I only need the last one solved, the concentration of A2-. I also know that the answers for the two above are correct, just included the first picture so you'd have the necessary Ka values. Also the answer is not 8.057X10^-8 in case you get that. What are the equilibrium concentrations of H,A and A²- in this solution?[H,A] =.049662M[A?-] = | .0500M%DIncorrect For the diprotic weak acid H2A, Ka1 = 2.3 × 10-6 and K2 = 7.9 × 10-9.What is the pH of a 0.0500 M solution of H, A?pH =3.47What are the equilibrium concentrations of H, A and A?- in this solution?[H,A] =.049662M

Answered: Image /qna-images/answer/7e00b620-c12d-49ba-9f29-0f0c83b024d6.jpg

For the diprotic weak acid H2A, Kal = 2.3 × 10-6 and K2 = 7.9 × 10-9. What is the pH of a 0.0500 M solution of H, A? pH = 3.47 What are the equilibrium concentrations of H,A and A²- in this solution? [H,A] = .049662

For the diprotic weak acid H2A, Kal = 2.3 × 10-6 and K2 = 7.9 × 10-9. What is the pH of a 0.0500 M solution of H, A? pH = 3.47 What are the equilibrium concentrations of H,A and A²- in this solution? [H,A] = .049662

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter15: Equilibria Of Other Reaction Classes

Section: Chapter Questions

Problem 91E: The equilibrium constant for the reaction Hg2+(aq)+2Cl(aq)HgCl2(aq) is 1.61013, Is HgCl2 a strong...

See similar textbooks

Related questions

Q: . Write the base dissociation reaction (equilibrium) for benzoate ion (C,H$CO2) in water; (remember,…

Q: 2) A 0.10 M solution of which of the following salts would be predicted to exhibit a pH of 7.46 at…

A: Henderson Hasselbalch equation The equation that is used to calculate the pH of a buffer system is…

Q: Knowing the approximate pKavalues above will help in answering this question. A) Which form…

A: Hi, this question can be solved without using pKa values.

Q: If we have a 25 mL solution of weak acid HA (Ka = 1,00 * 10-6) and at pH 4,00. How much water needs…

A: For case of dilution following formula is used M1V1 = M2V2 When m1 = Conc. of [H+] in previous…

Q: Calculate the pH of 0.02172968275M Formic Acid (Ka at 25C = 1.80x10-4). Show the complete solution

Q: The acid dissociation constant Ka of acetic acid HCH3CO2 is ×1.810−5. Calculate the pH of a 1.2M…

A: Acetic acid is weak acid and it dissociates partially into [CH3COO-] and [H3O+].

Q: CH3CH2CO2H , Ka = 1.3 x 105 CH3CH2CO2, Kb = 7.7 x 10-10 F, Kb = 1.4 x 10-11 HF , Ką = 7.2 x 10-4 For…

A: Conjugate acid formed when an acid donates a proton to a base Conjugate base is formed when a…

Q: For each of the following reactions, highlight or circle the substance on the left hand side which…

Q: 5,Calculate the [OH-]of the solution with pH=10.50 Group of answer choices 1.05 x 10-10 5.0 x…

A: According to guidelines i can answer only first question, please repost the other one.

Q: (4c-301-2.56) What is the HT concentration of a solution with a pH of 2.56? Write your answer to…

Q: What is the ionization constant at 25 ◦C for the weak acid (CH3)2NH3 +, the conjugate acid of the…

A: The expression for the ionic product of water is as follows, Kw =…

Q: The acid ionization constants for species that are listed below can be found by using data given in…

A: The Ka value will be more for strong acids. Ka for H3PO4 = Ka1 x Ka2 x Ka3 = (7.5 x 10–3)( 6.2 x…

Q: complete a net ionic equation for each proton-transfer reaction using curved arrows to show the flow…

A: Acid has capability of losing proton and Base is that which accepts protons. Conjugate acid is that…

Q: The ionization of the first proton from H2 SeO4 is complete (H2 SeO4 is a strong acid); the…

A: H2SeO4 dissociates as follows: Since ionization of first proton is complete, thus the concentration…

Q: Solve the following problem, taking turns in your group to explain how to do the next step: What is…

Q: (1) Write the net ionic equation for the reaction that occurs when equal volumes of 0.074 M aqueous…

Q: Write an equation in which H2PO3 acts as an acid. (Use the lowest possible coefficients. Be sure to…

A: According to Bronsted Lowry concept, an acid is a substance that donates proton in solution while…

Q: Calculate the concentration of hydroxide in the following solutions. a) Pure water (pH = 7.00) b)…

A: We know that; pH + pOH = 14 kb = concentration in product sideconcentration in reactant side…

Q: The acid dissociation constant Ka of hydrocyanic acid HCN is ×6.210−10. Calculate the pH of a 1.6M…

A: The acid dissociation constant, Ka, of hydrocyanic acid HCN is 6.2×10−10. The pH of a 1.6 M solution…

Q: Safari File Edit View History Bookmarks Window Help )) 48% Sun 10:59 AM…

A: The following compounds are to be classified as acid, base, salt or other: HCOOH, CH3CH3, NaOH,…

Q: The pH for 0.0715 M solution of CCl,CO2H is 1.40. Determine the value of Ka for CCl,CO2H. 1 2 Based…

A: pH of Solution = 1.40 [CCl3COO2H] = 0.0715 M Ka for CCl3COO2H =?

Q: Oxalic acid (H2C2O4) is a diprotic acid with Ka1=5.6×10-1 and Ka2=1.5×10-4. Oxalate ion (C2O42-)…

A: To derive the value of Kb1 and Kb2 for oxalic acid in terms of Ka1 and Ka2 and Kw.

Q: A 0.055 M solution of HX is 6.7% ionized. Calculate Ka of this acid.

Q: Which of the following ions are capable of acting like a base? Highlight the one(s) you select.…

A: The strength of a base is inversely related to the strength of its conjugated acid. The weaker the…

Q: What is the calculated pH of the initial 0.100M Acetic Acid solution? Ka = 1.8 x 10-5 . Give your…

A: The dissociation reaction of acetic acid is given below: CH3COOH(aq) + H2O(aq) ⇌ CH3COO-(aq) +…

Q: Construct the expression for Ka for the weak acid, CH;COOH. CH;COOH(aq) + H2O(1) = H;O*(aq) + CH;COO…

A: Chemical equilibrium is defined as the dynamic condition, reached by a reversible reaction when rate…

Q: Cation: Mg2+ Fe3 PН-раper: pH-рарer: pH-рарer: | pH-раper: |PH-раper: Fe2+ Deionised water 5 3 1 3 5…

A: pH of a substance is its measure of the H+ concentration in the solution . A solution with high pH…

Q: Acid Molarity pH HX 0.010 M 2.0 HY 0.10 M 3.0 HZ 1.0 M 3.0 Based on data in this table, place these…

A: Interpretation - To arrange acids in order from weakest (lowest Ka) to strongest (highest Ka)…

Q: At 60 °C, Kw for water is 1.0 × 10¹³. At 60 °C, a weak acid has a Ka of 1.3 x 10-4. What is the Kb…

A: Acid can be defined as a substance that give hydrogen ions in an aqueous solution.

Q: acid base K K₂b name formula name formula 10 nitrous acid HNO₂ 4.5 x 10 aniline |C HạNH, | 4.3 × 10…

A: Ka value of acetic acid = 1.8×10-5 Ka value of HNO2 = 4.5×10-4 Kb value of aniline = 4.3×10-10…

Q: A solution is prepared at 25 °C that is initially 0.44 M in methylamine (CH, NH,), a weak base with…

A: Methylamine is weak base and Methyl ammonium bromide is its salt.so the solution is buffer solution.…

Q: c) Arrange the bases shown below in terms increasing acid strength and assign Kb values that…

Q: An acid HA has a Ka of 1.00 x 10-7. Calculate the pH of a 0.100 M solution of its conjugate base.…

A: Given: Concentration of conjugate base of weak acid HA i.e. A- = 0.100 M And Ka of HA = 1.00 × 10-7…

Q: Calculate the pH of 0.0858 M NH3 MM NH3: 17.03 Kb = 1,8 x 10-5 Upload your answer and solutions…

A: The molarity of ammonia is = 0.0858 M The dissociation constant of ammonia is = 1.8×10-5 The pH of…

Q: What is the pH of 2.4E-2M barium cyanide?

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

Q: Show by computation which acid is the weakest based on its % ionization. The lesser its %…

Q: Predicting acid or base strength from the conjugate species 0.1 M aqueous solution НСООН HC,04…

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

Q: The question says "calculate the ph of the solution." It gives the following: 1.00x 10^-1 M…

A: The given solution mixture is a buffer solution of weak acid acetic acid (CH3COOH) and its salt of…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

Q: NaHSO3 is a salt, which ionized completely to give HSO3- ion. the following equations show that…

A: NaHSO3 dissociates as: NaHSO3→Na++HSO3- (A)

Q: Consider the following list when answering the questions that follow: C6H5CO2H , Ka = 6.3 x 10-5 %3D…

A: Fill in the blanks for the reaction of benzoic acid and a solution containing CN- ions.

Q: CH3NH2 is a weak base (Kb=5.0×10−4), so the salt CH3NH3NO3 acts as a weak acid. What is the pH of a…

Q: Provide your view on this? Strong bases have weak conjugate acids with high pKa values, usually…

A: Strong base are those which donate hydroxide ions easily in aqueous medium

Q: For each of the following reactions, highlight or circle the substance on the left hand side which…

Q: What is the [H3O+] of 0.10 M propanoic acid (CH3CH2COOH, can simplify to HPr) (Ka= 1.3x10−5)?…

A: pH of a solution measures acidity of the solution. pH + pOH = 14 Where, pH = -log [H3 O+ ] and pOH…

Q: What is the [OH-] present in a 3 M solution of NH3, if the Kb = 1.8×10-5? Clearly state and verify…

A: Kb, the equilibrium constant for base dissociation or also known as the proton association constant…

Q: Write the chemical equation for the reaction of carbonic acid (H, CO,) with water and identify the…

Q: Please show your work so I can understand any math, also I have attached a special period table in…

A: [H3O+ ] = 9.4×10−11 M Ionic product of water (Kw) =[OH-] x [H3O+ ] = 10-14 [OH-] = Kw/[H3O+ ] =…

Concept explainers

Analytical Tools

Analytical tools or analysis tools help one to get into a conclusion or results from the data collected. Analytical tools can be applied for simple data sets and also in the case of big data analytics.

Question

I only need the last one solved, the concentration of A2-. I also know that the answers for the two above are correct, just included the first picture so you'd have the necessary Ka values. Also the answer is not 8.057X10^-8 in case you get that.

What are the equilibrium concentrations of H,A and A²- in this solution?
[H,A] =
.049662
M
[A?-] = | .0500
M
%D
Incorrect

For the diprotic weak acid H2A, Ka1 = 2.3 × 10-6 and K2 = 7.9 × 10-9.
What is the pH of a 0.0500 M solution of H, A?
pH =
3.47
What are the equilibrium concentrations of H, A and A?- in this solution?
[H,A] =
.049662
M

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

Step 2

Step 3

Step 4

Step 5

Step by step

Solved in 5 steps with 5 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

The equilibrium constant for the reaction Hg2+(aq)+2Cl(aq)HgCl2(aq) is 1.61013, Is HgCl2 a strong electrolyte or a weak electrolyte? Mm are the concentrations of Hg2+ and Cl- in a 0.015-M solution of HgCl2?
8-49 A solution of NaOH base was titrated with 0.150 M HCI, and 22.0 mL of acid was needed to reach the end point of the titration. How many moles of the unknown base were in the solution?
Calenlate the ptl of I15 M tydrofluoric acíd (HP) it the K, =7.2x10*?
What are the concentrations of all the species (H*, HCO;", and CO3? ) in a 0.025 M H2CO3 solution? [H* ][HCO,] K, [H,CO,] = 4.2x10-7 H,CO, (aq) z H*(aq)+HCO;(aq) [H*][Co ] K, [HCO;] 4.8x 10-11 HCO; (aq) H*(aq)+ CO3-(aq) 2H,0 2 H,O*(aq)+OH¯(aq) K, = [H* ][OH¯] =1.00× 10-14 %3D 2.
In solutions 1-4 you are adding successively larger volumes of 0.00200 M SCN- to the Fe3+ solution and diluting to 10.00 mL. Calculate the final diluted molarity of SCN- in solution #1. 3 sig figs (Calculate the same thing for the solutions 2-4 and enter the results in table 3 as [SCN-] pre-equilibrium.)
Calculate the pH and concentrations of CH, NH, and CH, NH; in a 0.0363 M methylamine (CH, NH,) solution. The Kp of CH, NH, is 4.47 × 10 1. pH (CH, NH, %3! M [CH, NH;] !!
For the reaction of hydrazine (N2H4) in water, H,NNH, (ag) + H20(1) = H,NNH,+(aq) + OH¯(@ag) K, is 3.0 x 10-. Calculate the concentrations of all species and the pH of a 1.6-M solution of hydrazine in water. [H,NNH,] =| %3D [H,NNH, !3! JOH |= %3D [H*]=[ ]M pH= %3D
Al203 (s) = 2AI3+ (aq) + 302- (ag) If, at equilibrium, a beaker contains 1.00 L of solution with 19.2 grams of Al203, 0.338 M AI3+ and 0.0593 M O2-, what is the Ke value for the reaction above? (the answer should be entered with 3 significant figures; do not enter units; give answer in scientific notation--valid notation examples include 1.23e-8 and 1.23e8 and -1.23e-4 and 1.23e0)
10. If 223.0 mg of AgBr is completely dissolved in 184.0 ml. of 0.14 M NH3, what is the equilibrium concentration of Ag (aq) in the final solution? KAg(NH3)2] = 1.7E7 Include at least 3 significant figures in your arawer M Grade This Exercise
Complete the balanced chemical reaction for the following weak base with a strong acid. In this case, write the resulting acid and base as its own species in the reaction. CH;NH2(aq) + HCIO3(aq) > 4- 3. 2+ 3+ 4+ 1 2 6 7 8 O2 4 5. ) (s) (1) (g) (aq) H N H30* CI H20 OH 4- +
12) BaSO = Will precipitate form when 1.0x10³ M BaCl₂ is added to 3.3x10 M Al₂(SO₂);? Kof 1.1x10-8.
9. Solid sodium carbonate, Na,CO, is used to determine the concentration of a HBr(aq) by titration. What is the role of sodium carbonate in this titration? (A) Catalyst (B) IndicatorA8 (C) Primary standard (D)Proton donor euld bne el hotsolon (A) nielerd auld lom onolbni Vegnto nouloe s lo ophar Hq es Short Answer 1. Consider the following equilibrium for the chemical indicator phenol red, HInd, at pH = 7.3. 0.00 H,0 = H,O* + Ind red HInd + Yellow If 10.0 mL of 0.10 mol/L NAOH(aq) is added, how will the concentration of H,O* (aq) be affected, and what is the color of the resulting solution?