2) what is the PH of solutions containing naOh, nacO3, nh3, and nh4cl. Explain y

Question

2) what is the PH of solutions containing naOh, nacO3, nh3, and nh4cl. Explain your results with chemical reactants B. Base and Basic salutions 1. Reaction aqueous sodium hydroside with acid Describe your chservations 2. Dissolution ofsodium hydrovide Descrite your berwins 3 Dissolution of sodium carbonate Describe your observatoes, write equation that for your pll Measurements Briefly account for the if nur equal 7 Boiled, deionized *e fH goes to a base Unboilod, deionized Approsimae pH Balanced equatioe showing acidity basicity a010 M HCI 0010 MCH COOH 0 AM NaOH 0.010 M NH ovinegar Lemon juice Household ammonia Detergent solution 112 Acids, Bases, and Sals

Explanation / Answer

1) HCl is a stronger acid than acetic acid as HCl will dissociate completely.

It dissociates completely as water molecule assist in its dissociation(solvolysis) and can break bond between H+ and Cl- by hdyrating them. While water molecules cannot hydrate well O-H bond in acetic acid hence the acid is weaker.

Also, Cl- (the conjugate base) is weak base as compared to CH3COO-, which is a strong base.

HCl + H2O ---> H3O+ + Cl-

CH3COOH + H2O --> CH3COO- + H3O+

2

a) HCl will completely dissoicate into ions

[H+]= [HCl] = 0.01 M

pH = -log[H+] = -log0.01 = 2

b) for naOH, it will also dissociates completely

[OH-] = [NaOH] = 0.01

pOH = -log[OH-] = 2

pH = 14-pOH = 12

c) NH3

The Kb = 1.8 X 10^-4

[OH-] = (Kb X concentration)^1/2 = (1.8 X 10^-5 X 0.01 )^1/2 = 4.24 X 10^-4

pOH = -log[OH-] = 3.37

pH = 14-pOH = 14-3.37 = 10.63

d) Na2CO3 --> 2Na+ + (CO3)-2

Then the carbonate ions will react with water as
CO3-2 + H2O ---> HCO3- + OH-
[OH-] = (Kb X concentration)^1/2 = (2 X 10^-4 X 0.01)^1/2 = 1.414 X 10^-3

pOH = 2.85

pOH = 14-2.85 = 11.15

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