What is the pH of a 1.0 L buffer that consists of 0.0750 M c_2H_5NH_2 and 0.0500

Question

What is the pH of a 1.0 L buffer that consists of 0.0750 M c_2H_5NH_2 and 0.0500 M C_2H_5NH_2Cl after the addition of 10.0mL of 0.5 M HCP Calculate moles of C_2H_5NH_2, C_2H_5NH_2Cl, and HCl Write a reaction of the HCL with one of the other species. Set up reaction table(will use moles and stoichiometric) using the reaction as a header. Looking at your "After" line, use that information to determine what you have present in solutions and write down what you would need to in order to solve for the pH. You should be able to use either an ice table or the Henderson-Hasselbalch equation.

Explanation / Answer

The added acid (0.01 L x 5.0 moles/L) contains 0.05 moles of H3O+.

The added acid coverts 0.05 mole of base (NH2) into 0.05 mole of acid (NH3+.

After the addition of acid, 0.025 mole of NH3 and 0.10 mole NH4+ are now present in solution.

b)

C2H5NH2(aq)

+HCl(aq)

--->

C2H5NH3+(aq)

+Cl-(aq)

c)

Before

0.025

0.10

0

Reacts

-x

+x

+x

After

0.025-x

0.1+x

+x

e) Henderson-Hasselbalch equation :-

pHbuffer = pKa + log10([salt(aq)] / [acid(aq)])

Ka will be required.

C2H5NH2(aq)

+HCl(aq)

--->

C2H5NH3+(aq)

+Cl-(aq)

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