Done < АА session.masteringchemistry.com C Problem 17.27 - Enhanced - with Feedback 6 of 29 A Review Constants Periodic

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Done < АА session.masteringchemistry.com C Problem 17.27 - Enhanced - with Feedback 6 of 29 A Review Constants Periodic Table A buffer solution contains 0.11 mol of acetic acid and 0.13 mol of sodium acetate in 1.00 L. Correct The addition of a strong base to the buffer will raise the pH because some of the weak acid will be converted to its conjugate base. The Henderson-Hasselbalch equation can be used to calculate the new pH because adding 0.02 mol of OH is within the buffer capacity (the buffer capacity would be exceeded when the ratio of base to acid is greater than 10). base) pH = pK+log acid 4.74 + log 0.13 0.02 0.11 -0.02 Part C What is the pH of the buffer after the addition of 0.02 mol of HNO3 ? Express your answer to two decimal places. IVO AED O ? pH = Submit Previous Answers Request Answer X Incorrect; Try Again; 3 attempts remaining Provide Feedback Nest