0.901g KHP is fully titrated with 44.1 mL of an NaOH solution of unknown concentration. What...

0.901g KHP is fully titrated with 44.1 mL of an NaOH solution of unknown concentration. What is the concentration of the NaOH solution? (Report to 3 sig figs).

Expert Solution

Ans. Moles of KHP used = Mass / Molar mass

= 0.901 g / (204.23 g/mol)

= 4.4117 x 10^-3 mol

# Stoichiometry: 1 mol NaOH neutralizes 1 mol KHP.

Since 1 mol KHP is neutralized by 1 mol NaOH, the number of moles of both species must be equal at equivalence point.

So, moles of NaOH in 44.1 mL NaOH solution = 4.4117 x 10^-3 mol

Now,

Molarity of NaOH solution = Moles of NaOH / Volume of solution in liters

= 4.4117 x 10^-3 mol / 0.0441 L

= 0.1000 mol/ L ; [1 mol/ L = 1 M]

= 0.1000 M

Hence, molarity of NaOH solution = 0.100 M

queen_honey_blossom answered 2 years ago

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