Acids and Bases Molarity Calculations

What will be the pH of a 0.10 M HCl solution?

• 1.00
• 0.10
• 10.00
• 7.00

What is the formula for the conjugate base of the bicarbonate HCO₃^- ion?

• CO₃^2-
• H₂CO₃
• H₃CO₃⁺
• CO₂

How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 

• 2
• 3
• 4
• 6 

The pH of a substance is defined as:

• log[H+]

• –log[H–]

• -log[H+]

• –log[OH–]

Which concentration indicates a basic solution at 298 K?

• [OH–] > 1.0 × 10^–7

• [H3O+] > 1.0 × 10^–7

• [OH–] = 1.0 × 10^–7

• [H3O+] = 1.0 × 10^-7

A solution of acid A has a pH of 1 and a solution of acid B has a pH of 2. Which statement must be correct?

• Acid A is stronger than acid B.

• [A]>[B]

• The concentration of H+ ions in A is higher than in B

• The concentration of H+ ions in B is twice the concentration of

  H+ ions in A.

As the [H₃O⁺] in a solution decreases, the [OH^-]

• increases and the pH increases.

• increases and the pH decreases.

• decreases and the pH increases.

• decreases and the pH decreases.

Which of these solutions, all with a concentration 0.2 M, will have the highest pH?

• HF  Ka = 7.2 x 10^-4
• benzoic acid Ka = 6.3 x 10^-5
• H₂SO₃ Ka = 1.2 x 10^-2
• H₃O⁺  Ka = 55.5

Tags

NGSS.HS-PS1-1

I have 25mL of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?

• 0.8 M
• 1 M
• 1.25 M

Tags

NGSS.HS-PS1-7

The following neutralization reaction occurs in the classroom.
HCl  +  KOH  -->  H₂O  +  KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if 15.0mL of acid neutralized?

• 0.8M
• 1.2M
• 12.5M

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-7