Problem: Calculate the pH of a solution prepared by adding 20.0 mL of 0.40 M HCl to 80.0 mL of 0.10 M Sr(OH)2.A. 11.90B. 7.00C. 13.40D. 12.90E. 10.50

FREE Expert Solution

We’re being asked to determine the pH of a solution when 40.0 mL of 0.100 M HCl is mixed with 25.00 mL of 0.100 M KOH


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

▪ HCl → strong binary acid
▪ Sr(OH)2 → (OH- with Group 2A ion) → strong base
▪ the reaction between a strong base and strong acid → no need to create an ICE chart

Balanced reaction:             HCl(aq) + Sr(OH)2(aq) → 2 H2O(l) + SrCl2(aq)



Now let’s find the concentration of reactant remaining after the reaction:

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Problem Details

Calculate the pH of a solution prepared by adding 20.0 mL of 0.40 M HCl to 80.0 mL of 0.10 M Sr(OH)2.

A. 11.90

B. 7.00

C. 13.40

D. 12.90

E. 10.50

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Our tutors have indicated that to solve this problem you will need to apply the Strong Acid Strong Base Titrations concept. You can view video lessons to learn Strong Acid Strong Base Titrations. Or if you need more Strong Acid Strong Base Titrations practice, you can also practice Strong Acid Strong Base Titrations practice problems.