ap semester 1 units 3,4, 5

Front

What is the equilibrium constant (Kp) for the reaction 2 PF3(g) ⇌ 2 P(s) + 3 F2(g) when the pressure of the reaction mixture at equilibrium is 2.4 atm?

Back

Kp = 1.2

Front

What is the pH of a 0.010 M HCl solution after adding 90.0 mL of water to a 10.0 mL sample?

Back

pH = 3.0

Front

Which acid is the strongest among Acetic acid (CH₃COOH), Chloroacetic acid (CH₂ClCOOH), Dichloroacetic acid (CHCl₂COOH), and Trichloroacetic acid (CCl₃COOH)?

Back

Trichloroacetic acid (CCl₃COOH) is the strongest due to three chlorine atoms increasing electron withdrawal and acidity.

Front

In a 3.0 L solution containing 0.800 mol of a weak acid HA, which species is in the greatest concentration after adding 0.800 mol of NaOH?

Back

A⁻ is in the greatest concentration.

Front

What happens to the concentration of F- when 0.0010 mol of HCl is added to a 0.10 M HF solution?

Back

The concentration of [F-] will be the lowest when 0.0010 mol of HCl is added.

Front

Define the term 'equilibrium constant' in the context of chemical reactions.

Back

The equilibrium constant (K) is a numerical value that expresses the ratio of the concentrations of products to reactants at equilibrium.

Front

What is the relationship between pressure and equilibrium constant (Kp) for gaseous reactions?

Back

Kp is directly related to the partial pressures of the gases at equilibrium.

Front

Explain the concept of pH and its significance in chemistry.

Back

pH is a measure of the acidity or basicity of a solution, indicating the concentration of hydrogen ions (H+).

Front

What is the effect of adding a strong acid to a weak acid solution?

Back

Adding a strong acid increases the concentration of H+ ions, shifting the equilibrium and affecting the dissociation of the weak acid.

Front

How does the presence of electronegative substituents affect the acidity of carboxylic acids?

Back

Electronegative substituents increase acidity by stabilizing the negative charge on the conjugate base.