Problem: Given the balanced equation representing a reaction: HSO4-(aq) + H2O(l) → H3O+(aq) + SO42-(aq) According to one acid-base theory, the H2O(l) molecules act as a. a base because they accept H+ ions b. a base because they donate H+ ions c. an acid because they accept H+ ions d. an acid because they donate H+ ions

🤓 Based on our data, we think this question is relevant for Professor Turnpenny's class at BU.

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Problem Details

Given the balanced equation representing a reaction: 

HSO4-(aq) + H2O(l) → H3O+(aq) + SO42-(aq) 

According to one acid-base theory, the H2O(l) molecules act as 

a. a base because they accept H+ ions 

b. a base because they donate H+ ions 

c. an acid because they accept H+ ions 

d. an acid because they donate H+ ions

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Our tutors have indicated that to solve this problem you will need to apply the Bronsted Lowry Acid and Base concept. You can view video lessons to learn Bronsted Lowry Acid and Base. Or if you need more Bronsted Lowry Acid and Base practice, you can also practice Bronsted Lowry Acid and Base practice problems.

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Based on our data, we think this problem is relevant for Professor Turnpenny's class at BU.