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10 Nov 2019
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?
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?
Hubert KochLv2
16 Jan 2019
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