Calculate the pH at 25 °C of a 0.33 M solution of potassium butanoate (KC,H,Co,). Note that butanoic acid (HC,H,CO,) is a weak acid with apK, of4.82.Round your answer to 1 decimal place.pH =

The pH of the solution is calculated as shown in equation (1) where C is the concentration of…

Answered: Calculate the pH at 25 °C of a 0.33 M…

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter15: Solutions Of Acids And Bases

Section: Chapter Questions

Problem 15.124QE

See similar textbooks

Similar questions

Calculate the pH at 25 of a 0.590 M aqueous solution of a weak base with a Kb value of 1.27 x 10-5.
The value for Kw at 0.0°C is 1.14 x 10^-15. Calculate the pH for a neutral solution at this temperature.
The ionization constant, Ka, for dichloroacetic acid, HC2HO2Cl2 , is 5.0 × 10‑2. What is the pH of a 0.15 molar solution of this acid?
Acidic water can be treated with basic substances to increase the pH, although such a procedure is usually only a temporary cure. Calculate the minimum mass of lime, CaO, needed to adjust the pH of a small lake 1V = 4 * 109 L2 from 5.0 to 6.5. Why might more lime be needed?
A2 The dissociation constant of hydrazoic acid (HN3) Ka = 2.50 x 10–5. Using the Debye-Hückel limiting law, calculate the pH and degree of dissociation for a 0.054 m solution of hydrazoic acid a 0.054 m solution of hydrazoic acid with 0.150 m NaCl
Calculate the pH of a solution that is prepared by diluting 0.140 moles of sodium benzoate to 1.00 litre in water. (The Ka of C6H5COOH is 6.3x10-5).
The pH of an aqueous solution of acetic acid (CH3COOH) is 2.0. What is the initial molar concentration of CH3COOH, if its acid ionization constant is Ka = 1.8×10–5?
Find the pH of a 0.20 M aqueous solution of benzoic acid, for which Ka = 6.33 x 10-5
Look up the appropriate Ka1 and Ka2 values for oxalic acid andascorbic acid, and repeat these calculations for these two weak, diprotic acids. Calculate the pH of both solutions and rank the acidities of the carbonic acid, oxalic acid, and ascorbic acidsolutions. In what ways is the ranking consistent with the magnitudes of the ionization constants?
Calculate the pH of a weak base which dissociates as BOH ⇌ B+ + OH- ( like NH3 (g) + H2O(l) → NH4OH(aq) , where in water NH4OH ⇌ NH4+ + OH- ) knowing that the initial concentration of the base is 1.04 M, and the base dissociation constant, Kb , is 3.79e-10. pH ← please insert your value
Calculate the pH that results when 2.35 mL of a 0.0125 M aqueous solution of KOH is added to 23.50 mL of an 0.0132 M aqueous solution of methylamine (CH3NH2, Kb = 4.2 x 10–4). Show your work and justify any approximations made.
Bacteria in the human mouth release enzymes to break up sucrose, and thenpolymerize glucose to form a bacterial plaque. When this glucose is digested, it formslactic acid, which causes tooth decay. Tooth enamel is made of calcium phosphate.Lactic acid has a Ka 1.38x10 -4 and ionizes into lactate and H3O+ ions. Assuming aninitial lactic acid concentration of 0.10 mol/L on your tooth, determine the pH(assume a 1:1:1 mole ratio) and the percent ionization. Should people be concernedwith plaque buildup? Justify your answer.

SEE MORE QUESTIONS

Recommended textbooks for you

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Chemistry: Principles and Practice

Chemistry

ISBN:

9780534420123

Author:

Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:

Cengage Learning

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

SEE MORE TEXTBOOKS

Calculate the pH at 25 °C of a 0.33 M solution of potassium butanoate (KC,H,Co,). Note that butanoic acid (HC,H,CO,) is a weak acid with apK, of 4.82. Round your answer to 1 decimal place. pH =