1. Explain how the pH of the solution is changing using the titration curve. 2. Describe...

1. Explain how the pH of the solution is changing using the titration curve.
2. Describe the process in which you would titrate a weak acid with a strong base. Include an image of a titration curve.

3. Explain the titration curve of a polyprotic acid.

4. Difference between endpoint and equivalence point?

Expert Solution

queen_honey_blossom answered 11 months ago

When creating a titration curve for a weak base, the pH of the initial solution requires...

When creating a titration curve for a weak base, the pH of the initial solution requires setting up a table showing the initial, change, and equilibrium values for each species and plugging these into the equilibrium constant expression. The expression for the bicarbonate ion is Ka1=[H2CO3][H+][HCO3−] For an anion that can both hydrolyze and produce H+, the pH of a concentrated solution can be more easily approximated using the equation pH=12(pKa1+pKa2) During the titration before the equivalence point, provided that...

1) Generate a titration curve (pH vs. mL NaOH) for the titration of 10 mL 0.15M...

1) Generate a titration curve (pH vs. mL NaOH) for the titration of 10 mL 0.15M HCl with 0.15M NaOH ( suggest 2mL intervals up to 16 mL). Calculations: mL NaOH pH 0 2 4 6 8 10 12 14 16 2) Make another titration curve using acetic acid instead of HCl (same concentration)

Protein Denaturation: 1) If changing the pH of an enzyme solution greatly reduces the activity of...

Protein Denaturation: 1) If changing the pH of an enzyme solution greatly reduces the activity of that enzyme without precipitation, how could you tell in the lab if it were the result of denaturation or just going to a pH that is just not a good one for the enzyme? And how would a change in pH impact or even stop enzyme function without denaturation? (Consider the enzymes that are active in your stomach, such as pepsin-discussed in Wikipedia.) 2)...

Titration: Calculate the pH of each solution listed below. You are starting with a solution of...

Titration: Calculate the pH of each solution listed below. You are starting with a solution of NaClO and titrating that solution with HCl. A) What is the pH of 25.0 mL of 0.035 M NaClO? The Kb of ClO- is 2.86 x 10-7? B) What is the pH when you add 12.5mL of 0.035M HCl? C) What is the pH when you add 25.0 mL of 0.035 M HCl?

1. Describe the pH scale, and define the terms acid and base. 2. Explain how carbonic...

1. Describe the pH scale, and define the terms acid and base. 2. Explain how carbonic acid and bicarbonate are formed in the blood and the functions they serve. 3. Define the terms acidosis and alkalosis, and explain how they relate to hypoventilation and hyperventilation. 4. Explain how ventilation is adjusted to help maintain acid-base balance.

Calculate the pH of a polyprotic acid give and sketch the titration curve for the following...

Calculate the pH of a polyprotic acid give and sketch the titration curve for the following reaction: A 10.0-mL aliquot of 0.100M Na3AsO4 titrated with 0.100M HCl. pK1 = 2.25, pK2 = 6.77, pK3 = 11.60.

If changing the pH of an enzyme solution greatly reduces the activity of that enzyme without...

If changing the pH of an enzyme solution greatly reduces the activity of that enzyme without precipitation, how could you tell in the lab if the result of denaturation or just going to a pH that is just not a good one for the enzyme? And how would a change in pH impact or even stop enzyme function without denaturation? (consider the enzymes that are active in your stomach, such as pepsin)

Why does the curve of titration of acetic acid begin at a higher pH than the...

Why does the curve of titration of acetic acid begin at a higher pH than the curve for HCl? Why does the pH at the center of the rapidly rising region occur at a higher pH for the acetic acid curve than for the HCl curve?

Draw a titration curve for each of the following situations. Include the volumes and pH values...

Draw a titration curve for each of the following situations. Include the volumes and pH values for all equivalence points and halfway points. a) 45.0 mL of 0.250 M KOH is titrated with 0.400 M HCl. b) 15.0 mL of 0.150 M CH3NH2 IS TITRATED WITH 0.200 M HCl. c) 20.0 mL of 0.100 M 1,2-propanediamine, CH3CH(NH2)CH2NH2, a compound that accepts protons at two different N atoms, is titrated with 0.100 M HCl. The pKb values for 1,2-propanediamine are 4.18...

In a titration of a 100.0mL 1.00M NH3 solution with 1.00M HCl, what is the pH...

In a titration of a 100.0mL 1.00M NH3 solution with 1.00M HCl, what is the pH of the solution after the addition of 127 mL of HCl? Kb = 1.8 x 10-5 for NH3

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