Question

Consider the titration of a 23.0 ml sample of 0.105 moll-1 ch3cooh (ka=1.8×10-5) with 0.130 moll-1 naoh. Determine the volume of added base required to reach the equivalence point?

Answer 1

To determine the volume of added base required to reach the equivalence point in the titration of CH3COOH (acetic acid) with NaOH, you need to calculate the number of moles of acid and base present and use the equation n(CH3COOH)/v(CH3COOH) = n(NaOH)/v(NaOH). Then, rearrange the equation to solve for v(NaOH) and plug in the values to find the volume of added base required.

Step-by-step explanation:

To determine the volume of added base required to reach the equivalence point in the titration of CH3COOH (acetic acid) with NaOH, you first need to calculate the number of moles of acid (CH3COOH) and base (NaOH) present. Then, using the equation n(CH3COOH)/v(CH3COOH) = n(NaOH)/v(NaOH), you can find the unknown volume of NaOH required for neutralization.

1. Calculate the number of moles of CH3COOH: n(CH3COOH) = c(CH3COOH) * v(CH3COOH), where c(CH3COOH) is the concentration and v(CH3COOH) is the volume of the acid.
2. Calculate the number of moles of NaOH: n(NaOH) = c(NaOH) * v(NaOH), where c(NaOH) is the concentration and v(NaOH) is the unknown volume of the base.
3. Setting the moles of acid equal to the moles of base: n(CH3COOH) = n(NaOH).
4. Rearrange the equation to solve for v(NaOH): v(NaOH) = n(NaOH) / c(NaOH).

Plug in the values and calculate v(NaOH) to find the volume of added base required to reach the equivalence point in the titration.