calculate the ph at the equivalence point for the titration of 0.01 M Ch3COOH with 0.1 M NaoH ka= Ch3Cooh 1.8E-5

idek how to do it?

To calculate the pH at the equivalence point for the titration of acetic acid (CH3COOH) with sodium hydroxide (NaOH), we need to consider the stoichiometric relationship between the acid and the base.

The balanced chemical equation for the reaction between CH3COOH and NaOH is as follows:

CH3COOH + NaOH -> CH3COONa + H2O

At the equivalence point, the moles of CH3COOH completely react with the moles of NaOH, resulting in the formation of equal moles of CH3COONa (sodium acetate) and water (H2O).

Since the initial concentration of CH3COOH is given as 0.01 M and the concentration of NaOH is given as 0.1 M, we need to determine how many moles of CH3COOH and NaOH are present at the equivalence point.

To find the moles of CH3COOH, we can use the equation:

moles of CH3COOH = initial concentration × volume

Assuming we have a volume of V mL of CH3COOH, the moles of CH3COOH can be calculated as:

moles of CH3COOH = (0.01 M) × (V/1000 L)

Since CH3COOH and NaOH react in a 1:1 ratio, the moles of NaOH will also be equal to the moles of CH3COOH at the equivalence point.

Now that we have established the moles of CH3COOH and NaOH at the equivalence point, we can calculate the concentrations of CH3COONa and H2O using the same equation:

concentration = moles/volume

The concentration of CH3COONa will be equal to the moles of CH3COOH divided by the total volume of the solution (V mL).

To calculate the pH at the equivalence point, we need to consider the dissociation of CH3COOH in water.

CH3COOH is a weak acid, and it partially dissociates in water to form CH3COO- (acetate ion) and H+ (hydrogen ion). The dissociation equation is:

CH3COOH <-> CH3COO- + H+

The equilibrium constant for this reaction is given as Ka = 1.8 × 10^-5.

Using the equation for Ka, we can write the expression for the dissociation of CH3COOH as:

Ka = [CH3COO-][H+] / [CH3COOH]

Since the moles of CH3COOH and CH3COONa are equal at the equivalence point, the concentration of CH3COO- will also be equal to the concentration of CH3COONa.

At the equivalence point, the concentration of CH3COOH will be equal to the initial concentration minus the concentration of CH3COONa.

Now, we need to solve for [H+] in the dissociation equation.

[H+] = (Ka × [CH3COOH]) / [CH3COO-]

Finally, the pH can be calculated using the equation:

pH = -log[H+]

Substituting the calculated value of [H+] into this equation will give you the pH at the equivalence point for this titration.

Note: This calculation assumes that the volume of NaOH required to reach the equivalence point is known.

To calculate the pH at the equivalence point for the titration of a weak acid with a strong base, you need to determine the concentration of the conjugate base just before reaching the equivalence point. In this case, the weak acid is CH3COOH (acetic acid) and the strong base is NaOH.

Step 1: Write the balanced chemical equation for the neutralization reaction between CH3COOH and NaOH:
CH3COOH + NaOH -> CH3COONa + H2O

Step 2: Determine the moles of CH3COOH and NaOH used. Since you have a 1:1 stoichiometric ratio, the moles of CH3COOH used will be equal to the moles of NaOH used.

Step 3: Use the equation C1V1 = C2V2 to find the volume of NaOH required to reach the equivalence point. Assume that the volume and concentration of CH3COOH are known, and that the volume of NaOH at the equivalence point is V2.

Step 4: Calculate the concentration of the conjugate base (CH3COONa) just before the equivalence point. This can be done by dividing the number of moles of CH3COOH at the equivalence point by the total volume of the solution at that point.

Step 5: Calculate the pOH at the equivalence point by taking the negative logarithm of the concentration of the conjugate base, following the formula: pOH = -log[CH3COONa].

Step 6: Use the equation pH + pOH = 14 to calculate the pH at the equivalence point.

Note: Since acetic acid is a weak acid, the pH at the equivalence point will be slightly greater than 7 due to the presence of the conjugate base.

By following these steps, you can calculate the pH at the equivalence point for the titration of CH3COOH with NaOH.