8. Calculate the pH of a solution prepared by mixing 0.00255 moles of HCl in 150

Question

8. Calculate the pH of a solution prepared by mixing 0.00255 moles of HCl in 150.0 mL of water. (Report your answer to 2 decimal places)

9. Calculate the pH of a solution prepared by mixing 0.00125 moles of C6H5COO- (Ka = 6.5 x10-5) in 150.0 mL of water. (Report your answer to 2 decimal places)

10. How much 1.50 M CH3COOH (Ka=1.8 x10-5) is required to prepare a 100.0 mL solution of CH3COOH with a pH of 2.60.

11. How much 0.150 M HCl is required to prepare a 100.0 mL solution of HCl with a pH of 2.10.

The rate of for the reaction was determined experimentally to be: R = k[NO2]2

Based on the information presented above, doubling the concentration of CO2 will:

a. Decrease the reaction rate by 1/2

b. Not change the reaction rate

c. Increase the reaction rate by 2

d. Increase the reaction rate by 4

The rate of for the reaction was determined experimentally to be: R = k[C4H6][I2]2

Based on the information presented above, doubling the concentration of I2 will:

a. Decrease the reaction rate by 1/2

b. Not change the reaction rate

c. Increase the reaction rate by 2

d. Increase the reaction rate by 4

23. Which of the following metals will result in the biggest gap when complexed with the CN- ion?

a. Fe+

b. Fe2+

c. Fe3+

d. Fe4+

Explanation / Answer

8)

concentration of HCl = moles of HCl / volume in L

= 0.00255 mol / 0.1500 L

= 0.0170 M

So,

[H+] = 0.0170 M

we have below equation to be used:

pH = -log [H+]

= -log (1.7*10^-2)

= 1.77

Answer: 1.77

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