Buffer solution-ph and concentration

Question

Discussion:

Buffer Solution, pH and Concentration

1- Solve an equilibrium problem (using an ICE table) to calculate the pH of each solution:a solution that is 0.165M in HC₂H₃O₂ and 0.120M in KC₂H₃O₂. Express your answer using two decimal places.

2- A buffer contains significant amounts of ammonia and ammonium chloride.Write an equation showing how this buffer neutralizes added acid (HI). Express your answer as a chemical equation.

3- A buffer contains significant amounts of ammonia and ammonium chloride. Write an equation showing how this buffer neutralizes added base (CsOH). Express your answer as a chemical equation.

4- Determine whether mixing each pair of solutions results in a buffer.

75.0 mL of 0.10 MHF ; 55.0 mL of 0.15 MNaF
150.0 mL of 0.10 MHF ; 135.0 mL of 0.175 MHCl
150.0 mL of 0.10 MHF ; 135.0 mL of 0.175 MHCl

5- A 1.0-L buffer solution is 0.105M in HNO₂ and 0.145M in NaNO₂ . Determine the concentrations of HNO₂ and NaNO₂ after addition of 1.4g HCl .