Question

In: Chemistry

1. Calculate the pH of a solution that is 0.060 M in potassium propionate (C2H5COOK or...

1. Calculate the pH of a solution that is 0.060 M in potassium propionate (C2H5COOK or KC3H5O2) and 0.090 M in propionic acid (C2H5COOH or HC3H5O2).

2. Calculate the pH of a solution that is 0.080 M in trimethylamine, (CH3)3N, and 0.12 M in trimethylammonium chloride, ((CH3)3NHCl).

3. Calculate the pH of a solution that is made by mixing 50.0 mL of 0.15 M acetic acid and 50.0 mL of 0.21 M sodium acetate.

Expert Solution

1. [CH3CH2COO] = 0.09M

[CH3CH2COOK] = 0.06M

PKa = 4.87

PH = PKa + log[CH3CH2COOK]/[CH3CH2COOH]

= 4.87 + log0.06/0.09

= 4.87 -0.176 = 4.694

2. [(CH3)3N] = 0.08M

[(CH3)NHCl] = 0.12M

Pkb = 4.194

POH = Pkb + log [(CH3)NHCl] / [(CH3)3N]

= 4.194 + log0.12/0.08

= 4.194 + 0.176 = 4.37

PH = 14-POH

= 14-4.37 = 9.63

3. no of moles of CH3COOH = molarity * volume in L

= 0.15*0.05 = 0.0075 moles

no of moles of CH3COONa = molarity * volume in L

= 0.21*0.05 = 0.0105moles

PH = Pka + log[CH3COONa]/[CH3COOH]

= 4.75 + log0.0105/0.0075

= 4.75 + 0.146 = 4.896 >>>>answer

queen_honey_blossom answered 1 year ago

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