Answered: At what pH is the concentration of a…

At what pH is the concentration of a compound, with a pKa = 8.4, 100 times greater in its basic form than in its acidic form?

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

Chapter16: Reactions Between Acids And Bases

Section: Chapter Questions

Problem 16.83QE

See similar textbooks

Related questions

Q: Ammonium (NH+6) is a weak acid in water as described in the reaction below: NH+4↔NH3+H+; pKa= 9.3…

A: We first need to calculate the concentration of H+ introduced in the solution by adding ammonium…

Q: Give the definitions of pH and pKa. What are the differences between these two terms? Calculate the…

A: pH-: The negative logarithm of hydrogen ion concentration in moles per liter in an aqueous solution…

Q: You have a 200 mM solution of polyionic acid (pKa 4.2 and 11.6) at pH 5. What are the concentrations…

Q: Write the expresson for the dissociation constant, Ka for an aqueous solution of butanoic acid.…

Q: If I’ve got 20.0 grams of tartaric acid with a (first ionization) pKa = 2.91. If I dissolve this…

A: The formula of tartaric acid is C4H6O6. Molar mass of C4H6O6 = Atomic mass of C X 4 + Atomic mass of…

Q: The concentration of the active ingredient in soap is a fatty acid salt NaA. A'=CH3(CH2),CO'. What…

A: The question is based on the concept of salt hydrolysis. we have to determine the pH of the given…

Q: What will be the pH of a buffer solution containing an acid with a pKa of 2.2 with an acid…

Q: -Methylvaleric acid, CH3(CH2)2CH(CH3)COOH has a pKa=4.9. What is the pH of its conjugate base which…

A: This molecule is a weak acid it's conjugate is strong base A solution in which weak acid or strong…

Q: 1. The following equilibrium exists when ammonium is dissolved in water: NH4+ (aq) + H2O (l) « H3O+…

Q: An acid is found to have a pKa = –1.15 at 25 °C. What is the Ka (to two decimal places) of the acid?

Q: Benozic acid (C6H5COOH) has a pKa of 4.20. What is the ratio of the acid to its conjugate acid at a…

Q: Determine the pKa of an acid; a 4e-3M solution of which has a pH of 2.4

Q: You create a solution that is 0.20 M formic acid and 0.25 M sodium formate and the equilibrium shown…

A: For the given reaction, HCOOH + H2O ⇌ HCOO– + H3O+ [Formic acid] = 0.20 M [Sodium formate] = 0.25 M…

Q: An analytical chemist is titrating 159.0 mL of a 0.05700M solution of diethylamine ((C₂H₂)₂NH) with…

A: Given - Volume of solution =159.0 mL Concentration of diethylamine =0.0570 0 M Concentration of…

Q: An analytical chemist is titrating 165.1 mL of a 0.8800M solution of diethylamine (C,Hs) NH) with a…

Q: 11.An acid-base equilibrium system is created by dissolving 0.20mol CH3COOH in water and diluting…

Q: An organic acid has pK = 3.74. What is its K, value?

A: Ka is acid dissociation constant and it is related to pKa as negative logarithm of it which may be…

Q: Which of the following is true of a buffer solution that contains equivalent amounts of acid and…

A: buffer solution that contains equivalent amounts of acid and conjugate base means [Conjugate base ]…

Q: Calculate the pH of an acetic acid solution, originally 0.25 M, in water. The pKa for acetic acid =…

A: Acetic acid is weak acid it dissociated feabily in aqueous solution

Q: Blood has a normal pH of about 7.40. Lactic acid has a pKa of 3.08. Is lactic acid…

A: pH of blood = 7.40 pKa of lactic acid = 3.08

Q: HA is a weak acid with pKa = 6.70. What is the pH of a 1.59 M solution of HA?

A: pKa=6.70[HA]=1.59MWe have to calculate the pH of the solution.

Q: A dilute (-0.10 M) butanoic acid solution (aka butyric acid) has a pH of 4.6. To the nearest…

A: pH = 4.6pKa = 4.82

Q: Calculate the pH of a 0.24 M solution of sodium lactate. The pKa of lactic acid is 3.86. Round to…

Q: Calculate pH of water solution of Hydrosulphuric acid with concentration of 0,050 M (pKa=6.99)

Q: An analytical chemist is titrating 126.8 mL of a 0.2600M solution of diethylamine ((C₂H₂)₂NH) with a…

A: Given : Concentration of diethylamine = 0.2600 M Volume of diethylamine = 126.8 ml Concentration…

Q: 4. Explain using equilibrium principles, how the Carbonic Acid/Bicarbonate system regulates…

A: Carbonic acid and bicarbonate ion buffer regulates the PH of the medium. The PH change can…

Q: Find the pH of the following solutions: 0.03M trichloroacetic acid, Cl3CCO2H, pKa = 0.638

A: The objective of this question is to calculate the pH of a 0.03M solution of trichloroacetic acid…

Q: 5) Find the concentration of H3O*(aq) in a 1.75 M solution of lactic acid, HC3H5O3, at 25°C. Ka=…

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: An analytical chemist is titrating 173.3 mL of a 0.1600M solution of diethylamine ((C₂H)2NH) with a…

A: The objective of this question is to calculate the pH of the base solution after a certain volume of…

Q: What is the pH, along with the concentration of each form of serine, in a 0.020 M solution of…

A: pH needs to be determined in a 0.020 M solution of serine.

Q: An analytical chemist is titrating 75.2 mL of a 0.5800 M solution of trimethylamine ((CH3)N) with a…

Q: A weak acid, HA, has a pKa of 4.268. If a solution of this acid has a pH of 4.853, what percentage…

Q: Calculate the pH of the solution after the addition of each of the given amounts of 0.0651 M HNO3 to…

Q: ome flowering plants will change color based on the pH of the soil. For example, hydrangeas will…

A: A question based on pH concept, which is to be accomplished.

Question

At what pH is the concentration of a compound, with a pK_a = 8.4, 100 times greater in its basic form than in its acidic form?

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

The pH has to be identified

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 3 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

What are the equilibrium concentrations of acetic acid, the acetate ion, and H3O+ for a 0.10 M solution of acetic acid (K2 = 1.8 105)? What is the pH of the solution?
Write the chemical equation and the expression for the equilibrium constant, and calculate Kb for the reaction of each of the following ions as a base. (a) sulfate ion (b) citrate ion
If the concentration of an acid in solution is 2.3 times larger than the concentration of its conjugate base, and the pH of the solution is 4.9, what is the pKa of the acid?
Consider the acid HXOy where X is a halogen that is less electronegative than oxygen. Which of the following gives the relationship between Ka of the acid and the value of y and gives the correct reasoning? As y increases the value of Ka increases because the conjugate base of the acid becomes less stable. As y increases the value of Ka increases because the conjugate base of the acid becomes more stable. As y increases the value of Ka decreases because the conjugate base of the acid becomes less stable. As y increases the value of Ka decreases because the conjugate base of the acid becomes more stable.
Calculate the pH of an acetic acid solution, originally 0.25 M, in water. The pKa for acetic acid = 4.76.
What effect does a decrease in pH have on the following equilibrium? CaCO3(s) + 2H+1(aq) ⟷ Ca+2(aq) + H2O(l) + CO2(g)
For an acid HA with a pKa of 5.2, what is the ratio of the concentration of the conjugate base to that of the acid at pH 7.2.
What is the pH of a solution containing 0.50 moles of benzoic acid and 0.75 moles of sodium benzoate if the pka is 4.19?
Consider two acids: HCO2H (formic acid, pKa = 3.8) and pivalic acid [(CH3)3CCO,H, pK = 5.0]. (a) Which acid has the larger K? (b) Which acid is the stronger acid? (c) Which acid forms the stronger conjugate base? (d) When each acid is dissolved in water, for which acid does the equilibrium lie further to the right? %3D The pKa values in Table 2.1 span a large range (-7 to 50). The pK, scale is logarithmic. small difference in pK, translates into a large numerical difference, For example, the diffe between the pK, of NH3 (38) and CH2=CH, (44) is six pKa units. This means that NH, is one million times more acidic than CH,=CH,.
The pH of an aqueous solution of weak monoprotic acid is 3.15. What is the initial concentration of the acid if the pKa of the acid 5.74?
A dilute (~0.10 M) butanoic acid solution (aka butyric acid) has a pH of 4.6. To the nearest hundredth of a unit, what is the ratio of the acidic form to basic form of the molecules at this pH? (The pKa of butanoic acid is 4.82.)
Predict the position of equilibrium and calculate the equilibrium constant, Keq, for acid-base reaction