Straight-forward%20buffers - 2 to 0.12 M Is this consistent...

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CHEM 1212 Straight-forward Buffers Equations pH = - log [H 3 O + ] pK a = - log K a + = - HA A log pK pH a Consider a 1.0 L buffer solution that is 0.10 M HNO 2 and 0.10 M NO 2 - The K a of HNO 2 is 4.5 * 10 -4 1. Begin by labeling the weak acid and the conjugate base: 2. Using the equation above solve for the pH of this buffer solution 3. Now consider if acid is added to the buffer solution. Write a chemical reaction showing how acid reacts with the buffer (consult your notes if you’re not sure): 4. The addition of 0.02 mol of HCl to this buffer will reduce the concentration of NO 2 - to 0.08 M and it will raise the concentration of HNO
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Unformatted text preview: 2 to 0.12 M. Is this consistent with the reaction you wrote in question 3? 5. Solve for the pH of the buffer solution after the HCl has been added: *********************************************************************** * 6. What is the pH of pure water? 7. When 0.02 mol of HCl is added to 1.0 L of pure water, the resulting concentration of [H 3 O + ] = 0.02 M. What is the pH of the resulting solution? 8. Compare the pH changes of adding acid to the buffer versus adding acid to pure water and solve which has a larger change?...
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