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11 Nov 2019

Suppose 50.0 mL of an aqueous solution containing an unknown monobasic weak base (called B) is titrated with 0.150 M HCl. The titration requires 38.02 mL of the hydrochloric acid solution to reach the equivalence point. What is the concentration (in molarity) of the unknown base solution?

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Patrina Schowalter
Patrina SchowalterLv2
16 Jul 2019

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Related questions

Morphine, C17H19O3N is a weak base (Kb = 7.4 x 10-7). Consider its titration with hydrochloric acid. In the titration, 50.0 mL of a 0.1500 M solution of morphine is titrated with 0.1045 M HCl.

a.Write a balanced net ionic equation for the reaction that takes place during titration.

b.What are the species present at the equivalence point?

c.What volume of hydrochloric acid is required to reach the equivalence point?

d.What is the pH of the solution before any HCl is added?

e.What is the pH of the solution halfway to the equivalence point?

Morphine, C17H19O3N, is a weak base (Kb = 7.4 x 10-7). Consider its titration with hydrochloric acid. In the titration, 50.0 mL of a 0.1500 M solution of morphine is titrated with 0.1045 M HCl.

(a) Write a balanced net ionic equation for the reaction that takes place during titration.

(b) What are the species present at the equivalence point?

(c) What volume of hydrochloric acid is required to reach the equivalence point?

(d) What is the pH of the solution before any HCl is added?

(e) What is the pH of the solution halfway to the equivalence point?

(f) What is the pH of the solution at the equivalence point?

Suppose 50.0 mL of an aqueous solution containing an unknown monoprotic weakacid is titrated with 0.200 M KOH. The titration requires 22.07 mL of the potassium hydroxidesolution to reach the equivalence point. What is the concentration (in molarity) of the unknownacid solution?Here is what I think I should do but I am unsure if this is correct. 22.07 mL of .2M KOH= x moles..2=x/.02207L, X= 4.414*10^-3 Moles of KOH. Since there are that many Moles of KOH there must be equal moles of the acid. So 4.14*10-3moles/.05L= X M of initial acid== .0828M?

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