A 25.0 mL sample of a saturated  Ca(OH)2 solution is titrated with 0.026 M  HClHCl , and the equivalence point is reached after 37.9 mL of titrant are dispensed. Based on this data, what is the concentration (M) of the hydroxide ion?

A buffer solution contains 0.235 M ammonium bromide and 0.314 M ammonia. If 0.0164 moles of hydrobromic acid are added to 125 mL of this buffer, what is the pH of the resulting solution? (Assume that the volume change does not change upon adding hydrobromic acid) pH =

An analytical chemist is titrating 149.7 mL of a 0.5500M solution of benzoic acid (HC H CO,) with a 0.8000 M solution of NaOH. The p K of benzoic acid is 4.20. Calculate the pH of the acid solution after the chemist has added 16.29 mL of the NaOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of NaOH solution added. Round your answer to 2 decimal places. do pH = Check Explanation 2021 McGraw-Hil Education. All Rights Reserved. Terms of Use Privacy Accessibility V I 11:55 acer &

Students titrate 30.0 mL of 0.122 M hypochlorous acid with 0.105 M potassium hydroxide. a) How many mL are required to reach the equivalence point? b) What will be the pH of the solution when the student has added half of the amount of titrant that you calculated in part (a)? c) what will be the pH at the equivalence point?