3. (8 pts) Consider the titration of 35.0 mL of 0.150 M CH3COOH W M NaOH...
A 50.0 ml sample of 0.50 M acetic acid, ch3cooh is titrated with a 0.150 M NaOH solution. calculate the ph after 25.0 ml of the base have been added (ka=1.8x10^-5)
Consider the titration of 50 mL of 0.100 M acetic acid (CH3COOH, Ka = 1.8 x 10-5) with 0.200 M NaOH solution. Show all calculations for full credit. a) Write the titration reaction: b) Calculate the pH after 5.00 mL of NaOH: c) Calculate the pH after 12.5 mL of NaOH: d) Calculate the pH after 25 mL of NaOH:
A 25.0 mL sample of 0.150 M acetic acid (CH3COOH) is titrated with 0.150 M NaOH solution. What is the pH at the equivalence point? The Ka of acetic acid is 4.5E-4
Consider the titration of 50 mL of 0.100 M acetic acid (CH3COOH, Ka = 1.8 x 10-5) with 0.200 M NaOH solution. Show all calculations for full credit. a) Write the titration reaction: b) Calculate the pH after 5.00 mL of NaOH: c) Calculate the pH after 12.5 mL of NaOH: d) Calculate the pH after 25 mL of NaOH:
Consider the titration of a 73.9 mL sample of 0.13 M HC2H3O2 with 6.978 M NaOH. Ka(HC2H3O2) = 1.8x10-5 Determine the initial pH before any NaOH is added. Express your answer using two decimal places. Consider the titration of a 46.6 mL sample of 0.078 M HC2H3O2 with 1.135 M NaOH. Ka(HC2H3O2) = 1.8x10-5 Determine the volume of added base required to reach the equivalence point. Answer in units of milliliters. Consider the titration of a 17.2 mL sample of...
If 100mL of 0.10M CH3COOH (Ka=1.8x10-5) is titrated with 0.10 M NaOH. Calculate the pH value for the following solution. A. 75.0 mL of NaOH is added B. 100.0 mL of NaOH is added C. Suggest an indicator for this titration
1) What is the pH of a solution in which 25 mL of 0.10 M NaOH is added to 15 mL of 0.10 M HCl? 2) If you add 2.50 mL of 0.150 M HCl to 100 mL of a buffer consisting of 0.100 M CH3COOH and 0.200 M CH3COONa, what will be the change in pH? (Ka of CH3COOH is 1.8x10^-5)
Consider the titration of a 18.1 mL sample of 0.113 M HC2H3O2 with 0.184 M NaOH. Ka(HC2H3O2) = 1.8x10-5 Determine the pH at 0.13 mL of added base. Enter to 4 decimal places.
4.) For the titration of 15.00 mL of 0.100 M C6H5OH with 0.150 M NaOH, calculate the pH after the addition of 6.00 mL of NaOH. 5.) For the titration of 30.00 mL of 0.090 M HNO2 with 0.120 M NaOH, calculate the pH at the equivalence point.
16. Consider the titration of a 7.5 mL sample of 0.106 M HC2H3O2with 0.146 M NaOH. Ka(HC2H3O2) = 1.8x10-5 Determine the pH at one-half of the equivalence point.