You have 75.0 mL of 0.17 M HA. After adding 30.0 mL of 0.10 M NaOH, the pH is 5.50. What is the Ka value of HA?

7. The pH titration curve of a weak acid, HA, is shown me below. As the titration progresses, HA is converted into its conjugate base, A-. 12 10 8 (a) What is the volume of NaOH at the equivalence point? 2 25 30 35 15 20 volume of NaOH added (mL) 5 10 (b) At what volume (or volumes) is all of the acid present in the protonated (HA) form? (c) At what volume (or volumes) is all of the acid present in the conjugate base (A') form? (d) At what point along the titration will half the original amount of HA have been converted to A-?

For 480.0 mL of a buffer solution that is 0.160 M in CH3CH2NH2 and 9.00×10−2 M in CH3CH2NH3Cl , calculate the initial pH and the final pH after adding 1.5×10−2 mol of HCl . ( Kb(CH3CH2NH2)=5.6×10−4 .)

Lemons get their sour flavor from citric acid (Ka = 7.4 x 10-4) a fresh squeezed lemon can have a citric acid concentration of 0.3 M and produce 20 mL. What is the pH after 20 mL of 0.6 KOH has been added?

Consider the buffer system of ammonia, NH3, and ammonium ion NH4+. (Ka= 5.6 x 10-10). a) What is the pH of a buffer solution prepared by adding 30.0g of ammonium chloride (NH4Cl) to 600 mL of .400 M ammonia? b) What is the pH of the solution after 100.0 mL of 2.0 M NaOH are added to the solution from part (a)?  c) What is the pH of the solution after 100.0 mL g 1.0 M HCl are added to the solution from part (a)? d) What is the pH of the solution after 30g of NaOH are added to the solution from part (a)?

What is the pH of a buffer solution that is 0.508 M in hydrofluoric acid and is 0.604 M is potassium fluoride? The K₂ of hydrofluoric acid is 6.4 x 10-4. (Two decimal places) Type your answer...

What is the pH of a solution prepared by mixing 20.0 mL of 0.50 M NaOH and 35.0 mL of 0.50 benzoic acid solution? (Benzoic acid is monoprotic with a Ka of 6.5 x 10-5.)

TUTOR Analysis of a Weak Acid-Strong Base Titration Curve Determine the pH during the titration of 63.3 mL of 0.465 M formic acid (K₂ = 1.8×10) by 0.465 M KOH at the following points. (Assume the titration is done at 25 °C.) (a) Before the addition of any KOH (b) After the addition of 16.0 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 95.0 mL of KOH

You start with 100.0 mL of 0.20 M CH3COOH in a flask.  The Ka of CH3COOH is 1.8 x 10-5. You add 10.0 mL of 0.20 M NaOH.  What is the pH of the solution after the NaOH is added? TRUE or FALSE:  The solution produced by mixing the reagents in the question above is a buffer.