Problem: 100.0 mL of a 0.50 M aqueous NH3 solution is mixed with 200.0 mL of 0.25 M aqueous HI. At 25°C the mixture will have a pH of a. not enough information is givenb. = 7.00c. > 7.00d. < 7.00

FREE Expert Solution

We are being asked to calculate the pH of 100.0 mL of a 0.50 M aqueous NH3 solution mixed with 200.0 mL of 0.25 M aqueous HI.


We will calculate the pH of the solution at the equivalence point using the following steps:

Step 1. Write the chemical equation for the reaction between NH3 and HI.
Step 2. Calculate the initial amounts of NH3 and HI in moles before the reaction happens.
Step 3. Construct an ICF Chart.
Step 4. Calculate the new concentration of the species left in the solution.
Step 5. Calculate pH.


Step 1. Write the chemical equation for the reaction between HF and NaOH.

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Problem Details

100.0 mL of a 0.50 M aqueous NH3 solution is mixed with 200.0 mL of 0.25 M aqueous HI. At 25°C the mixture will have a pH of 

a. not enough information is given
b. = 7.00
c. > 7.00
d. < 7.00

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What scientific concept do you need to know in order to solve this problem?

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