the pH at the equivalence point MISSED THIS? Read Section 18.4 (Pages 803 - 817) ; Watch_KCV 18.4A, IWE 18.6 . Express your answer as a whole number. Consider the titration of a 38.0 mL sample of 0.170 M HBr with 0.200 M KOH. Determine each of the following: pH = Submit Request Answer Part E the pH after adding 5.0 mL of base beyond the equivalence point Express your answer using two decimal places ? pH = Submit Request Answer

Consider a tritation of 25.00 mL of 0.112 of NaOH with 0.100 of HCl. a) determine the pH before starting the titration. b) determine the pH after adding 30.8mL of HCl.

An analytical chemist is titrating 109.3 ml. of a 0.8700 M solution of butanoic acid (HC,H,CO,) with a 0.9500 M solution of NaOH. The pK, of butanoic add is 4.82. Calculate the pH of the and solution after the chemist has added 36.93 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. pH = 0 X

100. mL of 0.200 M HC1 is titrated with 0.250 M NaOH.

Please answer both the question otherwise I'll downvote

Consider the situation in which 50.0 mL of 0.200 M HNO3 is being titrated with 0.100 M NaOH. Determine each quantity: 5. determine the pH after adding 100.0 mL of base