I don't get how to do this:

What is the pH of the solution created by combining 11.30 mL of the 0.10 M NaOH(aq) with 8.00 mL of the 0.10 M HCl(aq)? with 8.00 mL of the 0.10 M HC2H3O2(aq)?

What are the pH values if you take into account that the 8.00 mL of 0.10 M Acid was first diluted with 100 mL of water?

right you either go in to school and ask your chemistry or do it the messy way; get 11.30ml of the 0.10m NaOH(aq) with 8.00ml of the 0.10m HCI(aq) with 8.00ml of the 0.10m HC2H302(aq). mix them all together then look at the colour an there is you pH solution for that question.

by the way im only in year 8 at school.-you should know this

this is not done in lab. it's supposed to be calculated. people, like you, fail.

This is a buffer solution disguised so it's a little harder to recognize.

mols NaOH = L x M = 0.01130 x 0.100 M = ??
mols HCl = L x M = 0.00800 x 0.100 M = ??

Since the equation for the strong base and strong base is 1:1; i.e.,
NaOH + HCl ==> NaCl + H2O
Just subtracting mols NaOH - mols HCl will give you the amount of NaOH remaining (since it is the reagent in excess). THEN, you just have an equation of a strong base with a weak acid; i.e.,
NaOH + HC2H3O2 ==> NaC2H3O2 + H2O

which produces a buffer with the salt and the weak acid.

Calculate mols NaOH left from the first reaction. Calculate mols HC2H3O2 added. Determine the amount of HC2H3O2 left after the NaOH reaction and the amount of C2H3O2^- ion produced. You now have a weak acid and its conjugate base (HC2H3O2/C2H3O2^-) and you can use the Henderson-Hasselbalch equation.
pH = pKa + log(base/acid)
Post your work if you get stuck.

Doing it in the lab IS one way of solving some of these problems and lab work is quite important; however, one must ALSO know how to calculate the answers. A good chemist must know how to do both; that is, must be good in the lab as well as in theory. In this case, the problem is to be solved by calculation.

how the hell do u do this. just give me thanswER!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!!

To find the pH of a solution, we need to know the concentration of H+ ions present in the solution. There are a few steps involved in calculating the pH of a solution. Let's break it down step by step:

1. Calculate the moles of the acid and base: To determine the moles of NaOH and HCl, we can use the formula: Moles = Concentration (M) × Volume (L). For example, the moles of NaOH can be calculated as follows: 0.10 M × 0.01130 L = 0.00113 moles. Calculate the moles for HCl and HC2H3O2 as well.

2. Determine the limiting reactant: To find the pH of the resulting solution, we need to identify the limiting reactant—the reactant that is completely consumed in the reaction. Compare the moles of HCl with those of NaOH and HC2H3O2. The limiting reactant is the one with the fewest moles.

3. Calculate the moles of H+ ions: Since HCl is a strong acid, it completely dissociates in water, so the number of moles of H+ ions is equal to the moles of HCl. For HC2H3O2, it is a weak acid, so it only partially dissociates. As a result, we need to use the Henderson-Hasselbalch equation to determine the moles of H+ ions.

4. Calculate the concentration of H+ ions: Divide the moles of H+ ions by the total volume of the resulting solution (11.30 mL + 8.00 mL + 100 mL for the diluted acid case).

5. Calculate the pH: The pH is calculated using the formula: pH = -log[H+]. Plug in the concentration of H+ ions calculated in the previous step to determine the pH.

For the diluted acid case, you will have to account for the extra 100 mL of water added. This will affect the overall volume but not the concentration of H+ ions. Repeat steps 4 and 5 using the correct total volume (11.30 mL + 8.00 mL + 100 mL) to calculate the pH in this scenario.