We’re being asked to calculate the pH of a solution made by mixing 100.0 mL of 0.644 M CH3NH2 with 100.0 mL of 0.100 M HCl.
We will calculate the pH of the solution using the following steps:
Step 1. Write the chemical equation for the reaction between CH3NH2 and HCl.
Step 2. Calculate the initial amounts of CH3NH2 and HCl 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.
Methylamine (CH3NH2) has a Kb = 4.4 x 10-4. If 100.0 mL of a 0.5000 M aqueous methylamine solution is mixed with 100.0 ml of 0.5000 M aqueous hydrochloric acid, the resulting solution will have a pH
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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.
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Our tutors rated the difficulty ofMethylamine (CH3NH2) has a Kb = 4.4 x 10-4. If 100.0 mL of a...as high difficulty.
What professor is this problem relevant for?
Based on our data, we think this problem is relevant for Professor Carlson's class at UWM.