An 80 mL sample of 0.200 M ammonia is titrated with 0.100 M HCl. K_b for ammonia is 1.8*10^-5. Calculate the pH of the solution at each of the following points of the titration:

a) before the addition of any HCl

b) halfway to the equivalence point

c) at the equivalence point

d) after the addition of 175 mL of 0.100 M HCl

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A 50.0-mL sample of a 0.100 M solution of NaCN is titrated by 0.200 M HCl.

K_b for CN− is 2.0×10⁻⁵. Calculate the pH of the solution:

Prior to the start of the titration
After the addition of 15.0 mL of 0.200 M HCl
At the equivalence point
After the addition of 30.0 mL of 0.200 M HCl

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25.0 mL of a 0.100 M NH3 is titrated with a strong acid. 0.100 M HCl. Calculate the pH of the NH3 solution at the following points during the titration: (Kb= 1.8 x 10^-5) A. Prior to the addition of any HCl. B: After the addition of 10.5 mL of a 0.100 M HCl. C: At the equivilance point. D: After the addition of 3 mL of 0.100 M HCl. Show your work.

Rank the following titrations in order of increasing pH at the halfway point to equivalence (1 = lowest pH and 5 = highest pH).

1. 200.0 mL of 0.100 M HC₂H₃O₂ (K_a = 1.8 x 10^-5) by 0.100 M NaOH

2. 100.0 mL of 0.100 M HF (K_a = 7.2 x 10^-4) by 0.100 M NaOH

3. 200.0 mL of 0.100 M (C₂H₅)₂NH (K_b = 1.3 x 10^-3) by 0.100 M HCl

4. 100.0 mL of 0.100 M HI by 0.100 M NaOH

5. 100.0 mL of 0.100 M NH₃ (K_b = 1.8 x1 0^-5) by 0.100 M HCl

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