What is the pH of a buffer made from 0.580 mol of CH3NH2 (Kb = 4.4 x 10-4) and 0.250 mol of CH3NH3I?

Write the buffer equilibrium reaction, then write the neutralization reaction. What isthe pH of the 0.20M NH3/NH4CL buffer after the addition of 10.0 mL of 0.10 HCl to65.0 mL of buffer? The Ka for NH3 is 5.6 x 10-10

A 25.0 mL sample of 0.450 M (CH3)2NH is titrated with HBr. What is the pH of the solution after 30.0 mL of 0.375 M HBr have been added to the methylamine solution? ((CH3)2NH; Kb Give answer to 2 decimal places. = 5.9×10-4)

What is the pH of the buffer that results when 2.3 g of NH3 and 6.46 g of NH4Cl are dissolved in 250 mL water? (Ka for NH4+ = 5.60 × 10-10) Please give the answer to 2 decimal places.

A buffer solution is 0.397 M in H2 S and 0.382 M in KHS. If Kai for H2S is 1.0 × 10-7, what is the pH of this buffer solution? pH =

The pK, value for HCN is 9.40. Would a buffer prepared from HCN and KCN with a pH of 11.4 be considered to be an effective buffer? A buffer in which the mole ratio of KCN to HCN is 0.60 has a pH of 9.18. Would this buffer solution have a greater capacity for added acid (H30*) or added base (OH )?

A buffer solution is 0.402 M in H2CO3 and 0.314 M in KHCO3. If Kal for H2CO3  is 4.2 X 10 -7 , what is the pH of this buffer solution? pH =

45.0 mL of a buffer solution contains 0.20 M CH3COOH and 0.25 M CH3COONa. What is the pH of the mixture after 18.0 mL of 0.45 M HCI is added to this buffer solution? Ka of CH3COOH = 1.8 x 10-5.

What is the pH of a buffer made from 0.580 mol of CH3NH2 (Kb = 4.4 x 10-4) and 0.260 mol of CH3NH31?