Chemistry

Chemistry

Problem

For which of the following aqueous solutions of a monoprotic weak acid HA is it MOST reasonable to treat the equilibrium concentration of HA as essentially equal to its initial concentration when calculating the pH? a) 0.050 M HA with Ka=6.0×10−40.050\,\text{M } \text{HA with }K_a = 6.0\times10^{-4} b) 0.050 M HA with Ka=2.0×10−90.050\,\text{M } \text{HA with }K_a = 2.0\times10^{-9} c) 0.050 M HA with Ka=2.0×10−40.050\,\text{M } \text{HA with }K_a = 2.0\times10^{-4} d) 0.00050 M HA with Ka=6.0×10−40.00050\,\text{M } \text{HA with }K_a = 6.0\times10^{-4}

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