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An analytical chemist is titrating 192.3 mL of a 0.2200M solution of ethylamine (CH5NH) with a 0.6400M solution of HNO3. The pK, of ethylamine
An analytical chemist is titrating 192.3 mL of a 0.2200M solution of ethylamine (CH5NH) with a 0.6400M solution of HNO3. The pK, of ethylamine 3.19. Calculate the pH of the base solution after the chemist has added 7.9 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 = X
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Calculating the pH of the ethylamine solution after adding HNO3 1 Initial moles of ethylamine Molari...
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General Chemistry
Authors: Darrell Ebbing, Steven D. Gammon
9th edition
978-0618857487, 618857486, 143904399X , 978-1439043998
