12. Consider the titration of 0.100 L of 0.200 M ascorbic acid with 0.500 M NaOH....

12. Consider the titration of 0.100 L of 0.200 M ascorbic acid with 0.500 M NaOH. What is the pH at the endpoint of the titration? Enter your answer to two decimal places; for this question we can assume the 5% assumption is valid.

Expert Solution

queen_honey_blossom answered 2 years ago

You are titrating 0.100 L of 0.100 M carbonic acid (shown below) with 0.500 M NaOH....

You are titrating 0.100 L of 0.100 M carbonic acid (shown below) with 0.500 M NaOH. What will the pH be when 23.0 mL of NaOH have been added? pkas: 6.05 and 10.64

1) Consider the titration of 50.0 mL of 0.200 M HClO4 by 0.100 M NaOH. Complete...

1) Consider the titration of 50.0 mL of 0.200 M HClO4 by 0.100 M NaOH. Complete the table with answers to the following questions: What is the pH after 35.5 mL of NaOH has been added? At what volume (in mL) of NaOH added does the pH of the resulting solution equal 7.00?

Consider the titration of 25.0 mL of 0.100 M acetic acid (HA) with 0.100 M NaOH....

Consider the titration of 25.0 mL of 0.100 M acetic acid (HA) with 0.100 M NaOH. 1. Write the balanced chemical equation and equilibrium constant expression (ECE) for all of the reactions that occur when NaOH is added to the acetic throughout the titration. Hint: think of what is in the solution (acetic acid) with water, acetic acid with sodium hydroxide, and acetate ion with water) as the titration is proceeding. 2. Calculate the volume of NaOH solution needed to...

Consider the titration of 0.100 L of 0.200 M sulfurous acid (see Ka/Kb table from table)...

Consider the titration of 0.100 L of 0.200 M sulfurous acid (see Ka/Kb table from table) with 0.500 M NaOH. What is the pH at the endpoint of the titration?

Consider a the titration of 0.685 L of 0.773 M ascorbic acid (H2C6H6O6) with 1.76 M...

Consider a the titration of 0.685 L of 0.773 M ascorbic acid (H2C6H6O6) with 1.76 M NaOH. What is the pH at the second equivalence point of the titration?

Pertaining to the titration of 25.0mL of 0.100 M HCN (Ka=6.2x10-10) with 0.200 M NaOH, calculate...

Pertaining to the titration of 25.0mL of 0.100 M HCN (Ka=6.2x10-10) with 0.200 M NaOH, calculate the pH at the following points. a) initial pH, 0.0mL NaOH b) after the addition of 4.0mL NaOH c) after the addition of 6.25 mL NaOH d) at the equivalence point e) after the addition of 17.0 mL NaOH

Consider the titration of 40.0 mL of 0.200 M HClO4 by 0.100 M KOH. Calculate the...

Consider the titration of 40.0 mL of 0.200 M HClO4 by 0.100 M KOH. Calculate the pH of the resulting solution after the following volumes of KOH have been added. a. 0.0 mL d. 80.0 mL b. 10.0 mL e. 100.0 mL c. 40.0 mL answers are A) 0.699 B) 0.854 C) 1.301 D) 7.00 E) 12.15 I would just like to know how to do the work please and tbank you

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Consider the titration of 40.00 mL of 0.200 M NH3 with 0.500 M HCl. Calculate pH a) initially b) after addition of 5.00 mL of 0.500 M HCl c) at the half-neutralization point (halfway to equilvalence point) d) after the addition of 10.00 mL of 0.500 M HCl e) at the equivalence point

Consider the titration of 0.100 M HCl, a strong acid, with 0.100 M NH3, a weak...

Consider the titration of 0.100 M HCl, a strong acid, with 0.100 M NH3, a weak base: HCL(aq)+NH3(aq)---NH4+(aq)+H2O(l) Calculate the pH at the following points in the titration when 25.0 mL of 0.0100 M NH3 is titrated with 0.100 M HCL. A. 0.0 mL of HCl added B. 10.0 mL of HCl added C. At equivalence point D. 35.0 mL of HCL added

Please explain... In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric...

Please explain... In the titration of a weak acid HA with 0.100 M NaOH, the stoichiometric point is known to occur at a pH value of approximately 11. Which of the following indicators would be best to use to mark the endpoint of this titration? a. an indicator with Ka = 10–13 b. an indicator with Ka = 10–14 c. an indicator with Ka = 10–10 d. an indicator with Ka = 10–8 e. an indicator with Ka = 10–11...

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