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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Phosphoric add can supply one, two, or three H3O+ ions in aqueous solution. Write balanced equations (like those for sulfuric acid on page 142) to show this successive loss of hydrogen ions.

Interpretation Introduction

Interpretation:

The balanced equation for the ionization of Phosphoric acid in water should be given.

Concept introduction:

The law of conservation of mass states that no atoms can be created or destroyed in a chemical reaction, therefore, the number of atoms present in the reactants is equal to the number of atoms present in the products.

Bronsted acid: An acid donates (loses)H+ ion.

Bronsted Base: A base accepts (gains)H+ ion.

Explanation

  

Phosphoric acid is a triprotic acid (it contains three ionizable hydrogens).  Phosphoric acid gives the H+ ion to water molecule and forms the hydronium ion (H3O+) and dihydrogen phosphate (H2PO4-).  Here Phosphoric acid behaves as acid because it donates the proton to the water molecule therefore water molecule behaves as a base (it abstract the proton), the balanced equation for the Phosphoric acid in water is given above.

  

Dihydrogen phosphate (H2PO4-) gives the H+ ion to water molecule and forms the hydronium ion (H3O+) and dihydrogen phosphate (HPO4-)

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