1.Write the acid dissociation reaction for following solutions, and calculate th

ID: 898034 • Letter: 1

Question

1.Write the acid dissociation reaction for following solutions, and calculate the pH for each of them:

a.0.001 M HCl

b.0.005 M H2SO4

c.0.005 M KOH

2.A solution is prepared by dissolving 0.001 Mole of NaCOOCH3 (NaAc) into 1 L DI water. Answer the following questions:

a.Write all the dissociation reactions for this solution

b.Write mass balance for this solution

c.Write charge balance for this solution

d.Write proton condition for this solution

e.Calculate the pH of the solution

3.Answer the questions in problem 1. (a – e), if the solution is prepared by dissolving 0.001 mole of HAc into 1 L DI water.

4.Answer the questions in problem 1. (a – e), if the solution is prepared by dissolving 0.0005 mole of HAc and 0.0005 mole of NaAc into 1 L DI water.

1) a) HCl (aq) --------> H3O+ (aq) + Cl- (aq)

pH = -log[H3O+] = - log (0.001) = 3.0

b) H2SO4 (aq) -------------> 2 H+ (aq) + SO42- (aq)

pH = -log[H3O+] = -log(2*0.005) = -log(0.01) = 2.0

c) KOH (aq) ------------> K+ (aq) + OH- (aq)

pOH = -log[OH-] = -log (0.005) = 2.30

2) a) CH3COONa (aq) ----------> CH3COO- (aq) + Na+ (aq)

b) 0.001 [ CH3COONa] = 0.001 [CH3COO-]

c) [CH3COO-] + [OH-] = [Na+]

d) proton concentration is very less as the resultant solution is basic in nature.

e) pH = 14 - pOH

Where- [OH-] = (Kb*concentration)1/2 = (5.62*10-10* 0.001 )1/2 = 7.49*10-7 M

pOH = -log [OH-] = - log (7.49*10-7) = 6.12

pH = 14-6.12 = 7.9

3) a) AcOH (aq) <------> AcO- (aq) + H+ (aq)

b) [AcO-]total = [AcOH] + [AcO-]

c) [H+] = [AcO-]

d) proton concentration is very less as the resultant solution is basic in nature.

e) [H+] = (Ka*C)1/2 = (1.8*10-5) *(0.001) ]0.5 = 1.34*10-4 M

pH = -log [H+] = 3.87

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