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# Buffer Solution, pH and Concentration

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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.

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 .

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This solution offers succinct and logical answers to some problems related to buffer solution and all steps of the calculation are shown.

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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. ...

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