Calculating pH of Buffered Solutions: Do You Need a Ka/Kb Value?

In summary, the conversation discusses a question about calculating the pH of a buffered solution in AP Chemistry homework. The question only provides the chemical formula and molarity, and the person is unsure how to find the pH without a Ka/Kb value. Suggestions are given to Google the species name or check for a pKa table in the book.
  • #1
Dpasi314
1
0
Hello,
So as the end of the year comes to an end, AP Chemistry is getting increasingly more difficult to the point where I don't understand anymore. In our homework there is a questions asking to calculate the pH of a buffered solution. The only information it gives you is the chemical formula and the molarity. i.e
Calculate the pH of each of the following buffered solutions:
a. 0.50 M C2H5NH2/0.25 M C2H5NH3Cl

I'm not quite sure how I'm suppose to be able to figure out the pH without having a Ka/Kb value given? Is the question assuming that I need to know what the Ka/Kb value? Or am I missing something entirely?

Thanks for the help!
 
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  • #2
Hi Dpasi314. Welcome to Physics Forums.

Do you know the name of the 0.5 M species? If so, have you tried Googling it? It should take less than a minute to find the Kb.

Chet
 
  • #3
Perhaps you were given a pKa table? Or there is one in your book?
 

1. What is equilibrium in chemistry?

Equilibrium in chemistry refers to a state where the forward and reverse reactions of a chemical reaction are occurring at the same rate, resulting in no net change in the concentrations of reactants and products.

2. How is equilibrium achieved in a chemical reaction?

Equilibrium is achieved when the rate of the forward reaction is equal to the rate of the reverse reaction. This can be achieved by altering the concentration, temperature, or pressure of the system.

3. What is the significance of equilibrium in chemistry?

Equilibrium is important because it allows for the production of desired products in chemical reactions. It also helps to maintain a stable environment, as any changes to the equilibrium can be quickly corrected.

4. What is pH and how does it relate to equilibrium?

pH is a measure of the acidity or basicity of a solution. In a chemical equilibrium, the concentration of hydrogen ions (H+) and hydroxide ions (OH-) can affect the pH of the solution. pH can also impact the direction of a chemical reaction towards either the reactants or products.

5. How can pH be controlled in a chemical reaction?

pH can be controlled by adding acids or bases to the solution, which will increase or decrease the concentration of hydrogen ions. Additionally, changing the temperature or pressure can also impact the pH of a solution and shift the equilibrium towards the desired products.

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