Problem: Calculate the pH for each of the following cases in the titration of 35.0 mL of 0.160 M KOH(aq), with 0.160 M HCl(aq).(b) after addition of 13.5 mL of HCl

FREE Expert Solution

We’re being asked to determine the pH after addition of 13.5 mL of HCl

Let’s first write the balanced reaction between HCl and KOH:

▪ HCl → strong oxyacid
▪ KOH → (OH- with Group 1A ion) → strong base
▪ the reaction between a strong base and strong acid → no need to create an ICE chart

Balanced reaction:              HCl(aq) + KOH(aq) → H2O(l) + KCl(aq)

Let’s first calculate the initial amount of KOH in moles:

Recall:

molarity (M)=molL

moles  KOH=0.16 mol  KOHL 35.0 mL x 10-3 L1 mL

moles KOH = 0.0056 mol KOH

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Problem Details

Calculate the pH for each of the following cases in the titration of 35.0 mL of 0.160 M KOH(aq), with 0.160 M HCl(aq).

(b) after addition of 13.5 mL of HCl

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