Determine the pH during the titration of 26.8 mL of 0.447 M hypochlorous acid (K = 3.5×108) by 0.467 M NAOH at the following points. (a) Before the addition of any NaOH 3.90 (b) After the addition of 6.20 mL of NaOH 6.95 (c) At the half-equivalence point (the titration midpoint) |6.90| (d) At the equivalence point (e) After the addition of 38.5 mL of NaOH

Determine the pH during the titration of 35.1 mL of 0.297 M diethylamine ((C2H5)2NH , Kb = 6.9×10-4) by 0.297 M HI at the following points.(a) Before the addition of any HI(b) After the addition of 13.1 mL of HI(c) At the titration midpoint (d) At the equivalence point (e) After adding 54.4 mL of HI

Calculate pH for a weak base/strong acid titration. Determine the pH during the titration of 35.9 mL of 0.286 M methylamine (CH3NH₂, K₁ = 4.2x10-4) by 0.286 M HCIO4 at the following points. (a) Before the addition of any HCIO4 (b) After the addition of 13.2 mL of HCIO4 (c) At the titration midpoint (d) At the equivalence point (e) After adding 54.9 mL of HCIO4

A 35.00−mL solution of 0.2500 M HF is titrated with a standardized 0.1390 M solution of NaOH at 25°C. (a) What is the pH of the HF solution before titrant is added?   (b) How many milliliters of titrant are required to reach the equivalence point?  mL (c) What is the pH at 0.50 mL before the equivalence point?   (d) What is the pH at the equivalence point?   (e) What is the pH at 0.50 mL after the equivalence point?

Determine the pH during the titration of 60.6 mL of 0.420 M hydrocyanic acid (Ka = 4.0×10-10) by 0.420 M NaOH at the following points.(a) Before the addition of any NaOH(b) After the addition of 14.0 mL of NaOH(c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 90.9 mL of NaOH

Specify which of the following systems can be classified as a buffer system:(a) H2CO3/KHCO3 (b) NH3/ NH4Br (c) HNO2/NaNO2 (d) KHSO4/H2SO4 (e) HCOOH/HCOONa (f) HClO4/NaClO4 (g) HCN/NaCN (h) H2CO3/NaHCO3 (i) KH2PO4/K2HPO4 (j) KCl/HCl

Ff.202.

The following pH curve is for the titration of 20.0 mL of a 0.10 M solution of a weak monoprotic acid with a 0.10 M solution of a strong monoprotic base. Data points at 1 mL increments. (a) What is the pH before any titrant has been added? (b) What is the pH at the midpoint of the titration? (c) What is the pH at the equivalence point? (d) What is the value of K, for the weak acid? 14.0 12.0 10.0 공 8.0 6.0 4.0 2.0 0.0 0.0 10.0 1444444444444ÄÄÄÄÄÄÄÄÄÄÄÄÄ 20.0 30.0 Volume of titrant (mL) 40.0 50.0

Determine the pH during the titration of 20.1 mL of 0.429 M hydrocyanic acid (Ka by 0.359 M KOH at the following points. (a) Before the addition of any KOH (b) After the addition of 5.40 mL of KOH (c) At the half-equivalence point (the titration midpoint) (d) At the equivalence point (e) After the addition of 36.0 mL of KOH = 4.0×10-10)

t ent Determine the pH during the titration of 64.4 mL of 0.443 M acetic acid (K₂ = 1.8x10-5) by 0.443 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 96.6 mL of KOH