Given the following experimental data, calculate the molarity and the pKa of the acid analyte (HA) in the titration, with the following data: HA + NaOH à NaA + H2O.       -A pH reading of 3.65 is obtained when 13.0 mL of 0.413 M NaOH is added to the 25.0 mL analyte.      -The endpoint of the titration is achieved when 31.25 mL of NaOH have been added. Show all your calculations.

The half‑equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted.If 0.340 moles of a monoprotic weak acid (Ka=6.3×10−5) is titrated with NaOH ,what is the pH of the solution at the half‑equivalence point?

The half-equivalence point of a titration occurs halfway to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.480 moles of a monoprotic weak acid (Ka-5.3x10-5) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?

Calculate the pH at the equivalence point for the following titration: 0.30 M HC1 versus 0.30 M methylamine (CH₂NH₂). Round your answer to 2 decimal places. Note: The K of methylammonium is 2.21 × 10-¹¹. pH =

A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for HC2H3O2 is 1.8×10−5. Calculate the pH of the solution upon addition of 47.2 mL of 1.00 M HCl to the original buffer. Express your answer using two decimal places.

Propanoic acid has a Ka=1.3x10-5. The titration starts with 40.00 mL of 0.1000 M propanoic acid (HPr), and we slowly add 0.1000 M NaOH. What is the pH at 0.00 mL and 30.00 mL?

In a lab, you titrate 27.0 mL of 0.100 M acetic acid (CH3COOH, a weak acid, pKa 5.756, Ka 2.75 x 10-5), with 0.100 M NaOH. Identify the the weak acid-base equilibrium that corresponds to this Ka. When the analyte (acetic acid) is 100% in its acid form, before any titrant (NaOH) has been added, what is the pH?  At what pH has 50% of the reactant acid been titrated? At the equivalence point, what percentage of the analyte has been titrated?  At the equivalence point, the primary species in solution is _____. At the equivalence point, the concentration of the primary species in solution is approximately What is the pH of the solution at the equivalence point?

The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted. If 0.280 moles of a monoprotic weak acid (Ka 4.8 x 10-) is titrated with NaOH, what is the pH of the solution at the half-equivalence point? pH =

Calculate the volume in liters of 0.545 M KOH necessary to titrate 0.0113 moles of hydrochloric acid, HCl, to a phenolphthalein end-point. Report the answer with three significant figures.

Consider the titration of 100.0 mL of 0.250 M aniline, C6H5NH₂, (Kb = 3.8 x 10-10) with 0.500 M HCl at 25 °C. Calculate the pH when 25.00 mL of titrant have been added. Enter your response in pH units to the nearest 0.01.