calculations KHP -204.44 g/mol

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Trinidad TremblayLv2

14 Jan 2019

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HCl (aq) + NaOH (aq) --> H2O (l) + NaCl (aq)

4.00 mL of an unknown acid solution containing HCl was added to flask containing 30.00 mL of deionized water and two drops of an indicator. The solution was mixed and then titrated with NaOH until the end point was reached. Use the following titration data to determine the mass percent of HCl in the acid solution.

Mass of flask: 125.59 g

Mass of flask + acid solution: 129.50 g

Initial volume of NaOH from buret: 0.15 mL

Final volume of NaOH from buret: 16.70 mL

Molarity of NaOH: 0.5458 M