Use the Relerences to access important valoes il needed for this qaestion A 1.00

Question

Use the Relerences to access important valoes il needed for this qaestion A 1.00 liter solution contains 0.41 moles acetic acid and 0.32 moles sodium acetate 0.16 moles of hydoiodic acid are added to this system, indicate whether the following statements are true or false. (Assume that the volume does not change upon the addition of hydroiodic acid) A. The number of moles of CH COOH will remain the same. B. The number of moles of CH,COO will increase. C. The equilibrium concentration of Hy0t will increase ? D. The pH will remain the same -YE. The ratio of [CHiCOOH) / tCHC001 will increase Submit Answr Retry Entire Group 11:54 SAMSUNG 5 9 0

Explanation / Answer

When HI is added to the buffer solution of acetic acid/sodium acetate

the HI is dissociated into H+ and I-

sodium acetate may react with H+ and form acetic acid which leads to decrease in the moles of acetate conjugate ion

1) So the number of moles of acetic acid increases.is true

2) The number of acetate ions increase is false. It will decrease

3) The equilibrium concentration of H3O+ ion increase- true

4) The pH will remain same - false it increases as the H+ ions concentration increase

5) The ratio of [CH3COOH]/[CH3COO-] will increase - true because as the moles of acetate ions decrease in denominator the ratio increases.

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