1.) Consider the following salt solutions all at the same concentration. NaHCO 3

Question

1.) Consider the following salt solutions all at the same concentration. NaHCO3, NaCl, MgBr2, NaCN, NaNO3.

Evaluate the acid/base strengths of the ions and determine:

Which salt is the most acidic?

Which salt is the most basic?

Hint: Usually, anions like X- are bases. However, some negative ions like HX- can be weak acids.

Which salts have a neutral pH? (Check all of the right aswers.)

NaCl

NaCN

MgBr2

NaHCO

NaNO3

2.)Consider the reactions below:

Which of these species are Arrhenius acids?

H-

Mg(OH)2

HBr

HCl

OCl-

H2O

Which of these species are Arrhenius bases?

HCl

H-

H2O

Mg(OH)2

HBr

OCl-

Which of these species are Lowry Bronsted acids?

Mg(OH)2

OCl-

HBr

HCl

H2O in reactions 3 and 5

H-

Which of these species are Lowry Bronsted bases?

OCl-

H2O in reaction 1

H-

HBr

Mg(OH)2

HCl

3.) Based on their compositions and structures and on conjugate acid-base relationships, select the stronger base in each of the following pairs.

a.) NO2? or NO3?

b.) PO43? or AsO43?

c.) HS? or Cl?

2.

Explanation / Answer

Answer 1)

most acidic- NaHCO3

most basic- NaCN

Answer 2) hcl ,hbr, Arrhenius acid is a substance that dissociate in water to form H+ ions

Mg(OH)2 , OCl-,h- Arrhenius base is a substance that dissociate in water to form OH- ions.

Answer 3) Hbr , Hcl , are bronsted acid that donates the proton .

OCl- , H- , Mg(OH)2 they are bronsted base that accept proton .

Answer 3) NO2-

b)PO43-

c) Cl-

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