3. What would the titration curve look like if 0.10 M NaOH were in the flask...

3. What would the titration curve look like if 0.10 M NaOH were in the flask and 0.10 M HCl were in the buret? Make a rough sketch to illustrate your answer.

11. Biochemists and biologists often use the Henderson-Hasselbalch equation in working with buffers. When an acid solution is half-neutralized, half of the HA has been converted to A , and half of it is still in the form of HA. Therefore [HA] = [A ]. What happens to the Henderson-Hasselbalch equation when [HA] equals [A ]? How is it simplified?

Expert Solution

3) Titration is a method of determining the unknown molarity of a solution by adding enough acid or base of known molarity to neutralize it.

In an acid-base titration, a solution containing a known concentration of base is slowly added to an acid (or the acid is added to the base). Acid-base indicators can be used to signal the equivalence point of a titration (the point at which stoichiometrically equivalent quantities of acid and base have been brought together). Alternatively, a pH meter can be used to monitor the progress of the reaction producing a pH titration curve, a graph of the pH as a function of the volume of the added titrant. The shape of the titration curve makes it possible to determine the equivalence point in the titration. The titration curve can also be used to select suitable indicators and to determine the K_a of the weak acid or the K_b of the weak base being titrated.

The titration curve produced when a strong base is added to a strong acid has the general shape shown in Figure This curve depicts the pH change that occurs as 0.100 M NaOH is added to 50.0 mL of 0.100 M HCl. The pH can be calculated at various stages of the titration.

queen_honey_blossom answered 2 years ago

Sketch a titration curve for 50 mL of 0.10 M HCl titrated with 0.15 M NaOH....

Sketch a titration curve for 50 mL of 0.10 M HCl titrated with 0.15 M NaOH. Include on the graph: a) The initial pH b) The volume of the equivalence point c) The pH at the equivalence point d) The pH after addition of 50 mL of NaOH SHOW STEPS

For the titration of 75 mL of 0.10 M acetic acid with 0.10 M NaOH, calculate...

For the titration of 75 mL of 0.10 M acetic acid with 0.10 M NaOH, calculate the pH. For acetic acid, HC2H3O2, Ka = 1.8 x 10-5. (a) before the addition of any NaOH solution. (b) after 25 mL of the base has been added. (c) after half of the HC2H3O2 has been neutralized. (d) at the equivalence point.

Consider the titration of 10.00 mL of 0.10 M acetic acid (CH3COOH) with 0.10 M NaOH...

Consider the titration of 10.00 mL of 0.10 M acetic acid (CH3COOH) with 0.10 M NaOH a. What salt is formed during this reaction? b. do you expect the salt solution at the equivalence point to be acidic, neutral, or basic? Calculate the pH of this solution at the equicalence point.

3. Plot a schematic titration curve for acetic acid with NaOH. Superimpose the titration curve of...

3. Plot a schematic titration curve for acetic acid with NaOH. Superimpose the titration curve of HCl on this graph. What are the main differences? How can we determine the pKa of acetic acid from its titration curve?

25 ml of 0.10 M CH3CO2H is titrated with 0.10 M NaOH. What is the pH...

25 ml of 0.10 M CH3CO2H is titrated with 0.10 M NaOH. What is the pH after 15 ml of NaOH have been added? Ka for CH3CO2H = 1.8X10^-5

1.A student performs a titration by despensing 24.6 ml of 0.10 M NaOH into a 35.5...

1.A student performs a titration by despensing 24.6 ml of 0.10 M NaOH into a 35.5 mL sample of HCL. Calculate the molarity, mol/L, of the HCL solution. 2.Write the balanced equation for the dissolution of potassium hydrogen phthalate, KHC8H4O4, also known as KHP, in water to produce potassium ion and hydrogen phthalate ion, HC8H4O4-. 3. Write overall balanced equation for the reaction between sodium hydroxide, NaOH, and hydrogen phthalate ion, HC8H4O4-. 4.Write the net reaction that represents acid-base neutralization.

Question 3: Draw the titration curve (pH versus mL of NaOH added) that would be obtained...

Question 3: Draw the titration curve (pH versus mL of NaOH added) that would be obtained from the titration of 30 mL of a 0.10 M solution of an unknown triprotic acid, H3A (Ka1 = 1.26 x 10–3; Ka2 = 5.6 x 10–6; Ka3 = 3.32 x 10–10) with 0.10 M NaOH. Indicate the volume needed to reach the first, second, and third equivalence points and the pH at the half equivalence points for the three titration regions.

230 mL of 0.10 M NaOH are added to 100 mL of 0.10 M H3PO4. What...

230 mL of 0.10 M NaOH are added to 100 mL of 0.10 M H3PO4. What is the pH of the resulting solution?

(a) According to your experimental data, what volume of 0.10 M NaOH represents the half-equivalence (a.k.a. half-neutralization) point in this titration?

Table 1: Equilibrium Constants Data Syringe Reading pH After Each 0.5 mL Increment Color Observations 0 1.7 Clear yellow 2.5 2 yellow 5 2.5 Light yellow 7.5 3 off yellow 10 3.4 off yellow 12.5 3.8 off yellow 15 4 off orange 17.5 4.2 off orange 20 4.5 off orange 22.5 4.8 off orange 25 7.1 0range 27.5 9 Off orange 30 9.2 Off orange 32.5 9.4 Off orange 35 9.5 pink 37.5 9.7 off pink 40 10 Pink 42.5...

What would a philips curve graph look like for the past couple of years in Brazil?

Question