11.(a) 10.06 cm3 of the stock 0.100 mol dm–3 solution of NaOH was required to fully neutralise 49.5 mg of a diprotic acid (H2A). Write a balanced equation for this reaction and hence determine the molar mass (Mr) of the acid. (b) Determine the pH of 0.100 mol dm–3 NaOH at 298 K [pKw = 14.0].
11.(a) 10.06 cm3 of the stock 0.100 mol dm–3 solution of NaOH was required to fully neutralise 49.5 mg of a diprotic acid (H2A). Write a balanced equation for this reaction and hence determine the molar mass (Mr) of the acid. (b) Determine the pH of 0.100 mol dm–3 NaOH at 298 K [pKw = 14.0].
Chapter10: Effect Of Electrolytes On Chemical Equilibria
Section: Chapter Questions
Problem 10.8QAP
Related questions
Question
11.(a) 10.06 cm3 of the stock 0.100 mol dm–3 solution of NaOH was required to fully neutralise 49.5 mg of a diprotic acid (H2A). Write a balanced equation for this reaction and hence determine the molar mass (Mr) of the acid.
(b) Determine the pH of 0.100 mol dm–3 NaOH at 298 K [pKw = 14.0].
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 2 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you