1. Write two sets of definitions, each including one for acids and one for bases

Question

1. Write two sets of definitions, each including one for acids and one for bases: a) The Arrhenius definitions b) The Brønsted-Lowry definitions 2. Write the formula for the conjugate base for each of the following: a) HCl b) H20 c) H2PO4 ) NH4 3. Write the formula for the conjugate acid for each of the following: a) F b) H,O c) H2PO4 d) CH NH2 4. Write the dissociation reaction for perchloric acid, HCIO4, and identify conjugate acid-base pairs. 5. Write an equilibrium expression for the equation in question 4.

Explanation / Answer

Ans 1

a)As defined by Arrhenius, acid-base reactions are characterized by acids, which dissociate in aqueous solution to form hydrogen ions (H+) and bases, which form hydroxide (OH) ions.

b)In Brønsted theory, acids are defined as proton donors; whereas bases are defined as proton acceptors.

Ans 2.

a) Cl-

b) OH-

c) HPO42-

d)NH3

Ans 3)

a)HF

b)H3O+

c) H3PO4

d)CH3NH3+

Ans 4.

HClO4(l) + H2O —-> H3O+(aq) + ClO4-(aq)

In this case, the acid is perchloric acid and its conjugate base is the perchlorate ion (ClO4-) .

Ans 5 .HClO4 is a very strong acid. It will dissociate fully in aqueous solution. Therefore it does not have a Ka value. The Ka value is used exclusively with weak acids that dissociate only partially.

Related Questions

Navigate

• Browse (All)
• Browse 1
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.