If 0.50 L of a buffer containing 1.0 mol H2PO4-and 1.0 mol HPO4-2 is diluted to a volume of 5.0 L, how much would the pH change?

1000 mL of a buffer solution contains 0.275 moles of HCN, and 0.175 moles of NaCN. Ka of HCN = 6.2 x 10^-10.a) calculate the initial pH b) calculate the pH of the buffer after the addition of 27.5 L of 1.0 M of HCl. c) what is the change in pH of the solution if the same amount of Hcl which was used in part (b) were added to 1000 mL pure water.

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

Which of the following, if dissolved in 1.0 L of pure water, will produce a buffer solution? 0.1 mole HCL + 0.1 mole KCl 0.1 mole NaH2PO4 + 0.1 mole Na2HPO4 0.1 mole NaCl + 0.1 mole KCl 0.1 mole of H3O+ + 0.1 mole OH- I am guessing option 2, but need clarification please!