A student needs to prepare a buffer solution with a pH of 5.52. Assuming a pK₂ of 4.07, how many mL of 0.1 M B would need to be added to 25.0 mL of 0.1 M HB prepare this buffer?

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A student needs to prepare a buffer solution with a pH of 5.52. Assuming a pK₂ of 4.07, how many mL of
0.1 M B would need to be added to 25.0 mL of 0.1 M HB prepare this buffer?
Please include a proper (abbreviated) unit.
HINT: Use pH = pK₂ + log ([B minus]/[HB]) or, if concentrations are the same,
pH = pka + log (Volume of B minus/ Volume of HB)
Transcribed Image Text:A student needs to prepare a buffer solution with a pH of 5.52. Assuming a pK₂ of 4.07, how many mL of 0.1 M B would need to be added to 25.0 mL of 0.1 M HB prepare this buffer? Please include a proper (abbreviated) unit. HINT: Use pH = pK₂ + log ([B minus]/[HB]) or, if concentrations are the same, pH = pka + log (Volume of B minus/ Volume of HB)
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