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

precipitation

explanation:

when it goes from cloud to rain/back to earth in the form of rain

answer: c.

explanation: