Question
What volumes of 0.53 M HNO2 and 0.46 M NaNO2 must be mixed to prepare 1.00 L of a solution buffered at pH = 3.55?
HNO2
HNO2
Answers
Use the Henderson-Hasselbalch equation.
pH = pKa + log (base/acid)
You must look up Ka and substitute pKa.
pH = pKa + log (base/acid)
You must look up Ka and substitute pKa.
228mL
452mL
452mL
Related Questions
Buffers- Common Ion effect
IS this Correct
Calculate the pH of a aqueous solution containing 0...
You have solutions of 0.200 M HNO2 and 0.200 M KNO2 (Ka for HNO2 = 4.00 10-4). A buffer of pH 3.00...
You have solutions of 0.200 M HNO2 and 0.200 M KNO2 (Ka for HNO2 = 4.00 10-4). A buffer of pH 3.00...
What volumes of 0.46 M HNO2 and 0.54 M NaNO2 must be mixed to prepare 1.00 L of a solution buffered...