For a given acid HA, it was determined that at pH 6.0 the concentration of the conjugate base [A]was 0.075 M and the acid [HA] was 0.025 M.What percent of this acid is ionized at pH 6.0?What is the pKa of this acid?What pH would this acid be 50% lonized? Under anerobic conditions, when our bodies lack enough oxygen to complete respiration, theproduct of the glycolytic pathway, pyruvate, is reduced to lactate in an effort to allow for energyproduction to continue. Lactate is the conjugate base of lactic acid, thus high lactate levels can leadto a drop in pH in our muscle cells.0OHOH0CсH, - сCCH, + HHOH0Hhydrogenionlactic acidlactateThe ionization of lactic acid to lactate has a K₂ of 1.585 x 10-4.A solution containing a mixture of lactic acid and lactate was found to have a pH of 3.80.What percent of that solution is lactate?с

Percent ionization of HA = [H+]/[HA] *100% pH =6.0 pH = -log[H+] 6.0 =-log[H+] [H+] = inv log…

For a given acid HA, it was determined that at pH 6.0 the concentration of the conjugate base [A] was 0.075 M and the acid [HA] was 0.025 M. What percent of this acid is ionized at pH 6.0? What is the pKa of this acid? What pH would this acid be 50% ionized?

For a given acid HA, it was determined that at pH 6.0 the concentration of the conjugate base [A] was 0.075 M and the acid [HA] was 0.025 M. What percent of this acid is ionized at pH 6.0? What is the pKa of this acid? What pH would this acid be 50% ionized?

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: A monoprotic weak acid (HA) has a pKa value of 3.841. Calculate the fraction of HA in each of its…

A: Given for a weak acid pKa = 3.841 pH = 5.275

Q: The pka of the methylammonium ion is 10.62. At what pH is methylammonia 1/5 ionized

A: To find the pH at which methylammonia (CH3NH2) is 1/5 ionized, you can use the Henderson-Hasselbalch…

Q: + 2) HA is a weak acid. HA is dissociated to H and A in water. At equilibria, if the pH of the…

A: We know , PH = -log[H+] and log1 = 0

Q: The Ka for an acid is 4.45 x 10-10. Calculate the pKa for this acid.

A: Ka = 4.45 x 10-10

Q: What is the pKa of Sylvianic Acid if it is 2.3% dissociated at pH = 10.26?

Q: What is the pH of a 0.10 M solution of an acid with a pKA of 8.4?

Q: Which statement correctly describes Ka, pKa and the strength of a weak organic acid? The larger the…

A: The acid dissociation constant (Ka) is a quantitative measure of the strength of an acid in…

Q: Use pka values to predict which of the following equilibria will favor the reactants.

Q: If the Ka for an acid is 0.010, what is the pK for its conjugate base? Give your answer to 2 decimal…

A: The objective of this question is to calculate the pK of the conjugate base of an acid given the Ka…

Q: An analytical chemist is titrating 147.6 mL of a 0.4800M solution of ethylamine (C₂H-NH₂) with a…

Q: Cacodylic acid is used as a cotton defoliant. Cacodylic acid is 0.77% deprotonated in a 0.011 M…

A: Degree of dissociation of Cacodylic acid is = 0.77% Concentration = 0.011M PH =?Ka =?

Q: The Ka of an acid is determined to be 0.00589. What is the pKa?

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: A 0.1 M solution of acid HA has a pH of 3.2. W

A: C concnetration having weak acid HA dissociate into HA…

Q: If the Ka of the conjugate acid is 5.06 × 10-5 , what is the pKb for the base?

A: First find out the Kb value using Ka value. Using that Kb value, find out the pKb.

Q: When ammonium (NH4*) is placed in water, a chemical reaction occurs and an equilibrium is…

A: Given :

Q: 1. What is the pH of a 0.2 M acetic acid solution where the Ka for acetic acid is 1.33 x 10-5 M. 2.…

A: Concentration of acetic acid solution = 0.2 MKa for acetic acid = 1.33 × 10-5pH of the solution = ?

Q: For each value of Ka, calculate the corresponding value of pKa. Which compound is the stronger acid?…

A: pKa of any acid can be calculated as: pKa=-logKa Ka is dissociation constant of an acid. Larger the…

Q: Calculate the pH of a 1.8M solution of trimethylacetic acid.

A: Ka(acid dissociation constant) is the ratio of product of concentration of products raised to their…

Q: What is the K₂ of an acid whose pka is 9.01?

Q: Write down the reaction of ethanoic acid with water and identify the conjugate base.

Q: Chloroacetic acid, ClCH₂COOH, has a pKₐ of 2.87. What are [H₃O⁺], pH, [ClCH₂COO⁻], and [ClCH₂COOH]…

A: Given : pKa of ClCH2COOH = 2.87 And initial concentration of ClCH2COOH = 1.25 M Since ClCH2COOH is…

Q: The pKas of the conjugate acids of -OH (conjugate acid H2O) and HPO42- (conjugate acid H2PO4-) are…

Q: What is the K a of an acid whose pK a is 8.60?

Q: Methylamine Ethylamine H3NH₂ C₂H5NH₂ H₂NH3 C₂H5NH3+ 4.38 X 10 5.6 x 10-4 Aniline CH;NH, C6H5NH3 +…

Q: The following compound is derived from one of the twenty mammaliam "amino acids". It is the ethyl…

A: Highly basic Nitrogen protonated. Guanidine moiety is highly basic than secondary amine so…

Q: Assuming the same concentration of solution and all solutions at the same temperature, when…

A: The pH of a solution is the negative logarithm of hydrogen ion concentration. The pKb is the…

Q: , NH +? What is the pK of NH +?

A: Acid forms conjugate base by donating proton (H+) while base forms conjugate acid by accepting…

Q: At what pH will the concentration of a compound with a pK, 8,4 be 100 times greater in ita acidic…

A: Reaction involved :- HA + OH-1 = A- + H2O HA = acidic form A- = basic form

Q: An analytical chemist is titrating 70.1 mL of a 0.5200 M solution of piperidine (C-H₁0NH) with a…

A: For weak acid-base titration, the equilibrium pH depends on the excess concentration of the species…

Q: Consider the following reaction: X-SH ⇌ X-S- + H+ The pKa for the sulfhydryl (thiol) group…

A: The reaction of X-SH is given as, => X-SH ⇌ X-S- + H+

Q: An analytical chemist is titrating 92.3 mL of a 0.6600M solution of ethylamine (C₂H5NH₂) with a…

Q: A newly found weak acid is found to have a pH of 4.13 when an aqueous solution of 0.326 M is…

A: Calculate the concentration of hydrogen ions released in the solution.

Q: Isobutylamine is a weak base. If the initial concentration of isobutylamine is 0.055 M and teh…

Q: I don't understand the pKa equation. What is the "p"? What does negative logarithm mean?

Q: A 1.819 g sample of N-2-acetamido-2-aminoethane-sulfonic acid potassium salt (ACES¯K+, MW = 220.29…

Q: How did you know the molecules were weak or strong acid? Please give the pKa if that's the method…

A: In this question, we have to explain How did you know the molecules were weak or strong acid.

Q: For a solution of formic acid, a weak acid with a pKa of 8.74, at what pH will the concentration of…

A: Using Henderson-Hasselbalch equation for buffer solution :- pH = pKa + log([conjugate base]/[weak…

Q: What is the pH of a solution that is 0.05M in ethylamine and 0.08M in its chloride salt (pKa=10.8)

A: pH of a solution =? [ C2H5NH2 ] = 0.05 M [ C2H5NH3+ ] = 0.08 M Acid dissociation constant :…

Q: What are the concentrations of imidazole hydrochloride and imidazole if the final solution…

A: The solution contains imidazole (weak base) and imidazole hydrochloride (its conjugate acid). So,…

Q: Calculate the percentage of ionize and unionized forms present in the following solution. Assume…

A: Weak acids partially dissociates so there is degree of dissociation alpha.

Q: what would be product of the acid base reaction below H— F + H—Ö— -H

A: Since you have posted multiple question, we will provide solution to the first question.Please…

Q: the Kb of a weak base is 4.7E-9, what is the Ka of its conjugate acid? Do not include any units with…

Q: Calculate the pH of the solution after the addition of each of the given amounts of 0.0603 M HNO3…

Q: Common aspirin is acetylsalicylic acid, which has the structure shown below and a pKa of 3.5.…

A: The question is based on the concept of pH of the solution. It is defined as a negative logarithm…

Question

For a given acid HA, it was determined that at pH 6.0 the concentration of the conjugate base [A]
was 0.075 M and the acid [HA] was 0.025 M.
What percent of this acid is ionized at pH 6.0?
What is the pKa of this acid?
What pH would this acid be 50% lonized?

Under anerobic conditions, when our bodies lack enough oxygen to complete respiration, the
product of the glycolytic pathway, pyruvate, is reduced to lactate in an effort to allow for energy
production to continue. Lactate is the conjugate base of lactic acid, thus high lactate levels can lead
to a drop in pH in our muscle cells.
0
OH
OH
0
C
сH, - с
C
CH, + H
HO
H
0
H
hydrogen
ion
lactic acid
lactate
The ionization of lactic acid to lactate has a K₂ of 1.585 x 10-4.
A solution containing a mixture of lactic acid and lactate was found to have a pH of 3.80.
What percent of that solution is lactate?
с

Expert Solution

This question has been solved!

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

SEE SOLUTION Check out a sample Q&A here

Step 1 Calculate percent ionization of acid at pH 6

VIEW

Step 2 Calculate the pKa of the acid

VIEW

Step 3 Calculate the pH at 50% ionized

VIEW

Step by step

Solved in 3 steps

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

Consider a 0.14 M solution of thriethylamine with a pH of 4.8. Calculate the percentage ionisation of the acid in this solution.
I need help with this problem. Compare the pH of propionic acid and nitric acid when they are dissolved in water at a concentration of 20 mM using the "Arrhenius Concept". Include:a balanced equation describing the acid-base reactions involvedThe calculation of the pKa for bothThe calculation of the two pH's (of propionic acid and nitric acid when they are dissolved in water at a concentration of 20 mM)and A calculation of the percent of dissociation of both propionic acid and nitric acid.The gibbs free energy ΔG are listed as the following:Nitric acid: -152 kJ/molPropionic Acid : -291 kJ/molPropionate: -361 kJ/mol
3. Draw the two structures in most abundance of the amino acid, cysteine, at a pH of 8.0. What are their respective concentrations in a 50 mM solution? If you had 1.0 L of this solution, how much 3.0 M NaOH would be required to take the pH to 10.4? What two species are now in most abundance (draw the structures)?
Benozic acid (C6H5COOH) has a pKa of 4.20. a. What is the ratio of the acid to its conjugate base at a pH of 2.20?
If the concentration of an acid in solution is 2.2 times larger than the concentration of its conjugate base, and the pH of the solution is 3.5, what is the pKa of the acid? Include the answer to 3 significant figures
What is the pKa of Sylvianic Acid if it is 2.3% dissociated at pH = 10.26?
A weak acid, HA, has a pka = 6.78. If one dissolved 0.898 moles of a salt containing one mole equivalent of the conjugate base of the weak acid (e.g. NaA where A is the conjugate base of the weak acid) into 1 Liter of water, then what would be the resulting pH?
If the pKa of a weak acid HA is 3.84, what is the pkb of its conjugate base A-
Explain why a pKa is not found for the strong acid, but one will be found for the weak acid.
For an acid with a pKa of 5.00, what is the pKb of its conjugate base?
Write the acid dissociation constant expression (Ka ) for the dissociation of HCN.
Using the table of the weak base below, you have chosen Pyridine as your weak base in the buffer solution. You have already added enough of the conjugate acid salt to make the buffer solution concentration at 0.62 M in this salt. The desired pH of the buffer should be equal to 4.5. Values of K, for Some Common Weak Bases Conjugate Acid Name Formula Kb Ammonia NH3 NH4+ 1.8 x 10-5 Methylamine CH;NH, CH3NH3+ 4.38 x 10-4 5.6 x 10-4 Ethylamine C₂H5NH₂ C₂H5NH3+ Aniline CcHsNH₂ CH5NH3+ 3.8 x 10-10 Pyridine C,H,N CH,NH* 1.7 x 10-⁹ 1. Compute the poH of the buffer solution.