Each of these results is also the number of moles of strong base, since the KHP

Question

Each of these results is also the number of moles of strong base, since the KHP and base react in a 1:1 mole ratio. The concentration of the base solution is the moles of base divided by the number of liters of base required to reach the endpoint (remember to convert mL of base to liters): mol NaOH / L = M of base Do this calculation for each of the three trials, and enter the calculated base concentrations below. Be careful to enter the correct number of sig figs in your reported values. M of base for trial#1 > L1065 M of base for trial#2 .1012 M of base for trial#3 .1008

Explanation / Answer

Average of three trials M of base = 0.1065 M + 0.1012 M + 0.1008 M / 3 = 0.1028 M concentration

The reaction between base and acid here is 1 : 1 ratio.

Given, volume of HCl = 5 ml

The number of ml of base used is missing from the data.

Lets say we used 5 ml of base for the titration then,

mols of base used = M x L = 0.1028 M x 0.005 L = 5.14 x 10^-4 mols

So, moles of HCl = 5.14 x 10^-4 mols

Molarity of HCl solution = moles/L = 5.14 x 10^-4 mols / 0.005 L = 0.1028 M

Check the volume of base used and you can easily calculate the mols and Molarity of HCl used by this method.

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