State whether the pH at the equivalence point in each of the following titrations is expected to be less than 7, equal to 7, or greater than 7. a. Strong acid (e. g. HCl) with strong base (e. g. NaOH) b. Weak acid (e. g. acetic acid, CH3COOH) with strong base (e. g. NaO

A. equal to 7

B. greater than 7

Explanation:

a. Strong acid (e.g. HCl) with strong base (e.g. NaOH)

HCl + NaOH ⇒ NaCl + H₂O

The reaction of HCl and NaOH will form a neutral salt, NaCl. So, the pH at the equivalence point will be equal to 7.

b. Weak acid (e.g. acetic acid, CH₃COOH) with strong base (e.g. NaOH)

CH₃COOH + NaOH ⇒ CH₃COONa + H₂O

The reaction of CH₃COOH and NaOH will form a basic salt, CH₃COONa. So, the pH at the equivalence point will be greater than 7.

fe 55.85 g/mol and h2o 18.02 g/mol.

every chemical equation adheres to the law of conservation of mass, which states that matter cannot be created or destroyed. therefore, there must be the same number of atoms of each element on each side of a chemical equation.