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18 Nov 2019
please answer Ph of diluted HCL solution and A-E ..PLEASE!! ..ooo Verizon LTE 10:46 AM 84%. genchem.rutgers.edu 1. You add Hydrochloric Acid to distilled water. If all the HCI dissociates in solution, calculate the pH of the final solution given the following data. (assume the liquid volumes are asaative) Volume of distilled water used 25.74 mL Volume of HCI added 0.76 mL, 1.531 M Concentration of added HCI pH of diluted HCI solution 2. You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured with a pH meter. The "neutralized" solution is added to the "original" solution and the pH of this combined "final" solution is also measured. The following are the measured values: Mass of unknown acid 1.4949 g 12.02 mL Volume of NaOH used in titration Concentration of the NaOH used 0.2153 M pH of the original acid solution 2.37 3.68 pH of the final acid solution CALCULATE the following (a) Molecular Weight ofAcid used in titration (b) Molarity of UNKNOWN Acid solution from itration (c) Ka of UNKNOWN Acid (d) Concentration of undissociated Acid from pH measurements (e) Total concentration of N acid from pH measurements
please answer Ph of diluted HCL solution and A-E ..PLEASE!!
..ooo Verizon LTE 10:46 AM 84%. genchem.rutgers.edu 1. You add Hydrochloric Acid to distilled water. If all the HCI dissociates in solution, calculate the pH of the final solution given the following data. (assume the liquid volumes are asaative) Volume of distilled water used 25.74 mL Volume of HCI added 0.76 mL, 1.531 M Concentration of added HCI pH of diluted HCI solution 2. You weigh a sample of a monoprotic unknown acid and dissolve it in 50.00 mL of distilled water. Exactly half of this solution is titrated with Sodium Hydroxide to the phenolphthalein end point. The pH of the other half of the original solution is measured with a pH meter. The "neutralized" solution is added to the "original" solution and the pH of this combined "final" solution is also measured. The following are the measured values: Mass of unknown acid 1.4949 g 12.02 mL Volume of NaOH used in titration Concentration of the NaOH used 0.2153 M pH of the original acid solution 2.37 3.68 pH of the final acid solution CALCULATE the following (a) Molecular Weight ofAcid used in titration (b) Molarity of UNKNOWN Acid solution from itration (c) Ka of UNKNOWN Acid (d) Concentration of undissociated Acid from pH measurements (e) Total concentration of N acid from pH measurements
Lelia LubowitzLv2
27 May 2019