A buffer solution was prepared by mixing 0.1M K2HPO2 and 0.1M KH2PO4 (pH 6.64) - calculate the ionic strength (I) of the standard phosphate buffer solution
According to the Henderson-Hasselbulch equation:
pH = pKa + Log[K2HPO4]/[KH2PO4])
i.e. 6.64 = pKa + Log(0.1/0.1)
i.e. pKa = 6.64
i.e. pH = pKa
In the case of pH = pKa, the ionic strength (I) of the buffer solution = 0
A buffer solution was prepared by mixing 0.1M K2HPO2 and 0.1M KH2PO4 (pH 6.64) - calculate...
0.1M K2HPO4 and 0.1M KH2PO4 was used to make a buffer- calculate the ionic strength of the standard phosphate buffer solution with a pH of 6.64
Calculate the ionic strength of the standard phosphate buffer solution with a pH of 6.64 when 0.1M K2HPO4 and 0.1M KH2PO4 was used to make the buffer
A buffer at pH 7.45 is prepared by mixing solutions of KH2PO4 and K2HPO4. Which of the following ratios of [base]/[acid] is required? For phosphoric acid, Ka1 = 7.5 × 10-3 Ka2 = 6.2 × 10-8 Ka3 = 4.2 × 10-13 [base]/[acid] = 1.75 [base]/[acid] = 1.24 [base]/[acid] = 0.57 [base]/[acid] = 1.27 [base]/[acid] = 0.79
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