A certain indicator, HA, has a K, value of 1.0 x 10-7. The protonated form of...

A certain indicator, HA, has a K, value of 1.0 x 10-7. The protonated form of the indicator is red and the ionized form is bl

stion 12 of 14 The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte

A certain indicator, HA, has a Ka, value of 1.0 x 10-7. The protonated form of the indicator is red and the ionized form is blue.

What is the pK, of the indicator?

What is the color of this indicator in a solution with pH=5.

The half-equivalence point of a titration occurs half way to the equivalence point, where half of the analyte has reacted to form its conjugate, and the other half still remains unreacted.

If 0.480 moles of a monoprotic weak acid (K, = 8.3 x 10 ) is titrated with NaOH, what is the pH of the solution at the half-equivalence point?

Expert Solution

queen_honey_blossom answered 2 years ago

A certain weak acid, HA , has a Ka value of 2.2×10−7. Part A Calculate the...

A certain weak acid, HA , has a Ka value of 2.2×10−7. Part A Calculate the percent ionization of HA in a 0.10 M solution.

A certain weak acid, HA, has a Ka value of5.8×10−7.Part A) Calculate the percent...

A certain weak acid, HA, has a Ka value of 5.8×10−7.Part A) Calculate the percent ionization of HA in a 0.10 M solution.Express your answer as a percent using two significant figures.Part B) Calculate the percent ionization of HA in a 0.010 M solution.Calculate the percent ionization of HA in a 0.010 M solution.

A certain weak acid, HA, has a Ka value of 8.7×10−7. Calculate the percent dissociation of...

A certain weak acid, HA, has a Ka value of 8.7×10−7. Calculate the percent dissociation of HA in a 0.10 M solution. Calculate the percent dissociation of HA in a 0.010 M solution.

A certain weak acid, HA, has a Ka value of 1.3×10−7. A) Calculate the percent ionization...

A certain weak acid, HA, has a Ka value of 1.3×10−7. A) Calculate the percent ionization of HA in a 0.10 M solution. Express your answer as a percent using two significant figures. B)Calculate the percent ionization of HA in a 0.010 M solution. Express your answer as a percent using two significant figures.

A certain weak acid, HA, has a Ka value of 2.8×10−7. Calculate the percent ionization of...

A certain weak acid, HA, has a Ka value of 2.8×10−7. Calculate the percent ionization of HA in a 0.10 M solution. Calculate the percent ionization of HA in a 0.010 M solution.

1) A certain weak acid, HA, has a Ka value of 4.6×10−7. Part A Calculate the...

1) A certain weak acid, HA, has a Ka value of 4.6×10−7. Part A Calculate the percent ionization of HA in a 0.10 M solution. Express your answer to two significant figures and include the appropriate units. 1.12×10−2 M Ba(OH)2 Express your answer using three significant figures. Enter your answers numerically separated by a comma. Part B Calculate the percent ionization of HA in a 0.010 M solution. Express your answer to two significant figures, and include the appropriate units....

A certain weak acid, HA, has a Ka value of 2.0×10−7. Part A: Calculate the percent...

A certain weak acid, HA, has a Ka value of 2.0×10−7. Part A: Calculate the percent ionization of HA in a 0.10 M solution. Part B: Calculate the percent ionization of HA in a 0.010 M solution.

HA, a weak acid, with Ka=1.0×10−8, also forms the ion HA−2. The reaction is HA(aq)+A−(aq)⇌HA−2(aq) and its K = 4.0.

HA, a weak acid, with Ka=1.0×10−8, also forms the ion HA−2. The reaction is HA(aq)+A−(aq)⇌HA−2(aq) and its K = 4.0. 1-) Calculate the [H+] in a 1.0 M solution of HA. 2-)Calculate the [A−] in a 1.0 M solution of HA 3-)Calculate the [HA−2] in a 1.0 M solution of HA. answers; [HA−2] = 1.8×10−4 M [A−] = 4.5×10−5 M [H+] = 2.2×10−4 M ,

250.0 mL of 0.10 M HA (Ka = 1.0 x 10-4 ) is mixed with 100.0...

250.0 mL of 0.10 M HA (Ka = 1.0 x 10-4 ) is mixed with 100.0 mL 0.25 M KOH. What is the pH?

A certain weak acid, HA, has a Ka value of 7.3

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