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1.Calculate the pH at the following points in the titration of 50.0 mL of 0.100 methylamine (CH,N...
Calculate the pH at the equivalence point for the titration of 0.110 M methylamine ( CH 3 NH 2 ) with 0.110 M HCl . The Kb of methylamine is 5.0×10^-4
Consider the titration of 100.0 ml of 0.200 M CH3NH2 by 0.100 M HCl. (Kb for CH3NH2 = 4.4 x 10^-4) At what volume of HCl added, does the pH = 10.64?
QUESTION 14 Calculate the pH at each of the following points for the titration of 50.0 mL of 0.320 M HA with 0.320 M KOH. The Ka for HA is 6.5x10-6 at 0 mL of KOH added the pH = at 15.0 mL of KOH added the pH- at 25.0 mL of KOH added the pH = at 50.0 mL of KOH added the pH = at 60.0 mL of KOH added the pH =
read #10 (8. Calculate the pH for the following cases in the titration of 25.00 ml 01 0.200-M acetic acid, CH3COOH(aq), with 0.200 M NaOH(aq): (a) before addition of any NaOH(aq) (b) after addition of 5.00 mL of NaOH(aq) (c) after addition of 12.50 mL of NaOH(aq) (d) after addition of 25.00 mL of NaOH(aq) (e) after addition of 26.00 mL of NaOH(aq) QlCalculate the pH for each of the following cases in the titration of 35.0 mL of 0.200-M...
Calculate the pH at 0, 10.0, 25.0, 50.0, and 60.0 mL of titrant in the titration of 25.0 mL of 0.200 M HA with 0.100 M NaOH. Ka = 2.0 x 10-5.
a 50.0 mL sample of a 0.100 M solution of NaCN is titrated by 0.100 M HCl. kb for CN is 2.0x10-5. A.calculate the pH of the solution prior to the start of the titration. B after the addition of 10.0 mL. C. after the addition of 25.0 mL of 0.100 M HCl. D. at the equivalence point. E. after the addition of 60.0 mL of 0.100 M HCl
Calculate the pH for each case in the titration of 50.0 mL of 0.100 M HCIO(aq) with 0.100 M KOH(aq). Use the ionization constant for HCIO. What is the pH before addition of any KOH? pH = What is the pH after addition of 25.0 mL KOH? pH = What is the pH after addition of 30.0 mL KOH? pH = What is the pH after addition of 50.0 mL KOH? pH = What is the pH after addition of...
Calculate the pH at the equivalence point for the titration of 0.240 M methylamine ( CH 3 NH 2 ) with 0.240 M HCl . The K b of methylamine is 5.0 × 10 − 4 .
3. Calculate the pH at the following points for the titration of 25.0 mL of 0.100 M formic acid (Ka = 1.80 x 10-4) with 0.100 M NaOH: VNaOH = 0.00 mL, 15.00 mL, 25.00 mL, 40.00 mL. Draw a graph of pH vs. VNAOH. (30 points) (b) Buffer capacity can be thought of as how well a solution resists changes in pH after a strong base/acid is added. A buffer is most effective to resisting pH changes when what...
Consider the titration of 50.0 mL of 0.100 M HC3H5O2 by 0.100 M KOH for the next five questions (Ka for HC3H5O2 = 1.3 x 10-5). Calculate all pH values to two decimal places. - Calculate the pH after 25.0 mL of KOH has been added?