A 20.00 mL solution of 0.200M diprotic acid (H2A, pKa1=3.500, pKa2=8.500) is titrated with 0.250M KOH....

A 20.00 mL solution of 0.200M diprotic acid (H2A, pK_a1=3.500, pK_a2=8.500) is titrated with 0.250M KOH. Sketch the titration curve for this titration. Label the x-axis, y-axis, pK_a's, and equivalence points.

Expert Solution

queen_honey_blossom answered 1 year ago

The diprotic acid,H2A has two ionizable protons with pKa1=4.175 and pKa2=10.235. Determine the pH, [H2A], [HA-...

The diprotic acid,H2A has two ionizable protons with pKa1=4.175 and pKa2=10.235. Determine the pH, [H2A], [HA- ], [A-2 ], [OH-1 ] for the following three solutions. a) A solution which is 0.1500M in H2A. b) A solution which is 0.1500M in NaA c) A solution which is 0.1500M in Na2A

20.0mL of 0.127M diprotic acid (H2A) was titrated with 0.1018M KOH. The acid ionization constants for...

20.0mL of 0.127M diprotic acid (H2A) was titrated with 0.1018M KOH. The acid ionization constants for the acid are Ka1=5.2

Suppose you have a 10.00mL solution of H2A, a diprotic weak acid, which has a pka1...

Suppose you have a 10.00mL solution of H2A, a diprotic weak acid, which has a pka1 of 4.00 and a pka2 of 9.00. The formal concentration is 0.100M and it is titrated by 0.100M NaOH. (a) Write the two major reactions during the titration. Find the two equivalence points. (b) For each of the following delivered volumes (mL) of the titrant, find the pH: Vb=0, 2.00, 5.00, 9.90, 10.00, 12.00, 15.00, 20,00 and 21.00mL. Show all work please! Thanks

A 20.00 mL solution of 0.0840M HOCl is titrated with 0.0560M KOH solution. Calculate the pH...

A 20.00 mL solution of 0.0840M HOCl is titrated with 0.0560M KOH solution. Calculate the pH after each of the following additions of the KOH solution: a. 15.00mL b. 30.0mL c. 32.0mL

1.) A diprotic acid has the following pK values: pKa1 = 5.50, pKa2 = 9.50 a.)...

1.) A diprotic acid has the following pK values: pKa1 = 5.50, pKa2 = 9.50 a.) At what pH does [H2A] = [HA- ]? b.) At what pH does [HA- ] = [A2- ]? c.) Which is the principal species at pH = 3.50, H2A, HA- , or A2- ? Justify your answer using the Henderson-Hasselbach equation. d.) Which is the principal species at pH = 7.5, H2A, HA- , or A2- ? Justify your answer (don’t use Henderson-Hasselbach equation,...

A 20.00 mL solution of 0.100 M HCOOH (formic) was titrated with 0.100 M KOH. The...

A 20.00 mL solution of 0.100 M HCOOH (formic) was titrated with 0.100 M KOH. The Ka for the weak acid formic is 1.40 x 10-5. a. Determine the pH for the formic prior to its titration with KOH. b. Determine the pH of this solution at the ½ neutralization point of the titration. c. Identify the conjugate acid-base pair species at the ½ neutralization point.

Weak diprotic acid H2A is titrated with 0.2000 M NaOH. The initial concentration of H2A is...

Weak diprotic acid H2A is titrated with 0.2000 M NaOH. The initial concentration of H2A is 0.1000 M and the initial volume is 50.00 mL. Ka1 = 1.0 x 10−5 Ka2 = 1.0 x 10−9 (a) (0.2 pt) Identify the predominate species at the first equivalence point, by chemical formula: (b) (0.5 pts) Calculate the pH of the acid solution before any base is added. (c) (0.5 pts) Calculate the pH at the first equivalence point. (d) (0.2 pts)...

A 40.00 mL sample of 0.1000 M diprotic malonic acid is titrated with 0.0900 M KOH....

A 40.00 mL sample of 0.1000 M diprotic malonic acid is titrated with 0.0900 M KOH. What volume KOH must be added to give a pH of 6.00 ? Ka1 = 1.42 × 10−3 and Ka2 = 2.01 × 10−6.

125.0-mL aliquot of 0.124 M diprotic acid H2A (pK1 = 4.03, pK2 = 8.06) was titrated...

125.0-mL aliquot of 0.124 M diprotic acid H2A (pK1 = 4.03, pK2 = 8.06) was titrated with 1.24 M NaOH. Find the pH at the following volumes of base added: Vb = 0.00, 1.80, 6.25, 11.50, 12.50, 13.50, 18.75, 24.00, 25.00, and 28.00 mL. (Assume Kw = 1.01 ✕ 10−14.)

Consider the stepwise dissociation of the diprotic acid H2SO3; pKa1= 1.82 ans pKa2=7.20 a) write balanced...

Consider the stepwise dissociation of the diprotic acid H2SO3; pKa1= 1.82 ans pKa2=7.20 a) write balanced net ionic equations and Ka expressions for the stepwise dissociation of the diprotic acid, H2SO3. b) calculate the pH and concentration of all species in a solution of 0.025 M H2SO3.

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