#30 Calculate the pH of a solution prepared from 1.0 mole NH3 and 1.5 mole NH4Cl dissolved in 5.0L of water. (For NH3, Kb=1.8x10^-5)

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17 Dec 2019

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A basic buffer is prepared by adding 0.1583g of NH₄Cl (MM = 53.4915 g/mol) to 1.00L of 0.1929 M NH₃. K_b (NH₃) = 1.8x10^-5. Calculate the pH.
Answer in 3 decimal places

50.0 mL of .50M NaOH is added to a 250mL solution containing .30M NH3 and .36 NH4Cl. What is the pH of the resulting solution?

Kb of NH3= 1.8x10-5

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Determine the value of [OH-] in a solution prepared by dissolving 0.005 mole of ammonia and so many of pyridine, in enough water to have 200 ml of solution
Kb NH3 = 1.8x10 ^ -5
Kb Pyridine = 1.5 x 10 ^ -9
What are the concentrations of ammonium and pyridinium ions?
Answer: [OH -] = [NH4 +] = 7 x10 ^ -4 M
[Ion Piridinio] = 5x10 ^ -8 M

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#30 Calculate the pH of a solution prepared from 1.0 mole NH3 and 1.5 mole NH4Cl dissolved in 5.0L of water. (For NH3, Kb=1.8x10^-5)

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