An unknown compound, X, is thought to have a carboxyl group with a pK₂ of 2.5 and a second ionizable group with a pKa between 5.0 and 8.0. When 50.0 mL of 0.2 M NaOH is added to 75.0 mL of a 0.2 M solution of X at pH 2.5, the pH increases to 7.13. Calculate the pK₂ of the second ionizable group of X. pK₂ = 6.97 Incorrect
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- An unknown compound, X, is thought to have a carboxyl group with a pKa of 2.0 and another ionizable group with a pKa between 5 and 8. When 75 mL of0.1 M NaOH is added to 100 mL of a 0.1 M solution of X at pH 2.0, the pH increases to 6.72. Calculate the pKa of the second ionizable group of XAn unknown compound, X, is thought to have a carboxyl group with a pK, of 2.5 and a second ionizable group with a pk₁ between 5.0 and 8.0. When 50.0 mL of 0.2 M NaOH is added to 75.0 mL of a 0.2 M solution of X at pH 2.5, the pH increases to 7.13. Calculate the pK, of the second ionizable group of X. pK₂ =What is the pH of a solution containing 0.50 moles of benzoic acid and 0.75 moles of sodium benzoate if the pka is 4.19?
- An analytical chemist is titrating 75.2 mL of a 0.5800 M solution of trimethylamine ((CH3)N) with a 0.2600M solution of HNO3. The p K₂ of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 197.6 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places. pH = 0 X 5 4Write the values of Y and X. H2SO4 CH3CH=CH2 + H2O CH;CH-CH2 H HỌ 2-propanol an alcohol The pKa of a protonated alcohol is about -2.5, and the pKa of an alcohol is about 15. Therefore, as long as the pH of the solution is greater than Y and less than X, more than 50% of 2-propanol will be in its neutral, nonprotonated form. Express your answers using two significant figures separated by a comma. AX中 Y, X = %3|The pK₂ of acetic acid, HC₂H3O2, is 4.96. A buffer solution was made using an unspecified amount of acetic acid and 0.1 moles of NaC2H3O2 in enough water to make 1.82 liters of solution. Its pH was measured as 4.04. How many moles of HC2H3O2 were used? Report your answer with 2 places past the decimal point. Do not put unit in your answer.
- An analytical chemist is titrating 198.9 mL of a 0.2300 M solution of diethylamine ((C,H5)¸NH) with a 0.1500 M solution of HNO3. The p K, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 357.1 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places.An analytical chemist is titrating 176.4 mL of a 0.2800M solution of trimethylamine ((CH₂), N) with a 0.7000M solution of HNO3. The pK of trimethylamine is 4.19. Calculate the pH of the base solution after the chemist has added 46.2 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. PH-0 = X 5An analytical chemist is titrating 248.4 mL of a 0.1600M solution of diethylamine ((C,H,) NH) with a 0.7200M solution of HNO3. The p K, of diethylamine 2 is 2.89. Calculate the pH of the base solution after the chemist has added 64.6 mL of the HNO, solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH = U ?
- An analytical chemist is titrating 226.0mL of a 0.8900M solution of diethylamine ((C2H5)2 NH) with a 0.6800M solution of HNO3. The pKb of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 92.3mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.b An analytical chemist is titrating 112.7 mL of a 0.6400M solution of ethylamine (C₂H5NH₂) with a 0.8100M solution of HNO3. The p K² of ethylamine is 3.19. Calculate the pH of the base solution after the chemist has added 21.5 mL of the HNO3 solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO3 solution added. Round your answer to 2 decimal places.An analytical chemist is titrating 118.6 mL of a 0.5800M solution of diethylamine ((C,H,) NH) with a 0.7600M solution of HNO3. The p K, of diethylamine is 2.89. Calculate the pH of the base solution after the chemist has added 37.4 mL of the HNO, solution to it. 3. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of HNO, solution added. Round your answer to 2 decimal places. pH