Calculate the mass of sodium acetate that must be added to 500.0 mL of 0.300 M acetic acid to form a pH

22.4 g

Explanation:

Calculate the mass of sodium acetate that must be added to 500.0 mL of 0.300 M acetic acid to form a pH  = 5.00 buffered solution.

Step 1: Given data

Volume of solution: 500.0 mL

[acetic acid]: 0.300 M

pH = 5.00

pKa of acetic acid: 4.74

Step 2: Calculate the concentration of sodium acetate

We will use the Henderson-Hasselbach equation.

pH = pKa + log [sodium acetate]/[acetic acid]

5.00 = 4.74 + log [sodium acetate]/0.300 M

[sodium acetate] = 0.546 M

Step 3: Calculate the moles of sodium acetate

We have 500.0 mL of a 0.546 M sodium acetate solution

0.5000 L × 0.546 mol/L = 0.273 mol

Step 4: Calculate the mass of sodium acetate

The molar mass of sodium acetate is 82.03 g/mol.

0.273 mol × 82.03 g/mol = 22.4 g

conduction is the transfer of thermal energy (heat in transfer) due to collisions between the molecules in the object. collisions between adjacent atoms and molecules transfer kinetic energy from the warmer to the cooler object. the objects must be in physical contact.