Problem: Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.250 M HClO(aq) with 0.250 M KOH(aq). The ionization constant for HClO can be found here.(a) before addition of any KOH(b) after addition of 25.0 mL of KOH(c) after addition of 30.0 mL of KOH(d) after addition of 50.0 mL of KOH(e) after addition of 60.0 mL of KOH

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We are being asked to determine the pH of the HClO solution.


(a) before addition of any KOH 

The dissociation of HClO in water:

HClO  +  H2O     H3O+  +   ClO-


0.250 M HClO(1 mol H3O+1 mol HClO)=0.250 M H3O+


pH = -log[H3O+]pH = -log[0.250 M]

pH = 0.60


(b) after addition of 25.0 mL of KOH

We will calculate the pH of the HClO solution using the following steps:

Step 1. Calculate the initial amounts of HClO and KOH in moles before the reaction happens.

Step 2. Write the chemical equation for the reaction between HClO and KOH.

Step 3. Construct an ICF Chart.

Step 4. Calculate pH.

 

Step 1. Calculate the initial amounts of HClO and NaOH in moles before the reaction happens.

molarity (volume) → moles

Recall:

Molarity = moles of soluteLiters of solution

*convert volumes from mL to L → 1 mL = 10-3 L


 50.0 mL of 0.250 M HClO(aq)

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Problem Details

Calculate the pH for each of the following cases in the titration of 50.0 mL of 0.250 M HClO(aq) with 0.250 M KOH(aq). The ionization constant for HClO can be found here.

(a) before addition of any KOH

(b) after addition of 25.0 mL of KOH

(c) after addition of 30.0 mL of KOH

(d) after addition of 50.0 mL of KOH

(e) after addition of 60.0 mL of KOH