Which of the following mixtures would result in buffered solutions when 1.0 L of each of the two solutions are mixed?

a) 0.10 M NaCl and 0.10 M NaNO2
b) 0.10 M NaCl and 0.10 M NH4Cl
c) 0.10 M CH3NH2 and 0.15 M CH3NH3Cl
d) 0.10 M HCl and 0.05 M NaNO2
e) 0.10 M HCL and 0.20 M NaC2H302
f) 0.1 M CH3COO and 0.15 M NaC2H5OO

Please explain i have a final tomorrow.

I know the a buffer is a mixture of a weak acid or base ans its conjugate base.

So d and e have HCl which is a strong acid so they are not one of the right answers i think.

c is a buffered solution. CH3CH2NH2 is a weak base (ethyl amine) and the salt. I don't think any of the other will qualify.

a is a salt and a salt.
b is a salt and a salt.
c is buffered.
d and e, as you correctly point out, contain a strong acid so they are out.

You are correct that options d) and e) are not buffered solutions because they contain a strong acid, HCl. A buffered solution requires a weak acid or base and its conjugate base or acid.

Let's analyze the remaining options:

a) 0.10 M NaCl and 0.10 M NaNO2:
This mixture does not contain any weak acid or base, so it is not a buffered solution.

b) 0.10 M NaCl and 0.10 M NH4Cl:
This mixture contains NH4Cl, which is a weak acid, and its conjugate base, NH3. Therefore, this is a buffered solution.

c) 0.10 M CH3NH2 and 0.15 M CH3NH3Cl:
This mixture contains CH3NH2, which is a weak base, and its conjugate acid, CH3NH3+. Therefore, this is a buffered solution.

f) 0.1 M CH3COO and 0.15 M NaC2H5OO:
This mixture contains CH3COO-, which is a weak base, and its conjugate acid, HC2H5OOH. Therefore, this is a buffered solution.

So the correct choices for buffered solutions are b), c), and f).

You're correct, a buffer solution is a mixture of a weak acid and its conjugate base or a weak base and its conjugate acid. The buffer solution helps to resist changes in pH when small amounts of strong acid or base are added to it.

Let's go through each of the given options:

a) 0.10 M NaCl and 0.10 M NaNO2
In this case, we have NaCl (a strong salt) and NaNO2 (a strong salt). Since both components are strong, this mixture will not act as a buffer.

b) 0.10 M NaCl and 0.10 M NH4Cl
Here, we have NaCl (a strong salt) and NH4Cl (a weak acid and its conjugate base). Since NH4Cl contains the weak acid NH4+ and its conjugate base Cl-, this mixture can act as a buffer.

c) 0.10 M CH3NH2 and 0.15 M CH3NH3Cl
CH3NH2 (methylamine) is a weak base and CH3NH3Cl is its conjugate acid. Since this mixture contains a weak base and its conjugate acid, it can act as a buffer.

d) 0.10 M HCl and 0.05 M NaNO2
As you correctly pointed out, HCl is a strong acid, so this mixture will not act as a buffer.

e) 0.10 M HCl and 0.20 M NaC2H302
Similar to the previous case, HCl is a strong acid, so this mixture will not act as a buffer.

f) 0.1 M CH3COO and 0.15 M NaC2H5OO
CH3COOH (acetic acid) is a weak acid and NaC2H5OO (sodium acetate) is its conjugate base. Since this mixture contains a weak acid and its conjugate base, it can act as a buffer.

Therefore, the buffered solutions are b) 0.10 M NaCl and 0.10 M NH4Cl and f) 0.1 M CH3COO and 0.15 M NaC2H5OO.

Remember to always check if the combination consists of a weak acid (or base) and its conjugate base (or acid) to determine if a solution can act as a buffer. Good luck on your final!