An aqueous solution of potassium hydroxide is standardized by titration with a 0.122 M solution of hydrobromic acid. If 22.1 mL of base are required to neutralize 18.8 mL of the acid, what is the molarity of the potassium hydroxide solution?

The molarity of the potassium hydroxide solution is 0.104 M

Explanation:

Step 1: Data given

Molarity of hydrobromic acid (HBr) = 0.122 M

Volume of potassium hydroxide (KOH) = 22.1 mL = 0.0221 L

Volume of hydrobromic acid = 18.8 mL = 0.0188 L

Step 2: The balanced equation

HBr(aq) + KOH(aq) → KBr(aq) + H2O(l)

Step 3: Calculate moles of HBr

Moles HBr = molarity HBr * volume HBr

Moles HBr = 0.122 M * 0.0188 L

Moles HBr = 0.0022936 moles

Step 4: Calculate molarity of KOH

We need 0.0022936 moles of KOH to neutralize the HBr

Molarity = moles / volume

Molarity KOH = 0.0022936 moles  /0.0221 L

Molarity KOH = 0.104 M

The molarity of the potassium hydroxide solution is 0.104 M

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