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Calculating pH and pOH Worksheet Answers Key, Exercises of Chemistry

Find out pH and pOH of a 0.0235 M HCl solution at Everett Community College Tutoring Center Student Support Services Program.

Typology: Exercises

2020/2021

Uploaded on 04/20/2021

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Calculating pH and pOH worksheet
W 335
Everett Community College Tutoring Center
Student Support Services Program
1) What is the pH of a 0.0235 M HCl solution?
2) What is the pOH of a 0.0235 M HCl solution?
3) What is the pH of a 6.50 x 10-3 M KOH solution? (Hint: this is a basic solution
concentration is of OH -)
4) A solution is created by measuring 3.60 x 10-3 moles of NaOH and 5.95 x 10-4 moles of
HCl into a container and then water is added until the final volume is 1.00 L. What is
the pH of this solution?
5) What is the pH of a 6.2 x 10-5 M NaOH solution? (Hint: this is a basic solution
concentration is of OH -)
6) A solution with a H+ concentration of 1.00 x 10-7 M is said to be neutral. Why?
pf2

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Calculating pH and pOH worksheet

W 335

Everett Community College Tutoring Center Student Support Services Program

1) What is the pH of a 0.0235 M HCl solution?

2) What is the pOH of a 0.0235 M HCl solution?

3) What is the pH of a 6.50 x 10-3^ M KOH solution? (Hint: this is a basic solution –

concentration is of OH

4) A solution is created by measuring 3.60 x 10-3^ moles of NaOH and 5.95 x 10-4^ moles of

HCl into a container and then water is added until the final volume is 1.00 L. What is

the pH of this solution?

5) What is the pH of a 6.2 x 10-5^ M NaOH solution? (Hint: this is a basic solution –

concentration is of OH

6) A solution with a H+^ concentration of 1.00 x 10-7^ M is said to be neutral. Why?

Solutions Note: The significant figures in the concentration of [H+] or [OH - ] is equal to the number of decimal places in the pH or pOH and vice versa.

1) What is the pH of a 0.0235 M HCl solution?

pH = -log[H+] = -log(0.0235) = 1.

2) What is the pOH of a 0.0235 M HCl solution?

pH = -log[H+] = -log(0.0235) = 1. pOH = 14.000 pH = 14.000 1.629 = 12.

3) What is the pH of a 6.50 x 10-3^ M KOH solution?

pOH = -log[OH-] = -log(6.50 x 10-3) = 2. pH = 14.000 pOH = 14.000 2.187 = 11.

4) A solution is created by measuring 3.60 x 10-3^ moles of NaOH and 5.95 x 10-4^ moles of

HCl into a container and then water is added until the final volume is 1.00 L. What is

the pH of this solution?

Since there is both acid and base we will assume a 1 mole acid:1 mole base ratio of neutralization. There is more base than acid so the leftover base is what will affect the pH of the solution. 3.60 x 10-3^ moles - 5.95 x 10-4^ moles = 3.01 x 10-3^ moles NaOH 3.01 x 10-3^ moles NaOH = 3.01 x 10-3^ M NaOH 1.00 L soln pOH = -log[OH-] = -log(3.01 x 10-3) = 2. pH = 14.000 pOH = 14.000 2.521 = 11.

5) What is the pH of a 6.2 x 10-5^ M NaOH solution?

pOH = -log[OH-] = -log(6.2 x 10-5) = 4.

pH = 14.00 pOH = 14.00 4.21 = 9.

6) A solution with a H+^ concentration of 1.00 x 10-7^ M is said to be neutral. Why?

pH = -log[H+] = -log(1.00 x 10-7) = 7. pOH = 14.000 pH = 14.000 7.000 = 7. pOH = -log[OH-] = -log(OH-) = 7.000 we can use this to find the OH-^ concentration -log[OH-] = 7. log[OH-]-1^ = 7. log[OH-]-1^ 7. 10 = 10 [OH-]-1^ = 107. 1 = 107. [OH-]

[OH-] = 1.00 x 10-7^ M The concentrations of H+^ and OH-^ are equal, as are the pH and pOH, so the solution must be neutral.