Answered: A weak base has a Kb of 4.29E-10.…

Science

Chemistry

A weak base has a Kb of 4.29E-10. Calculate the pH of a 0.250M solution of the weak base.

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter15: Acid–base Equilibria

Section: Chapter Questions

Problem 35P

See similar textbooks

Related questions

Q: Succinic acid (H2C4H6O4), which we will denote H2Suc,is a biologically relevant diprotic acid with…

A: Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Calculate the pH of a solution that is 0.0729 M LiC2H3O2 at 25°C.

A: LiC2H3O2 ( Lithium acetate) is the salt of a weak acid and strong base. LiC2H3O2 → CH3COO- +…

Q: Calculate pH of the following solutions: a) 0.25 M HNO3 in 0.065 M CH3COOH (K,=1.75x10). b) 0.33 M…

Q: A 0.513 M solution of a weak base has a pH of 11.4. What is the Kb of the base?

A: Weak base concentration is given and pH is also given we have to find the Kb.

Q: The pH of 0.259 M solution of an unknown acid is measured to be 2.353. What is the Ka of the acid?

Q: The pH of a 0.0068 M solution of Ca(OH)₂ is?

A: pH + pOH = 14 pOH = -log[OH-]

Q: The pH of a 0.0068 M solution of Ca(OH)₂ is

A: pOH = - log[OH-] pH + pOH = 14

Q: The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31. What is the Ka of the acid?

A: Given pH = 2.31 Concentration of acid = 1.86 M Ka =?

Q: Determine the pH of a solution that is 0.15 M CH3COOH and 0.30 M CH3COONa.

A: GivenThe concentration of Acetic acid = 0.15MThe concentration of sodium acetate = 0.30M

Q: the Ph of a 0.050 M weak acid solution is 5.25. Calculate the Ka of the acid.

A: Given, pH of weak acid= 5.25 [weak acid ] =0.050 M Ka = ?

Q: What is the ph of a 0.214 M weak base solution? The Kb of the weak base is 0.000033.

A: Given :- Concentration of weak base = 0.214 M Kb = 0.000033 To calculate :- pH of solution

Q: A solution is 0.0500 M in NH4Cl and 0.0300 M in NH3. Calculate its OH- concentration and its pH.

Q: 1) A conjugate acid is defined as 2) In the general ionization reaction: HX(aq) + H,0(1) H,0* +…

Q: Determine the pH of a solution that is 0.20 M CH3COOH and 0.15 M CH3COONa.

A: Given :The solutions given are 0.20 M CH3COOH and 0.15 M CH3COONa.We need to pH of the solution.

Q: concentration

A: pOH = 14 - pH pOH = 14 - 10.41 pOH = 3.59

Q: A certain solution was found to have a pH of 5.50. Which of following statements is true about this…

Q: The pH of a solution of 0.63 M pyridine is 9.51, what is the Kb of pyridine? What is the Ka of its…

Q: The pH of 0.01 m Potassium hydrogen phthalate is

Q: The pH of a 0.70 mol/L weak base solution is 10.22. What is the Kb of the base?

Q: Butyric acid, C3H;COOH, has ionization constant of 1.54 x 10-5. a) Calculate the pH of 50.0 mL of a…

Q: Calculate the pH of a solution that is 0.0736 M KC2H3O2 at 25°C.

Q: The compound ethylamine is a weak base like ammonia. A solution contains 0.111 M C,H5NH3* and 0.406…

Q: The pH of 0.0720M solution of a weak acid is 2.670. What is the Ka of the acid

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: Benzoic acid, C6H5COOH, is a weak acid (Ka = 6.28*10-5). If I dissolve 1.22 g of C6H5COOH in enough…

A: Molarity of benzoic acid (M)= No of moles / Volume in Liter No of moles = Mass / molar mass = 1.22 /…

Q: Sodium hypochlorite solution is also known as bleach. It contains the hypochlorite ion ClO-. (a)…

Q: Determine the pH of a solution

A: Given :- Concentration of CH3COOH = 0.50 M Concentration of CH3COONa = 0.30 M To calculate :- pH…

Q: The pH of a 0.0062 M solution of Ca(OH)₂ is

Q: Calculate the pH of a 0.080 M solution of the weak base pyridine C5H5N: Kb= 1.7 x 10-9

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: The pH of a solution of 0.50 M NH4Cl is

A: NH4Cl dissociates as follows: Ka of NH3 is 5.6×10-10 Thus concentration of HCl is 1.67×10-5 M.

Q: The pH of a 0.0063 M solution of Ca(OH)₂ is

Q: 7. Calculate [H3O+] and [OH-] for each solution of either a strong acid or a strong base. Calculate…

A: Since you have posted a question with multiple sub-parts ,we will solve the first three sub-parts…

Q: The ka of an unknown acid, HYO₂, is determined to be 5 x 10⁻² empirically. What is the pH of a 0.1…

A: The objective of this question is to calculate the pH of a 0.1 M solution of an unknown acid HYO2,…

Q: a) What is the pH of a solution prepared by adding 11.1 mL of 0.50 M NaOH solution to 200. mL of a…

A: The question is based on the concept of buffer solution. A buffer is a solution which resist any…

Q: The pH of a 0.10 M solution of a weak base is 9.67. What is the Kb of the base?

A: Assuming the weak base is monoprotic base Hence the dissociation of base will have below reaction…

Q: Chemistry Question

A: Heavy unstable nuclei undergo spontaneous radioactive decay process. The half life time of a…

Q: The pH of a 0.30M solution of a weak base is 10.66 . What is the Kb of the base?

Q: Determine the pH of the solution

A: According to question Ka = 1.82 x 10-⁵ Mass of acetic acid = 20.0 g Molar mass = 60.05g/mol No. Of…

Q: The pH of a weak base (B) is 9.99 when the concentration of the weak base is 0.18 M. What is the…

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

A weak base has a Kb of 4.29E-10. Calculate the pH of a 0.250M solution of the
weak base.
pH =
*** assume the temperature is 25°C.

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

12.62 Write the formula of the conjugate acid of each of the following bases, (a) OH-, (b) NHj, (c) CHjNHt, (d) HPO/-, (e) CO.,2’
What is the pH of a solution obtained by mixing 235 mL of NaOH with a pH of 11.57 and 316 mL of Sr(OH)2 with a pH of 12.09? Assume that volumes are additive.
Why have chemists not tabulated the fraction ionized for different acids? Such a table would make problems such as calculating the pH of an acid solution quite simple.
Calculate [OH-] and pH in a solution in which the hydrogen sulfite ion, HSO3-, is 0.429 M and the sulfite ion is (a) 0.0249 M (b) 0.247 M (c) 0.504 M (d) 0.811 M (e) 1.223 M
A student prepares 455 mL of a KOH solution, but neglects to write down the mass of KOH added. His TA suggests that he take the pH of the solution. The pH is 13.33. How many grams of KOH were added?
You are asked to calculate the H+ concentration in a solution of NaOH(aq). Because sodium hydroxide is a base, can we say there is no H+. since having H+ would imply that the solution is acidic?
You are asked to determine whether an unknown white solid is acidic or basic. You also need to say whether the acid or base is weak or strong. You are given the molar mass of the solid and told that it is soluble in water. Describe an experiment that you can perform to obtain the desired characteristics of the white solid.
Consider an aqueous solution of HF. The molar heat of formation for aqueous HF is -320.1 kJ/mol. (a) What is the pH of a 0.100 M solution of HF at 100C? (b) Compare with the pH of a 0.100 M solution of HF at 25C.
For solutions of the same concentration, as acid strength increases, indicate what happens to each of the following (increases, decreases, or doesnt change). a. [H+] b. pH c. [OH] d. pOH e. Ka
Consider two weak acids, HA (MM=138g/mol)and HB (MM=72.0g/mol). A solution consisting of 11.0 g of HA in 745 mL has the same pH as a solution made up of 5.00 g of HB in 525 mL. Which of the two acids is stronger? Justify your answer by an appropriate calculation.
The pH of a 0.15-M solution of HSO4- is 1.43. Determine Ka for HSO4- from these data.
Consider a 0.33 M solution of the diprotic acid H2X. H2X H+(aq)+ HX(aq)Ka1=3.3 10 4 HX H+(aq)+ X2(aq)Ka2=9.7 10 8 Calculate the pH of the solution and estimate [HX-] and [X2-].