Acid & Base pH calculation

What is the [H⁺] in a solution with a pH of 11?

• 1 x 10^-1 M

• 1 x 10^-2 M

• 1 x 10¹¹ M

• 1 x 10^-11 M

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

4.605.02.57

• 4.6

• 5.0

• 2.5

• 7.0

What is the [OH-] if the [H+] is 1.0 x 10-3 M?

• 1.0 x 10-3 M

• 6.02 x 10-23 M

• 1.0 x 10-14 M

• 1.0 x 10-11 M

What is the [OH-] if the pH is 4.9?

• 7.94 x 10-10 M

• 1.0 x 10-4 M

• 7.94 x 10-14 M

• 4.9 x 10-10 M

What is the pOH of a 1 x 10^-8 M solution of HNO₃?

• 8

• 6

• 7

• 9

What completely ionizes in solution?

• Weak acids

• Strong acids

• Strong Salts

• Neutral salts

CO₃^2-(aq) + H₂O(l) → HCO₃^-(aq)+OH^-(aq)

Using the above reaction, which compound is the conjugate base?

• CO₃^2-

• H₂O

• HCO₃^-

• OH^-

An Arrhenius acid:

• donates H+ to another substance

• accepts H+ from another substance

• produces H+

• produces OH-

A Bronsted Lowry base:

• donates H+ to another substance

• accepts H+ from another substance

• produces H+

• produces OH-

In the equation below, what is the Bronsted Lowry acid?

HCl + NH₃ --> Cl^- + NH₄⁺

• HCl

• NH₃

• Cl^-

• NH₄⁺