1.When mixing 45mL of 0.65M acetic acid with 65mL of 0.45M NaOH the resulting mixture is

a. basic
b. neutral
c. acidic
d. pH < 7
e. both c and d
The correct answer is b. neutral right?

2.The concentration of [OH-] in Al(OH)3 is 2.6 x 10^-5. What is the concentration of Al3+?

a.7.8 x 10^-5
b.5.2 x 10^-5
c.8.7 x 10^-6
d.7.8 x 10^-15
The answer is c right

2 is right. 1 is wrong. For 1, it is true that the number of mols acid - number of mols base; however, remember that the salt formed hydrolyzes.

So what would the correct answer for 1 be?

You tell me. If I let HAc stand for acetic acid and NaAc is sodium acetate, then

HAc + NaOH ==> NaAc + H2O
Now you write the equation for the hydrolysis of the acetate ion (Ac^-) and the answer will be obvious. (Hint: hydrolysis means reacting with water)

1. To determine the answer to this question, you need to calculate the moles of acetic acid and NaOH, and then compare the number of moles of acidic and basic components present.

First, calculate the moles of acetic acid:

moles of acetic acid = volume of acetic acid (in L) x concentration of acetic acid (in mol/L)
= 45 mL / 1000 mL/L x 0.65 mol/L
= 0.02925 mol

Next, calculate the moles of NaOH:

moles of NaOH = volume of NaOH (in L) x concentration of NaOH (in mol/L)
= 65 mL / 1000 mL/L x 0.45 mol/L
= 0.02925 mol

Since the moles of acetic acid and NaOH are equal, they will react in a 1:1 ratio according to the balanced equation for the reaction between acetic acid and NaOH:

CH3COOH + NaOH -> CH3COONa + H2O

This means that all the acetic acid will react with NaOH, resulting in the formation of water and sodium acetate. Therefore, the resulting mixture will be neutral (option b).

2. To determine the concentration of Al3+ in Al(OH)3 from the concentration of OH-, you need to know the solubility constant (Ksp) of Al(OH)3.

The balanced equation for the dissociation of Al(OH)3 in water is:

Al(OH)3 -> Al3+ + 3OH-

The Ksp expression for Al(OH)3 is:

Ksp = [Al3+][OH-]^3

Given that the concentration of OH- is 2.6 x 10^-5, you can plug it into the Ksp expression:

Ksp = (unknown concentration of Al3+)(2.6 x 10^-5)^3

To solve for the unknown concentration of Al3+, you need the value of Ksp for Al(OH)3. Without that information, it is not possible to accurately determine the concentration of Al3+.

Therefore, it is not possible to determine the correct answer to this question without the Ksp value for Al(OH)3.