# 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 HC 2 H 3 O 2 and 0.120M in KC 2 H 3 O 2. 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.

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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 HNO 2 and 0.145M in NaNO 2 . Determine the concentrations of HNO 2 and NaNO 2 after addition of 1.4g HCl .

Ionics Part 2
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.
You can use the ICE table method to do it … or you can use the ‘x is small’ method. Using the Henderson Hasselbach equation:
pH = pKa + log [ base / acid ] (tricky part is knowing which is base and which is acid)
pH = – log(1.8 * 10^-5) + log (0.120/ 0.165) = 4.61

2- A buffer contains significant amounts of ammonia and ammonium chloride. …

Solution Summary
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