(Solved) When a 1M solution of HCl is titrated with 1M solution of NaOH what happens to the solution's conductivity?

Juniordelor

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11 years ago

When a 1M solution of HCl is titrated with 1M solution of NaOH what happens to the solution's conductivity?

A. The conductivity will decrease
B. The conductivity will increase
C. The conductivity will remain the same
D. There will be no conductivity

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nyenohwin

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11 years ago

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buggingout16

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11 years ago

Thing to remember here: "conductivity of a solution is proportional to its ion concentration"

A. You started with 1M HCl and it dissociates completely (high conductivity) .

After titration, the acid and base react completely (no NaOH or HCl left), producing water, and the same number of moles of NaCl as the original HCl. (write down balanced equation to see this.)

NaCl also dissociates completely. However, because the reaction also produced water, this means the molarity increased for NaCl also (same number of moles of NaCl in a greater amount of water). This means a lower concentration of NaCl than the original HCl, leading to a decrease in conductivity.
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bunny13

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11 years ago

The conductivity would be almost zip but since there is a tiny bit in water, your answer is A and this is why. This is called a double replacement reaction. The formula is AB + CD = CB + AD. If you number your parts,
A = H
B = Cl
C =Na
D = OH
Now fit them into the equation. 2HCl + Na2O =2 NaCl + HOH (H2O). The products are table salt and plain water. Water conducts very slightly by itself but if you add an ion to it, it is a great conductor. If you add the salt to water the solution wold have good conductivity but table salt by itself doesn not conduct electricity..

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trejor00

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11 years ago

during the titration the high conductance of H+ ions will replaced by the less conductance Na+ ions . so the conductivity will decrease

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