Problem: What is the pH of a solution made by mixing 40.0 mL of 0.100 M HCl with 25.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.A) 0.64B) 1.64C) 12.36D) 13.36E) 10.00

FREE Expert Solution
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
▪ 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)



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

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Problem Details

What is the pH of a solution made by mixing 40.0 mL of 0.100 M HCl with 25.00 mL of 0.100 M KOH? Assume that the volumes of the solutions are additive.

A) 0.64

B) 1.64

C) 12.36

D) 13.36

E) 10.00

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