What is the pH of the solution created by combining 0.80 mL of the 0.10 M NaOH(aq)with 8.00 mL of the 0.10 M HC2H3O2(aq)?

Look at the equation. Base + acid = salt + water.

NaOH + HC2H3O2 ==> NaC2H3O2 + H2O

Calculate the moles NaOH to start.
Calculate the moles HC2H3O2 to start. I haven't done the calculation but I assume that the HC2H3O2 will be in excess and all of the NaOH will be used. So you end up with a buffered solution, which in this case is a weak acid (HC2H3O2) and its salt (in this case NaC2H3O2.
Now use the Henderson-Hasselbalch equation,
pH = pKa + log (base/acid) to calculate pH.

To find the pH of the solution created by combining the given solutions, we need to use the concept of acid-base reactions and the properties of the components.

Step 1: Write the balanced chemical equation
NaOH(aq) + HC2H3O2(aq) → NaC2H3O2(aq) + H2O(l)

Step 2: Identify the strong acid and strong base
In this equation, NaOH is a strong base, and HC2H3O2 is a weak acid.

Step 3: Determine the moles of each component
Given that the volume and concentration of NaOH are 0.80 mL and 0.10 M, respectively, we need to convert the volume to liters and then multiply by the concentration to find the moles. Similarly, for HC2H3O2, the volume is 8.00 mL, and the concentration is 0.10 M. Again, convert the volume to liters before calculating the moles.

Moles of NaOH = (0.80 mL / 1000 mL/L) * 0.10 M = 0.008 mol
Moles of HC2H3O2 = (8.00 mL / 1000 mL/L) * 0.10 M = 0.080 mol

Step 4: Determine the limiting reactant
Compare the molar ratios of the reactants to identify the limiting reactant. In this case, HC2H3O2 is the limiting reactant because each mole of NaOH requires one mole of HC2H3O2.

Step 5: Determine the concentration of the resulting solution
Since HC2H3O2 is the limiting reactant, it will be entirely consumed in the reaction. Therefore, the final volume of the solution will be the sum of the initial volumes of NaOH and HC2H3O2.

Final volume = 0.80 mL + 8.00 mL = 8.80 mL = 0.0088 L

Step 6: Determine the concentration of the resulting solution
To calculate the concentration of the resulting solution, divide the moles of the limiting reactant by the final volume.

Concentration of NaC2H3O2 = (0.080 mol / 0.0088 L) = 9.09 M

Step 7: Calculate the pOH
pOH = -log[OH-]
Since NaOH is a strong base and completely dissociates in water, the concentration of OH- ions is the same as the concentration of NaOH.

pOH = -log(0.10 M) = 1

Step 8: Calculate the pH
pH = 14 - pOH = 14 - 1 = 13

Therefore, the pH of the solution created by combining 0.80 mL of 0.10 M NaOH(aq) with 8.00 mL of 0.10 M HC2H3O2(aq) is 13.