HO* (aq) + CHCHCOO (aq) K, 1.4 x 10 at 25C CHCHCOOH(aq) + OH(aq) K7.4 x...

 

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H₂O* (aq) + CH₂CH₂COO (aq) K, 1.4 x 10 at 25°C CH₂CH₂COOH(aq) + OH(aq) K7.4 x 10-10 at 25°C The acid equilibrium for CH₂CH₂COOH and the base equilibrium for CH₂CH₂COO are represented above. One liter of a buffer solution with pH 4.85 is made by mixing 0.100 M CH₂CH₂COOH and 0.100 M NaCH₂CH₂COO. if 10.0 mL of 0.500 M NaOH is added to the buffer, which of the following is most likely the resulting pH, and why? The pH will be much less than 4.85, because the buffer will respond to the addition of NaOH by producing more CH₂CH₂COOH. С CH₂CH₂COOH(aq) + H₂O(1) CH₂CH₂COO (aq) + H₂O(1) The pH will be much greater than 4.85, because there is a large increase in the concentration of the weak base, CH₂CH₂COO The pH will be slightly less than 4.85, because the addition of NaOH reduces the autoionization of H₂O. D The pH will be slightly greater than 4.85, because some CH₂CH₂COOH will react with the added bases, resulting in a slight decrease in (H₂O). H₂O* (aq) + CH₂CH₂COO (aq) K, 1.4 x 10 at 25°C CH₂CH₂COOH(aq) + OH(aq) K7.4 x 10-10 at 25°C The acid equilibrium for CH₂CH₂COOH and the base equilibrium for CH₂CH₂COO are represented above. One liter of a buffer solution with pH 4.85 is made by mixing 0.100 M CH₂CH₂COOH and 0.100 M NaCH₂CH₂COO. if 10.0 mL of 0.500 M NaOH is added to the buffer, which of the following is most likely the resulting pH, and why? The pH will be much less than 4.85, because the buffer will respond to the addition of NaOH by producing more CH₂CH₂COOH. С CH₂CH₂COOH(aq) + H₂O(1) CH₂CH₂COO (aq) + H₂O(1) The pH will be much greater than 4.85, because there is a large increase in the concentration of the weak base, CH₂CH₂COO The pH will be slightly less than 4.85, because the addition of NaOH reduces the autoionization of H₂O. D The pH will be slightly greater than 4.85, because some CH₂CH₂COOH will react with the added bases, resulting in a slight decrease in (H₂O).

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