Skip to main content

My Channels

17. Acid and Base Equilibrium

The pH Scale

17. Acid and Base Equilibrium

The pH Scale

Guided videos.

Learn with Jules

Go to the course

The pH Scale Example

The pH Scale Example

The pH Scale Example

The pH Scale Example

Additional pH and pOH Calculations

Additional pH and pOH Calculations

The pH Scale Example

The pH Scale Example

Showing 6 of 6 videos

Additional 1 creators.

Learn with other creators

Calculating the pH of a Strong Acid and Strong Base

Calculating the pH of a Strong Acid and Strong Base

00π productions

16.4 pH Calculations for Strong Acids and Bases | General Chemistry

16.4 pH Calculations for Strong Acids and Bases | General Chemistry

pH and pOH: Crash Course Chemistry #30

pH and pOH: Crash Course Chemistry #30

Acids and Bases, pH and pOH

Acids and Bases, pH and pOH

Professor Dave Explains

Practice this topic

Multiple Choice

Which of the following solutions will have the lowest concentration of hydronium ions?

Has a video solution.

Multiple Choice

Which of the following statements about aqueous solutions is/are true?

Has a video solution.

Multiple Choice

What is the Kw of pure water at 20.0°C, if the pH is 7.083?

Has a video solution.

Multiple Choice

Calculate the pH of 50.00 mL of 4.3 x 10^-7M H₂SO₄.

Has a video solution.

Multiple Choice

Determine the pH of a solution made by dissolving 6.1 g of sodium cyanide, NaCN, in enough water to make a 500.0 mL of solution. (MW of NaCN = 49.01 g/mol). The Ka value of HCN is 4.9 x 10^-10.

Has a video solution.

Multiple Choice

Which of the illustrations represents the weakest acid?

Multiple Choice

What is the pH of 0.0200 M HCl?

Multiple Choice

What is the pH of a solution of 0.0350 M Ba(OH)₂?

Multiple Choice

What is the percent ionization of 0.0550 M solution of HC₂H₃O₂?

Multiple Choice

Which of the following salts would produce a basic solution?

Multiple Choice

Rank the following in order of increasing base strength (weakest to strongest).

OI⁻ OCl⁻ OBr⁻

Multiple Choice

A solution of NaOH was prepared in a chemistry lab and the pOH was determined to be 9.3. What is the concentration of OH⁻ ions of this basic solution?

Has a video solution.

Multiple Choice

Calculate [OH⁻] of a lemon juice solution at 25°C with a [H⁺] = 5.7 × 10⁻⁴ M.

Has a video solution.

Multiple Choice

A 345 mL bottle of antacid (Mg(OH)₂) contains 1.45 × 10⁻² moles of hydroxide ions. Determine pH and pOH of the antacid.

Has a video solution.

Multiple Choice

Which of the following statement(s) on aqueous solutions is/are correct?

a) aqueous solutions have a pH of 7

b) as concentration of hydronium ion increases, concentration of hydroxide ion decreases

c) solutions of weaker acids generally have a higher pOH then solutions of stronger acids

d) pH of pure water equals to 7 at 35º C.

Has a video solution.

Textbook Question

The probe of the pH meter shown here is sitting in a beaker that contains a clear liquid. (c) Why is the temperature given on the pH meter?

Has a video solution.

Textbook Question

What is the concentration of hydroxide ions 3OH-4 in a glass of wine with pH = 3.64? (LO 16.5, 16.6) (a) 2.3 * 10-4 M (b) 6.4 * 10-3 M (c) 6.8 * 10-9 M (d) 4.4 * 10-11 M

Has a video solution.

Textbook Question

Calculate 3H+4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3OH-4 = 8.8 * 10-9 M

Has a video solution.

Textbook Question

Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (b) 3H+4 = 2.5 * 10-10 M

Has a video solution.

Textbook Question

Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (c) a solution in which 3H+4 is 1000 times greater than 3OH-4.

Has a video solution.

Textbook Question

Calculate 3OH-4 for each of the following solutions, and indicate whether the solution is acidic, basic, or neutral: (a) 3H+4 = 0.0505 M

Has a video solution.

Textbook Question

By what factor does 3H+4 change for a pH change of (a) 2.00 units?

Has a video solution.

Textbook Question

Calculate [H3O+] and [OH-] for each solution at 25 °C. b. pH = 11.23

Has a video solution.

Textbook Question

Calculate [H3O+] and [OH-] for each solution at 25 °C. a. pH = 8.55

Has a video solution.

Textbook Question

Complete the table. (All solutions are at 25 °C.)

Has a video solution.

Textbook Question

Complete the table. (All solutions are at 25 °C.)

Has a video solution.

Textbook Question

Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH of an acid solution should carry as many digits to the right of the decimal place as the number of significant figures in the concentration of the solution. [H3O+] = 0.044 M [H3O+] = 0.045 M [H3O+] = 0.046 M

Has a video solution.

Textbook Question

Determine the concentration of H3O+ to the correct number of significant figures in a solution with each pH. Describe how these calculations show the relationship between the number of digits to the right of the decimal place in pH and the number of significant figures in concentration. pH = 2.50 pH = 2.51 pH = 2.52

Has a video solution.

Textbook Question

Calculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (e) -1.0

Has a video solution.

Textbook Question

Calculate the H3O+ concentration to the correct number of significant figures for solutions with the following pH values. (d) 14.25

Has a video solution.

Textbook Question

The equivalence point was reached in titrations of three unknown bases at pH 5.53 (base A), 4.11 (base B), and 6.00 (base C). (a) Which is the strongest base? (b) Which is the weakest base?

Has a video solution.

The pH of an aqueous solution is 4.32. What is the [OH^–]?

Has a video solution.

What are the concentrations of H₃O⁺ and OH⁻ in tomatoes that have a pH of 4.10?

Has a video solution.

A solution of ammonia has a pH of 11.8. What is the concentration of OH^– ions in the solution?

Has a video solution.

What is the ratio of H⁺ ions to OH^– ions at a pH = 7?

Has a video solution.

The pH of a basic solution is 8.11. what is [H⁺]?

Has a video solution.

The pH of an acidic solution is 2.11. What is [H⁺]?

Has a video solution.

If the pH of a solution is 7, what is the molar concentration of H⁺?

Has a video solution.

The pH of a basic solution is 9.77. What is [OH⁻]?

Has a video solution.

What is the oh ion concentration of an aqueous solution with a pH of 5?

Has a video solution.

The OH^- concentration in an aqueous solution at 25 °C is 6.1 × 10^-5. what is [H⁺]?

Has a video solution.

Bleach has a pH of around 12. What is it considered on the pH scale?

Has a video solution.

A solution of HCl has = 0.01 M. What is the pH of this solution? use. –2 –1 1 2

Has a video solution.

What is the ph of an aqueous solution with the hydronium ion concentration

Has a video solution.

Match each H⁺ concentration to its corresponding OH^– concentration in aqueous solution.

Has a video solution.

Showing 45 of 45 practice