JUILLS alcalUWCU. FUUWI LLUCOCUIDLUI d luck! Question 21 ***A 50 mL solution of 0.10 MHC2H302 (aq)...
***A 50 mL solution of 0.10 M HC2H302 (aq) (K2 = 1.8 x 10-S) is titrated with 0.20 M NaOH (aq). ** What is the pH when 30 mL of NaOH(aq) is added? 8.98 o 12.10 - 1.90 O 11.23 o 12.90
Question 25 ***A 50 mL solution of 0.10 M HC2H2O2(aq) (Kg = 1.8 x 10-5) is titrated with 0.20 M NaOH (aq)** What is the pH after the addition of 5.0 mL of NaOH (aq)? 4.14 o 4.74 2.87 8.98 O 3.58 Previous
***A 50 mL solution of 0.10 M HC2H2O2 (aq) (K4 = 1.8 x 10-5) is titrated with 0.20 M NaOH (aq)*** What is the pH after the addition of 5.0 mL of NaOH(aq)? O 8.98 2.87 O 3.58 0 4.74 4.14
pls show all work. 11,13,14 all all part of the same titration problem! I attempted it several times and am getting very confused WA *** A 50 mL solution of 0.10 M benzoic acid (HC7H502 (aq)) (Ka = 6.5 * 10-5) is titrated with 0.20 M NaOH (aq). With this information, answer the questions (11-14) below.*** SB 11. What is the pH after the addition of 5.0 mL of NaOH (aq)? A) 5.49 B 3.58 C) 4.19 D) 2.59 E)...
***A 50 mL solution of 0.10 M HC2H2O2 (aq) (K = 1.8 x 10-5) is titrated with 0.20 M NaOH (aq). " At the equivalence point is the solution acidic, basic, or neutral and why? o Basic because of excess OH O Basic because of hydrolysis of C2H302 o Neutral salt of strong acid and strong base O Basic because of hydrolysis of HC2H2O2 Acidic because of hydrolysis of Nat
a 20.0 ml sample of 0.10 mol... CAN YOU EXPLAIN How to do B,C,D plz. i need it asap!! thank you so much A 20.0 mL sample of 0.10 mol/L CH3COOH was titrated with 0.20 mol/L. NaOH. Ka for CH3COOH is 1.8 x 10-6 a. What volume of NaOH is needed to reach the equivalence point? mL b. Calculate the pH of the solution in the flask at the equivalence point. pH = c. Calculate the pH of the solution...
25 mL of 0.10 M acetic acid is titrated with 0.10 M NaOH. What is the pH after 30 ml of NaOH have been added? Ka for acetic acid = 1.8 x 10^-5.
A 25.0 ml sample of 0.20 M Formic Acid (HCO2H, aq) is titrated with 0.10 M KOH(aq). What is the pH after 50.0 mL of the 0.10 M KOH has been added?
1) Calculate the pH of a solution produced by mixing 100.0 mL of 0.10 M HCl(aq) and 100.0 mL of 0.20 M NaOH(aq). 2) Calculate the pH of an aqueous solution made by mixing 100.0 mL of 0.40 M NH4Cl and 50.0 mL of 0.40 M NaOH. The pKa of NH4+ is 9.24.
assignment will be closed on Friday, March 29th at 12.00 PM (noon). The correct answers will be available on Friday March 29th. at 12:05 PM Question 1 1 pts A 10.0 mL sample of 0.25 M NHsloq) is titrated with 10.0 mL of 0.20 M HCloa) (adding HCI to NHal. Determine which region on the titration curve the mixture produced is in, and the pH of the mixture. Kb of NH3 is 1.8 × 10-5. Henderson-Hasselbalch equation: pH base] HCI...