For the diprotic weak acid H2A, Kal = 2.1 x 106 and K2 = 8.0 x 10-9.%3D%3DWhat is the pH of a 0.0500 M solution of H,A?pH =What are the equilibrium concentrations of H, A and A2-in this solution?careesPvacy policyterms of use contact us heipabout us* 风立 What are the equilibrium concentrations of H, A and A- in this solution?[H,A] =%3DM[A?-1 =Mtems of use contact ushelpcareersprivacy policy10:37 P3/10/20t9

Answered: Image /qna-images/answer/229fe74f-3811-4e1a-82f6-2084f6bace74.jpg

Answered: For the diprotic weak acid H2A, Kal =…

For the diprotic weak acid H2A, Kal = 2.1 x 106 and K2 = 8.0 x 10-9. %3D %3D What is the pH of a 0.0500 M solution of H,A? pH = What are the equilibrium concentrations of H, A and A in this solution?

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 diprotic acid, H, A, has acid dissociation constants of K 2.32 x 10 and K2 = 5.84 x 10-12.…

A: Hii there, As there are multiple question posted. we are answering first question. If you need…

Q: For the diprotic weak acid H₂A, K₁1 = 2.1 x 106 and K₁2 = 7.6 x 10-⁹. What is the pH of a 0.0400 M…

A: pH is a measure of how acidic/basic water is. The range goes from 0 - 14, with 7 being neutral. pH…

Q: The concentration of the hydronium ion in an aqueous solution at 25 °C is 0.0090 M. What is the…

Q: 2. Calculate pH and pOH for each of the following solutions and determine whether the solution is…

Q: Determine the voltage of a galvanic cell composed of Pb(s) in a 1.00 M solution of Pb²+, and Ni(s)…

Q: For the diprotic weak acid H₂A, Kal What is the pH of a 0.0750 M solution of H₂ A? pH = = = 3.7 ×…

A: Given, The concentration of H2A = 0.0750 M. Ka1 = 3.7 × 10-6 and Ka2 = 5.4 × 10-9 The pH of the…

Q: For the diprotic weak acid H2A, Kal = 3.7 x 10-6 and Ka2 = 6.9 x 10-9. What is the pH of a 0.0550 M…

Q: roic acid, HC6H11O2, is found in coconut oil and is used in making artificial flavors. A solution is…

A: Acid is commonly sour. An acid is a substance that renders an ionizable hydronium ion (H3O+) in its…

Q: What is the concentration (in molarity) of H+, HCO3−, and CO32–, in a solution that is initially…

A: Given the initial concentrations of H2CO3 = 0.0100 M initial concentrations of Na2CO3 = 0.000010 M…

Q: Write the dissociation equation and calculate the pH for a solution of 2.5 M HNO2 nitrous acid, Ka…

Q: H₂SO3 is a diprotic acid with Kal = 1.6 × 10°² and K₁2 = 6.4 × 10-8 What is the equilibrium constant…

A: When we subtract two equations; value of equilibrium constant gets divided.Equilibrium constant is…

Q: Sulfurous acid (H₂SO3) is a diprotic acid with Kal = 1.39 x 10-2 and K₁2 = 6.73 x 10-8. Determine…

Q: For the diprotic weak acid H₂A, K₁1 = 2.3 x 10-6 and K₁2 = 6.5 x 10-⁹. What is the pH of a 0.0550 M…

A: Given that for diprotic weak acid, Ka1 = 2.3 × 10-6 Ka2 = 6.5 × 10-9 Initial concentration of H2A…

Q: 2- Suppose a 0.046M aqueous solution of phosphoric acid (H3PO4) is prepared. Calculate the…

A: Given,Molarity of H3PO4 = 0.046 MpKa1 ( H3PO4 ) = 2.16pKa2 ( H3PO4 ) = 7.21

Q: Formic acid, HCOOH, ionizes in water according to the following equation. The equilibrium constant…

A: :- This question is answered by using the simple concept of ionisation of weak acid and then using…

Q: For the diprotic weak acid H2A, Kal = 3.7 × 10-6 and K2 = 6.9 × 10-9. What is the pH of a 0.0550 M…

Q: Phosphoric acid, H3PO4(aq), is a triprotic acid, meaning that one molecule of the acid has three…

Q: For the diprotic weak acid H₂A, Kal = 3.7 x 10-6 and Ka2 = 6.1 x 10-⁹. What is the pH of a 0.0800 M…

Q: We place 0.586 mol of a weak acid, HA, and 12.6 g of NaOH in enough water to produce 1.00 L of…

A: Step 1: Step 2: Step 3: Step 4:

Q: For the diprotic weak acid H₂A, K₁1 = 3.8 x 10-6 and K₁₂ = 7.7 x 10-⁹. What is the pH of a 0.0750 M…

A: Given, The concentration of H2A = 0.0750 M. Ka1 = 3.8 × 10-6 and Ka2 = 7.7 × 10-9 The pH of the…

Q: For the diprotic weak acid H,A, Kal = 3.2 x 10 and Ka2 = 6.3 x 10-9 What is the pH of a 0.0800 M…

A: For H2AKa1 = Ka2 = Concentration of H2A = 0.0800 MWe have to determine the pH of the solution and…

Q: For the diprotic weak acid H2A, Kal = 3.5 × 10-6 and K22 = 7.7 × 10-9. What is the pH of a 0.0400 M…

A: The pH is used to determine the alkalinity or acidity of a solution. the pH is determined as the…

Q: the diprotic weak acid H₂A, K₁1 = 3.3 x 10 and K₁2 = 7.7 x 10⁹. hat is the pH of a 0.0600 M solution…

Q: . Calculate the pH and all the equilibrium concentrations for the complete dissociation of a 2.0 M…

Q: What is the Ka of a weak acid (HA) if the initial concentration of weak acid is 4.5 x 10-4 M and the…

A: The objective of this question is to calculate the Ka (acid dissociation constant) of a weak acid…

Q: For the diprotic weak acid H₂A, K₂ = 2.1 x 106 and K = 7.2 x 10%. What is the pH of a 0.0600 M…

A: Given: Ka1 = 2.1×10-6 Ka2 = 7.2×10-9 Concentration of H2A = 0.06 M

Q: For the diprotic weak acid H2A, Kaj = 3.1 x 10-6 and Ka2 = 8.9 x 10-9. What is the pH of a 0.0550 M…

Q: Phosphoric acid, H, PO,(aq), is a triprotic acid, meaning that pKal pKa2 pKa3 one molecule of the…

Q: What is the pH of a 0.177 M diprotic acid solution (H2A)? Ka1 = 4.3 x 10-5 and Ka2 = 2.8 x 10-9.

A: The general equation for the dissociation of a diprotic acid (H2A) can be represented as follows:…

Q: For the diprotic weak acid H2A, Kal = 3.1 x 10-6 and Ka2 = 7.2 x 10-9. What is the pH of a 0.0650 M…

Q: Calculate the pH of a 0.299 M NH, solution. NH, has a Kp = 1.8 × 10-5. pH =

A: pH =11.366

Q: Percent ionization for a weak acid (HA) is determined by the following formula: [HA] ionized [HA]…

A: we have to calculate the percent ionization

Q: I'm not sure how to answer this question. I know that the first two answers are correct, but I don't…

A: The hydronium ion concentration can be calculated using ICE table as,

Q: Given a diprotic acid, H₂A, with two ionization constants of Kal = 4.0 x 104 and K₁2 = 4.7 x 10-¹1,…

A: 1. Given that, a diprotic acid H2A. The two ionization constants of H2A are Ka1 = 4.0×10-4, Ka2 =…

Q: 10. Calculate the pH of a 0.250 M solution The Ka of HCIO is 2.9x10-8.

Q: For the diprotic weak acid H2A, Kal = 3.0 x 10-6 and K2 6.0 x 10-9. %3D What is the pH of a 0.0400 M…

Q: Determine the pH of the molecules given in a 1L beaker containing 0.035M solution of the given…

A: 1 L beaker containing 0.035 M solution of - NaNO2 , C6H5CHCOOH and BaOH2We have to calculate the…

Q: An aqueous solution is composed of acetic acid and sodium hydroxide. The acetic acid is 0.155M and…

A: The condition given as mixture of weak acid and strong base ,in which base will react with weak acid…

Q: Caproic acid, HC6H11O2, is found in coconut oil and is used in making artificial flavors. A solution…

A: The pKa is the pH value at which a chemical species will accept or donate a proton. The lower the…

Q: For the diprotic weak acid H₂A, K₁= 3.4 x 10 and K = 5.2 x 10-⁹. What is the pH of a 0.0750 M…

Q: If the K of a weak base is 8.0 × 10-6, what is the pH of a 0.48 M solution of this base? pH

A: Weak base dissociated less in aqueous solutions

Q: 3+ Calculate the pH of a 0.064-M Al (NO3); solution. The K, value for Al (H20)," is 1.4 x 10.

A: Concentration of Al ion = 0.064 M

Q: Acetylsalicylic acid (aspirin), HC9H7O4, is the most widely used pain reliever and fever reducer.…

Q: Ascorbic acid (H,C,H,O,) is a diprotic acid. The acid dissocation constants for H,C,H,O, are Kal =…

Q: Below is the unbalance chemical equation of hydrochloric acid with barium hydroxide. Balance the…

A: The balanced equation has atoms on both sides equal that is on the reactant side and the product…

Q: For the diprotic weak acid H2A, Ka1 = 3.1 × 10-6 and K2 = 8.4 × 10-9. What is the pH of a 0.0500 M…

A: The concentration of diprotic weak acid H-A is 0.0500 M. The value of acid dissociation constant Ka1…

Q: Calculate the pH of a 0.383 M NH, solution. NH, has a Kp 1.8 x 10-5. pH

A: NH3 is a weak base and since Kb value is very less so it is assumed that reaction proceeds very less…

Q: For the diprotic weak acid H2A, Kal = 3.0 × 10-6 and Ka2 = 7.1 × 10-9. What is the pH of a 0.0700 M…

A: We will calculate pH and the equilibrium concentration of the solution.

Q: what is the ph of a 0.81 M hypochlorous acid (HClO) solution?

A: Given :- concentration of HClO = 0.81 M Ka = 3.0 × 10-8 To calculate :- pH of…

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

For the diprotic weak acid H2A, Kal = 2.1 x 106 and K2 = 8.0 x 10-9.
%3D
%3D
What is the pH of a 0.0500 M solution of H,A?
pH =
What are the equilibrium concentrations of H, A and A
2-
in this solution?
carees
Pvacy policy
terms of use contact us heip
about us
* 风
立

What are the equilibrium concentrations of H, A and A- in this solution?
[H,A] =
%3D
M
[A?-1 =
M
tems of use contact us
help
careers
privacy policy
10:37 P
3/10/20
t9

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

Find the pH

VIEW

Find the concentration of H2A & A2-

VIEW

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

Kc for formic acid dissociation in water is 1.8x10-4. What are the equilibrium concentrations of H30+ HCOO- and HCOOH if the initial concentration of HCOOH is .15 mol? HCOOH (aq) +H20 (L) >< H30 (aq) + HCOO (aq)
Consider two aqueous solutions of equal concentration: chlorous acid (HCNO, K, = 2.0 x 10 4) and acetic acid (CH3COOH, K, = 1.77 x 10-5). Which statement is true when the solutions are at equilibrium? %3! O CNO produces more [OH ] than CH3COO O HCNO produces less [H3O*] than CH3COOH O The pH value of HCNO solution is the same as that of CH3COOH solution. O HCNO produces more [H3O*] than CH;COOH O The pH value of HCNO solution is higher than that of CH3COOH solution.
For the diprotic weak acid H2A, Kal = 3.1 x 10-6 and Ka2 = 5.6 x 10-9. What is the pH of a 0.0650 M solution of H, A? pH What are the equilibrium concentrations of H,A and A²- in this solution? [H,A] = M [A?-] = M
For the diprotic weak acid H2A, Kal = 2.4 × 10-6 and Ka2 What is the pH of a 0.0700 M solution of H₂A? pH = 10.96 = 8.0 × 10-9. What are the equilibrium concentrations of H₂A and A²¯ in this solution? [H₂A] = [A²-] = M M
For the diprotic weak acid H₂A, K₁1 = 2.8 x 10-6 and K₁2 = 7.5 × 10-⁹. What is the pH of a 0.0800 M solution of H₂A? pH = What are the equilibrium concentrations of H₂A and A2 in this solution? [H₂A] = [A²] = M M
A solution is prepared at 25 °℃ that is initially 0.99M in acetic acid (HCH3CO₂), a weak acid with K (NaCH3CO₂). Calculate the pH of the solution. Round your answer to 2 decimal places. pH = 0 X Ś = 1.8 × 10 -5 I and 1.3 M in sodium acetate
Calculate the pH and concentration of species present in a polyprotic acid solution. For a 9.03x10 M solution of H,CO3, calculate both the pH and the CO," ion concentration. -2 H2CO3 + H20 H;0" + HC03 Kal = 4.2x10-7 HCO3 + H2O=H30* {co,?- Ka2 = 4.8x10 11 pH = [Co,?) =
Calculate the pH of a 3.5 M solution and the equilibrium concentrations of the species H3PO4, H2PO4- , HPO4-2, and PO4-3 (Ka1= 7.5 x 10-3, Ka2= 6.2 x 10-8, Ka3= 4.8 x 10-13)
Give pH of the solution (in clear handwritten paper)
For the diprotic weak acid H2A, Kal = 2.3 × 10-6 and K22 = 6.9 × 10-9. What is the pH of a 0.0600 M solution of H, A? pH What are the equilibrium concentrations of H, A and A2- in this solution? [H,A] = M [A?-] = М
For the diprotic weak acid H2A, Kal = 2.5 × 10-6 and K2 = 6.5 x 10-9. What is the pH of a 0.0400 M solution of H, A? pH = What are the equilibrium concentrations of H, A and A?- in this solution? [H, A] = [A?-] =
For the diprotic weak acid H₂A, Kal What is the pH of a 0.0650 M solution of H₂ A? pH = = [H₂A] : 2- What are the equilibrium concentrations of H₂A and A²- in this solution? = = 2.8 × 10-6 and K₁2 = 7.5 × 10−⁹. [A²-] = M M