Arsenic acid is a triprotic acid with the pKa values pK₁1 = 2.240, pKa2 = 6.960, and pK₁3 = 11.500. You wish to prepare 1.000 L of a 0.0200 M arsenate buffer at pH 6.840. To do this, you choose to mix the two salt forms involved in the second ionization, NaH₂ AsO4 and Na₂HASO4, in a 1.000 L volumetric flask and add water to the mark. What mass of each salt will you add to the mixture? 2.43 mass NaH₂ AsO4 = g mass Na₂HASO4 = g Incorrect 0.9574 Incorrect

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Q: What ratio of NaCN to HCN is needed to prepare a pH 9.90 buffer? (Ka of HCN is 4.9 × 10⁻¹⁰)

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Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.