Q: Which of the following statements best describes the behavior of strong acids and strong bases in water?

They completely ionize, so $$[\text{H}^+]$$ and $$[\text{OH}^-]$$ are equal to the initial concentration of the acid or base.

Q: If the pH of a solution is 4.34, what is the $$[\text{H}^+]$$ concentration?

$$[\text{H}^+] = 10$$^{-4.34}$$\ \text{M}$$

Q: A 25 mL sample of 5.45 \times $$10^{-4} M $$LiOH is prepared. What is the number of moles of LiOH in the sample?

$$1.36 \times 10$$^{-5}$$\ \text{mol}$$

Q: HI is a strong acid with $$K_a = 3.2 \times 10^9$. If you have a 7.1 \times 10$$^{-4}$$ M solution of HI, what is the $$[\text{H}^+]$$ concentration?

$$[\text{H}^+] = 7.1 \times 10$$^{-4}$$\ \text{M}$$

Q: Which of the following best explains why the pH and pOH of a strong acid and strong base solution are related by $$\text{pH} + \text{pOH} = 14 at 25$$°C?

Because the product of $$[\text{H}^+]$$ and $$[\text{OH}^-] is $$always $$1.0 \times 10$$^{-14}$$ at 25°C.

Q: A solution is made by dissolving 0.25 mol of Ca(OH)$$_2 in $$enough water to make 1.2 L of solution. What is the $$[\text{OH}^-] in $$the solution?

$$[\text{OH}^-] = 2 \times \dfrac{0.25}{1.2}\ \text{M}$$

Q: Which of the following is the correct formula to calculate the pOH of a solution given the $$[\text{OH}^-]$$?

$$\text{pOH} = -\log([\text{OH}^-])$$

Question 1

Which of the following statements best describes the behavior of strong acids and strong bases in water?

Accepted Answer

They completely ionize, so $$[	ext{H}^+]$$ and $$[	ext{OH}^-]$$ are equal to the initial concentration of the acid or base.

Question 2

Given a 0.25 M solution of HCl, a strong acid, what is the concentration of $$[	ext{H}^+] in $$the solution?

Accepted Answer

$$0.25\ 	ext{M}$$

Question 3

A 0.398 M solution of Ba(OH)$$_2 is $$prepared. What is the pOH of the solution? (Assume complete dissociation.)

Accepted Answer

$$	ext{pOH} = -\log(0.796)$$

Question 4

Which of the following ions is NOT typically found in a strong base?

Accepted Answer

$$	ext{NH}_4^+$$

Question 5

If the pH of a solution is 4.34, what is the $$[	ext{H}^+]$$ concentration?

Accepted Answer

$$[	ext{H}^+] = 10$$^{-4.34}$$\ 	ext{M}$$

Question 6

A 25 mL sample of 5.45 	imes $$10^{-4} M $$LiOH is prepared. What is the number of moles of LiOH in the sample?

Accepted Answer

$$1.36 	imes 10$$^{-5}$$\ 	ext{mol}$$

Question 7

HI is a strong acid with $$K_a = 3.2 	imes 10^9$. If you have a 7.1 	imes 10$$^{-4}$$ M solution of HI, what is the $$[	ext{H}^+]$$ concentration?

Accepted Answer

$$[	ext{H}^+] = 7.1 	imes 10$$^{-4}$$\ 	ext{M}$$

Question 8

Which of the following best explains why the pH and pOH of a strong acid and strong base solution are related by $$	ext{pH} + 	ext{pOH} = 14 at 25$$°C?

Accepted Answer

Because the product of $$[	ext{H}^+]$$ and $$[	ext{OH}^-] is $$always $$1.0 	imes 10$$^{-14}$$ at 25°C.

Question 9

A solution is made by dissolving 0.25 mol of Ca(OH)$$_2 in $$enough water to make 1.2 L of solution. What is the $$[	ext{OH}^-] in $$the solution?

Accepted Answer

$$[	ext{OH}^-] = 2 	imes \dfrac{0.25}{1.2}\ 	ext{M}$$

Question 10

Which of the following is the correct formula to calculate the pOH of a solution given the $$[	ext{OH}^-]$$?

Accepted Answer

$$	ext{pOH} = -\log([	ext{OH}^-])$$

Question 11

A nurse needs to prepare 100 mL of a 0.10 M NaOH solution. How many grams of NaOH are required? (Molar mass of NaOH = 40.0 g/mol)

Accepted Answer

$$0.40\ 	ext{g}$$

Question 12

A 0.50 M solution of NH$$_2^- is $$prepared. What is the $$[	ext{OH}^-] in $$the solution, assuming complete dissociation?

Accepted Answer

$$0.50\ 	ext{M}$$

Question 13

If a solution has a pOH of 3.0, what is its pH at 25°C?

Accepted Answer

$$	ext{pH} = 11.0$$

Question 14

A laboratory technician accidentally mixes 0.10 M HCl and 0.10 M NaOH in equal volumes. What is the resulting pH of the mixture?

Accepted Answer

$$	ext{pH} = 7.0$$

Question 15

Which of the following best describes the relationship between the concentration of a strong base and the pOH of its solution?

Accepted Answer

As the concentration of the strong base increases, the pOH decreases.

Strong Acids, Strong Bases, and pH/pOH Calculations in GOB Chemistry

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