A 25.00 mL sample of propionic acid HC3H5O2, of unknown concentration was titrated with 0.141 M KOH. The equivalent point was reached when 43.76mL of base had been added. What is the hydroxide-ion concentration at the equivalence point? Ka for propionic acid is 1.3 x 10-5 at 25C

A 0.258-g sample of a pure triprotic acid, H3A, (where A is the generic anion of the acid), was dissolved in water and titrated with 0.150 M barium hydroxide solution. The titration required 13.9 mL of the base to reach the equivalence point. What is the molar mass of the acid? 227 g/mol 82.5 g/mol 371 g/mol 124 g/mol 186 g/mol

The p?apKa of hypochlorous acid is 7.5307.530. A 56.056.0 mL solution of 0.1000.100 M sodium hypochlorite (NaOClNaOCl) is titrated with 0.2640.264 M HClHCl. Calculate the pH of the solution after the addition of 8.21 mL of 0.264 M HClHCl. pH=pH=     Calculate the pH of the solution after the addition of 22.0 mL of 0.264 M HCl pH=pH=     Calculate the pH of the solution at the equivalence point with 0.264 M HClHCl. pH=pH=

Calculating the pH of a weak acid titratéd WitH a SIU An analytical chemist is titrating 72.2 mL of a 0.8900M solution of propionic acid (HC,H,Co, with a 0.5400M solution of NaOH. The p K of propionic acid is 4.89. Calculate the pH of the acid solution after the chemist has added 130. 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 = Explanation Check O2021 McGraw-Hill Education. All Rights Reserved. Terms of Use Privacy Accessibilit 17 MacBook Air FI F10

Tyler titrates 40 mL of 0.350 M lactic acid (HC3H5O3,Ka=1.5×10−4) using 0.450 M NaOH. Calculate the pH of the resulting solution at each of the following points in the titration. After adding 30 mL of the NaOH solution: At the equivalence point: After adding 38.7 mL of the NaOH solution:

In a titration of 68.0 mL of a 0.750 M solution of a triprotic acid H₃C₆H₅O₇ (citric acid) with 0.500 M NaOH, how many mL of base are required to reach the third equivalence point?

A titration of 3.36 g of an acid requires 43.72mL of 0.100M NaOH to reach the equivalence point.  What is the molar mass of the acid?

When titrating 125 mL of nitric acid HNO3 0.165 mol/L, with KOH 0.219 mol/L.a) What is the pH of the solution before starting the titration, and what volume of KOH (in mL) is required to reach the equivalence point?b) What is the pH of the solution after the addition of 44.5 mL of KOH solution?c) What is the pH of the solution at the equivalence point, and the pH of the solution after the addition of 200 mL of KOH solution?

An analytical chemist is titrating 169.4 mL of a 1.000M solution of butanoic acid (HC3H,CO₂) with a 1.100M solution of KOH. The pK of butanoic acid is 4.82. Calculate the pH of the acid solution after the chemist has added 183.1 mL of the KOH solution to it. Note for advanced students: you may assume the final volume equals the initial volume of the solution plus the volume of KOH solution added. Round your answer to 2 decimal places. pH = ☑

Calculating the pH at equivalence of a titration A chemist titrates 170.0 mL of a 0.2614M cyanic acid (HCNO) solution with 0.7980M NaOH solution at 25 °C. Calculate the pH at equivalence. The p K, of cyanic acid is 3.46. Round your answer to 2 decimal places. Note for advanced students: you may assume the total volume of the solution equals the initial volume plus the volume of NAOH solution added. pH =