A 30 mL of 0.1 M CH3NH2 (kb = 4.8 × 10-4) is titrated with 0.1 M HCl. Calculate the pH after the addition of the following volumes of titrant: 0 mL of titrant 10 mL of titrant 15 mL of titrant 30 mL of titrant 40 mL of titrant

Imagine you are working in the lab, and your labmate Jordan has challenged you to figure out which one of the  following acetic acid/sodium acetate buffer solutions has the greatest buffering capacity at a pH above 4.74. pKa(acetic acid) = 4.74. Can you pick the solution with the highest buffering capacity at a pHabove 4.74? pKa(acetic acid) ?     0.36 M acetic acid and 0.12 M sodium acetate         0.16 M acetic acid and 0.12 M sodium acetate         0.36 M acetic acid and 0.22 M sodium acetate         0.16 M acetic acid and 0.22 M sodium acetate

11,The equivalence point of titrating of the weak base with the strong acid will be observed at Group of answer choices A, pH>7 B, pH<7 C, pH=pKb D, pH>pKb E, pH=7   12,The titration curve of titrating a diprotic acid with a strong base will have two distinct equivalence points  Group of answer choices A, if Ka1<<Ka2 B, if Ka1=Ka2 C, always D, in case of ta strong acid E, if Ka1>>Ka2

Calculating the pH of a weak acid titrated with a strong base Try Again Your answer is wrong. In addition to checking your math, check that you used the right data and DID NOT round any intermediate calculations. 0/5 An analytical chemist is titrating 165.1 mL of a 1.100M solution of acetic acid (HCH3CO2) with a 1.200M solution of KOH. The pK of acetic acid is 4.70. Calculate the pH of the acid solution after the chemist has added 71.89 mL of the KOH solution to it. a 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. ? 00. 18 Ar pH ☑

Determine the pH at the equivalence point in the titration of 50.0 mL of 0.300 M CH₃COOH with 0.300 M NaOH. The value of Ka for CH₃COOH is 1.8 × 10⁻⁵. Use a BCA table to detrmine the moles of reactant and product after the reaction of the acid and base. Ignore the amount of liquid water. Then, set up an ICE table to identify the unknown. Then figure the pH.

A 25.0 mL sample of 0.150 M hydrofluoric acid is titrated with a 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of hydrofluoric acid is 3.5 × 10-4.

If the pH at the 1/2 equivalence point is 4.19, what would be the Ka?