Phenolphthalein, a colorless weak acid (K3 = 6.31 x 1010) which dissociates in water forming pink anions is widely considered a suitable indicator for this titration. Along with a suitable calculation, find the working/useful range of this indicator to explain its use.
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- 50.0 mL of 0.31 M acrylic acid (C2H3COOH, Ka = 1.71 x 10 ) solution is titrated with 0.31 M NaOH to the equivalence point. The %3D reactants are completely transformed into sodium acrylate C2H3COONA at this point. What is the pH of the titration solution at equivalence point? Please keep your answer to two decimal places.3 A 0.6423 g sample that might contain NaOH, Na₂CO₃, NaHCO₃, or a permissible mixture of the bases is titrated with 0.1062 M HCl by the double indicator method. It is found that 40.83 mL of the acid are required to reach the phenolphthalein end point. Methyl orange is then added to the solution and the titration continued using an additional 12.38 mL of the acid. Calculate the percentage of each component in the sample.When 30.00 mL of 0.1011 M HCl in 50 mL of deionized water is titrated against 0.09889 M NaOH, the pH increases. Find the pH when the volume of NaOH added is 0.02 mL more than the volume required to reach the equivalence point. Comment on the significance of the changes in pH values in relation to the increments of sodium hydroxide added when going “through” the endpoint.
- Calculate the pH at the equivalence point for the titration of 0.25 M CH3COOH with 0.25 M NaOH. (For CH3COOH, K₂= 1.8 x <10-5.) Hint: This is the pH of a salt solution. Assume the concentration of CH3COONa is 0.125 M. Kw = K₂ x Kb = 1.0 x 10-14 8.92 8.72 8.52 8.32 None of the aboveA 1.43 x 10-4 L solution of 45.7 mg/mL protein was analyzed using the Kjeldahl procedure. After digestion of the protein, the liberated NH3 was collected in 9.80 mL of 0235 M HCl. The unreacted acid required 10.75 mL of a standard solution of 0.0149 M NaOH for complete titration. Calculate the weight percent of nitrogen in the protein. (Molar mass N = 14.00674 g/mol)Malonic acid is a dicarboxylic acid with structure CH2(COOH)2 with Ka1 and Ka2 = 2.0 × 106. Consider the titration of 50.0 mL of 0.2 M disodium malonate = 1.5 x 10-3 (N22CH2(COO)2) by 0.2 M HCI and answer the following questions. Calculate the pH after the following total volumes of HCI have been added. a) 0.0 mL b) 25.0 mL c) 50.0 mL d) 75.0 mL e) 100.0 mL f) 110.0 mL
- A 50.0 mL of acidic solute (Ka = 1.20 x 10-2) is titrated with a 2.50 mL of 1.00 x 10-5 M NaOH solution. Which of the following indicators would be best for this titration? Indicator pKa methyl orange methyl red bromocresol purple bromthymol blue thymol blue phenolpthalein 3.46 5.00 6.12 7.10 8.90 9.10A 300mg sample containing Na2CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1M HCl. The titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67mL to reach the methyl red end point. Determine the composition of the sample and calculate the percent of each titrated component.A 300 mg sample containing Na2CO3, NaHCO3 and NaOH and inert material either alone or in some combination was dissolved and titrated with 0.1M HCl. The titration required 24.41 mL to reach the phenolphthalein endpoint. And an additional 8.67mL to reach the methyl red end point. Determine the composition of the sample and calculate the percent of each titrated component.
- How many grams of potassium napthenate (KC11H7O2; MW=210.27 g/mole; Kb=85x10-10) must be added to 50.0 ml of 0.4 M Naphthenic acid (HC11H7O2; Ka=5.4x10-5) to obtain a buffer with pH 5.0?explain each of the following cases. a) when we treat 1 mol / liter of hydrochloric acid, the pH increases. There comes a cast that the pH reaches a certain value and does not change anymore. Why does this happen? b) Methyl orange can be used to determine the final titration point of nitric acid with ammonia solution, while phenophthalein is not used in this case. Why? c) pH of 10-8 mol / l HCl is not 8. Why?A sample containing the amino acid alanine, CH3CH(NH2)COOH, plus inert matter is analyzed by Kjeldahl method. A 2.00 g sample is digested, the ammonia is distilled and collected in 50.0 ml of 0.150 M H2SO4, and a volume of 9.0 ml of 0.100 M NaOH is required for back titration. Calculate the percent alanine in the sample.