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In a titration of a 250mL solution of 0.05M ammonia (NH3) (Kb=1.8 * 10^-5) with a...

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Chemistry

In a titration of a 250mL solution of 0.05M ammonia (NH3)(Kb=1.8 * 10^-5) with a concentrated (0.2M) solution of HCL,calculate the following:

1. What is the initial pH before adding HCL?

2. What is the pH of the system after adding 20mL of the 0.2 MHCL?

3. What is the pH at equivalence?

*I have the answers, I really need to know how to do the work toget to the answers.*

Answer & Explanation Solved by verified expert
3.8 Ratings (375 Votes)
1 NH3 dissociates as NH3 H2O NH4 OH 5102 0 0 5102x x x Kb NH4OHNH3 Kb xxcx Assuming x can be ignored as compared to c So above expression becomes Kb xxc so x sqrt Kbc x sqrt 181055102 9487104 since x is comparable c our assumption is not correct we need to solve this using Quadratic equation Kb xxcx 18105 x25102x 9107 18105 x x2 x2 18105 x9107 0 This is quadratic equation ax2bxc0 a 1 b    See Answer
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