In a sulfuric acid (H2SO4) - Sodium hydroxide (NaOH) acid-base titration, 17.3 mL of 0.126 M NaOH is needed to neutralize 25 mL of H2SO4 of unknown concentration. Find the molality of the H2SO4 solution, given that the neutralization reaction occurs is: H2SO4 (aq) + NaOH (aq) ----> Na2SO4 (aq) + H2O (l)
In a sulfuric acid (H2SO4) - Sodium hydroxide (NaOH) acid-base titration, 17.3 mL of 0.126 M NaOH is needed to neutralize 25 mL of H2SO4 of unknown concentration. Find the molality of the H2SO4 solution, given that the neutralization reaction occurs is: H2SO4 (aq) + NaOH (aq) ----> Na2SO4 (aq) + H2O (l)
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter15: Complex Ion And Precipitation Equilibria
Section: Chapter Questions
Problem 66QAP: The box below represents one liter of a saturated solution of the species , where squares represent...
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In a sulfuric acid (H2SO4) - Sodium hydroxide (NaOH) acid-base titration , 17.3 mL of 0.126 M NaOH is needed to neutralize 25 mL of H2SO4 of unknown concentration. Find the molality of the H2SO4 solution, given that the neutralization reaction occurs is:
H2SO4 (aq) + NaOH (aq) ----> Na2SO4 (aq) + H2O (l)
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