All reactions are at pH of 0 unless otherwise indicated. Because it has caused confusion in the past, let me be clear. You are asked to draw a poutbaix diagram for the table below. You are asked to draw a poutbaix diagram for Sulfur from the data below.Given Rxn data: Only use the given reaction data.ReactionE (V)S+ H20 + 2 e = SH° + OH"-0.478 pH = 14%3DS+ 2 H* + 2 e2 HS(ag)0.142S20g2 + 2 e=2 SO,²-2.010HSO3 + 5 H* + 4 e2S+ 3 H2O0.480SO32 + 6 H* + 4 e S+3 H2O-0.658 pH =14SO,2 + 4 H* +2 e2 H2SO3 + H2O0.172SOQ + H2O + 2 e SO3² + 2 °OH-0.930 pH = 14S2062 + 4 H* + 2 e° ² 2 H2SO30.5642 SO,2 + 4 H* + 2 e°² S20g²² + H20-0.22

Answered: Image /qna-images/answer/087cf742-5078-4059-9e36-c7634bef43e3.jpg

Answered: pH of 0 unless otherwise indicated.…

pH of 0 unless otherwise indicated. Because it has caused confusion in the past, let me be clear. You are asked to draw a poutbaix diagram

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 82AP

See similar textbooks

Related questions

Q: Identify the bronsted lowry acids and bases and their conjugated in the reaction HCO3- + H20…

Q: HO но. OH он NH, NH, NH3 (A) (B) (C) NH3 NH2 (D) (E) Dominates at pH 1 Use parentheses! Does not…

Q: Consider 0.1M H3A (Given Ka1= 1x10-4 , Ka2=1x10-9, Ka3=1x10-12 ). Calculate the Concentration of…

Q: Which of the following reactant combinations will result in a triol? -- Malic acid + LiAlH4 --…

A: Both LiAlH4 and NaBH4 are reducing agents. But, LiAlH4 is a stronger reducing agent than NaBH4.…

Q: CH3COO- (aq) + H+ (aq) ⇔ CH3COOH (aq), is an example of ________. Bronsted base…

A: Acid base concept is given by Bronsted as well as Arrhenius . Arrhenius acid is that which…

Q: The pH of a 1.1M solution of 4-pyridinecarboxylic acid (HC H,NO,) is measured to be 2.46. Calculate…

A: Dissociation constants are the equilibrium constants for ionization reactions. Dissociation constant…

Q: After creating a graph of pH versus log([HIn]/[In-]), the following trendline is obtained. y =…

A: Given: The graph of pH versus log([HIn]/[In-]) for bromophenol blue is following the trendline : y =…

Q: Name each functional group in these molecules as polar acidic, polar basic, polar neutral or…

A: The functional groups are

Q: Label acidic basic or neutral: (you will first need to find the pH) 9.5 x 10^-11 M NH3

A: As per the given data Concentration of NH3=9.5×10-11MpH=?

Q: List 4 factors that can influence the acidity of a Bronsted-Lowry acid (and thus, the stability of…

A: factors that can influence the acidity of a Bronsted-Lowry acid (and thus, the stability of its…

Q: Determine whether the given salt will undergo hydrolysis or not. Write: YES or NO (Note: case &…

Q: CH3NH2 is a (a)Arrhenius acid. (b)Arrhenius base. (c)Bronsted-Lowry acid.…

A: From given we are going to determine CH3NH2 ( methyl amine) nature

Q: In the following unbalanced reaction, which reactant acts like the Bronsted-Lowry acid? H3PO3 (aq)…

A: Answer

Q: SAMPLE Calamansi Tap water Distilled Water Vinegar Sugar in water Baking soda Comstarch Soft drink…

A: Acid or Base Depending on how one chooses to see the characteristics of acidity and basicity, the…

Q: Which would you predict to be the weakest acid? Lactic Acid (Ka = 1.4 x 10-4) Hydrofluoric…

A: Acidity: The acidic nature of chemical substances can be determined by their pH value. Stronger acid…

Q: 8. Which one of the following will be most acidic and why? 2-Chlorobutanoic acid, 4- Chlorobutanoic…

Q: 4- Lewis Acid accept an electron pair BF3 Base donates an electron pair : NH3 True False

A: In this question we have to tell the given statement is true or false.

Q: NaOH, DMSO solvent Br Ph Br NaOH, DMSO solvent Ph Br NaOH, DMSO solvent Br LDA, THF solvent

Q: In the reaction BF3 + NH3 → F3B:NH3 , the BF3 functions as a(an) __________. Bronsted-Lowery…

A: We are having reaction between ammonia and boron-trifluoride . We have to predict the nature of BF3.

Q: Label acidic basic or neutral: (you will first need to find the pH) 7.7 x 10^-7 M HNO3

A: Answer is explained below. Concentration of HNO3 is 7.7×10-7 M (Given). Thus, [H3O+] = 7.7×10-7 M.

Q: The main active ingredient in Tums© is calcium carbonate. It is used as a neutralizing agent when…

A: Given: The main active ingredient in Tums is calcium carbonate. It is used as a neutralizing agent…

Q: An aqueous solution of CH3NH3NO3 will be Group of answer choices A. basic, because of the…

A: Since the salt given CH3NH3NO3 is made from the acid HNO3 and base CH3NH2. And we know that the salt…

Q: H2PO41- + HS1- -> HPO42- + H2S In the reaction, H2PO41- is acting as a Bronsted acid In the…

A: According to the Bronsted and Lowry concept, an acid is a hydrogen-containing species (a molecule, a…

Q: Ка(НС-Нз О2) %3D 1.8 х 10 5 1. 0.10 M acetic acid/0.30 M sodium acetate pH : 2. 0.30 M acetic…

Q: Label each substance as an Arrhenius acid, Arrhenius base, or neither. HNO3(aq)…

A: Arrhenius acids are the compounds which can donate hydronium ion, thus will increase the…

Q: What is the pOH of 0.10 M mandelic acid 0.10 M maleic acid 0.10 M malonic acid

A: since basicity factor of mandelic acid is 1 therefore pH = - log ( 0.1) pH = 1 pOH = 14 -…

Q: Identify the base in the following non-aqueous reaction POCl3 + Cl- → POCl4-

A: The base in non aqueous medium is given below

Q: Complete the balanced molecular reaction for the following weak base with a strong acid: NaClO2(aq)…

A: Since we know that when sodium chlorite react with sulfuric acid to produce sodium sulfate, chloric…

Q: Calculate [OH−] for each solution. pH=1.82 pH=13.28 pH=8.29 pH=2.32

A: Given : a) pH = 1.82 b) pH = 13.28 c) pH = 8.29 d) pH = 2.32

Q: Physical Properties Odor Physical…

Q: Using their Ka values, what is the pOH of 0.10 M mandelic acid 0.10 M maleic acid 0.10 M malonic…

A: Ka = [H+][A-]/[HA] .....................(i) [H+] is the concentration of the proton…

Q: Classify K2O strong acid weak acid strong base weak base

A: Acid- The species which is able to donate H+ ion is called as acid. Bade The species which is able…

Q: ative pH before the addition of any HCl. ative pH after 56.0 mL HCl has been added. ative pH after…

A: 1) Before HCl , it is base. Hence , pH > 7 (A) is correct option. 2) after adding 56.0 mL it…

Q: Write the net ionic equation for the acid-base hydrolysis equilibrium that is established when…

Q: Convert each of the following OH- concentrations to pH. 1.1M 2.5 uM 0.030M

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question…

Q: An acidic solution at 25°C has [H3O+] > 1 × 10-7 M > [OH-]. [H3O+] [OH-]. [H3O+] = [OH-] > 1 ×…

A: The dissociation reaction of water is: H2O(l)+H2O(l)⇌H3O+(aq)+OH-(aq) The dissociation constant for…

Q: Circle the solution in each pair with the Higher pH. Lactic acid Ka = 1.4 x 10-4 Hydrocyanic acid…

A: a) Since more is the concentration of acid, more will be the acidity of the acid And more is the…

Q: Does the pH increase, decrease, or remain the same when each of the following is added? EXPLAIN:…

A: pH = -log[H+] So the concentration of H+ increases pH of the solution decreases while when…

Q: Ethanol can act as either a Lewis acid or a Lewis base (donates or accepts a pair of electrons).…

A: Ethanol is an alcohol with two carbon atoms bearing an alcoholic group with a molecular formula…

Q: 1)Why the PH start from 0 to 14 ? 2) why PH =14

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

Q: Order from lowest to highest pH i. 0.10M NaClO ii. 0.10M KBr iii. 0.10M NH4ClO4 ii

A: any solution, existence of any weak acid along with strong base results the higher pH (pH>7)…

Q: After creating a graph of pH versus log([Hln]/[In-1), the following trendline is obtained. y =…

Q: DQ6: Acid- Base Equilibria Discussion Topic

A: An acid is that which donates proton. Stability of acidity depends on various factors.

Q: Label acidic basic or neutral: (you will first need to find the pH) 6.0 x 10-2 M HCl

Q: Calculate the H3O+H3⁢O+ concentration for each pH. pH= 12 [H3O+] = M pH= 2 [H3O+] =…

A: pH is a negative logarithm of Hydrogen ion concentration, it is potenz or power of Hydrogen ion…

Q: Predict the Nature of the Adduct between the hard acid/base and soft acid/base with examples for…

A: The metal ions of alkali metals, light transition metals with higher oxidation states (Ti4+, Cr3+,…

Q: acidic dissociation of methyl ammonium hydrochloride,

Q: Assign each species on the left to a category on the right. Clear All NH3 LiOH HCl HF strong acid…

A: The correct answer is given below:-

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

All reactions are at pH of 0 unless otherwise indicated. Because it has caused confusion in the past, let me be clear. You are asked to draw a poutbaix diagram for the table below.

You are asked to draw a poutbaix diagram for Sulfur from the data below.
Given Rxn data: Only use the given reaction data.
Reaction
E (V)
S+ H20 + 2 e = SH° + OH"
-0.478 pH = 14
%3D
S+ 2 H* + 2 e2 HS(ag)
0.142
S20g2 + 2 e=2 SO,²-
2.010
HSO3 + 5 H* + 4 e2S+ 3 H2O
0.480
SO32 + 6 H* + 4 e S+3 H2O
-0.658 pH =14
SO,2 + 4 H* +2 e2 H2SO3 + H2O
0.172
SOQ + H2O + 2 e SO3² + 2 °OH
-0.930 pH = 14
S2062 + 4 H* + 2 e° ² 2 H2SO3
0.564
2 SO,2 + 4 H* + 2 e°² S20g²² + H20
-0.22

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 by step

Solved in 4 steps with 4 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

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
3.81944444 Be sure to answer all parts. The AG° for the reaction H;2) + I;(2) = 2HI(g) is 2.60 k.J'mol at 25°C. In one experiment, the initial pressures are PH, = 3.96 atm P, = 0.020 atm PHI = 0.55 atm Calculate AG for the reaction and predict the direction of the net reaction. kJimol The net reaction proceeds from left to right The reaction proceeds from right to left
Give the pH of 0.005 M C6H5O- (aq) at 298 K of the Ka for C6H5OH at the given T is 1.0 x 10-10
Ascorbic acid (H₂C,H,O) is a diprotic acid. The acid dissocation constants for H₂C,H,O, are Kal = 8.00 x 10-5 and K₁2 = 1.60 x 10-12 Determine the pH of a 0.117 M solution of ascorbic acid. pH = Determine the equilibrium concentrations of all species in the solution. [H₂C,H,O,] = [HC,H,O,]= [C,H,O2] = M M M
Use systematic treatment of equilibrium to solve this problem and determine the pH. STEP by STEP f. A 100 mM solution of ammonium acetate (CH3COO NH4). Use activity coefficients. NH4+ (aq) NH3(aq) + H+ (aq) 1 Ka= 5.69 x 10-10 CH₂COOH(aq) → CH3COO- (aq) + H+ (aq) Ka = 1.75 x 10-5
Determine if the following salt is neutral, acidic or basic. If acidic or basic, write the appropriate equilibrium equation for the acid or base that exists when the salt is dissolved in aqueous solution. If neutral, simply write only NR. KC3H;O3 O4- 3- O2+ 3+ D 4+ 1 2 3 4 6. 7 8 9 1 3 4 6. 7 (s) (1) (g) ||(aq) + NR OH C H H30* H20 K Reset • x H20 Delete 1L LO 2. 2.
R = 8.314 mol-K F = 96,485 mol AG = AG° + RT · In(Q) ΔΕ - (E) · In(Q) ΔΕ. Half Reaction (Note: All given as reduction) E° (V) 02 (g) + 4 H*(aq) + 4 e 2 H20 (1) 1.229 Z2 (s) + 2 e 3+ (aq) + 3 e 2z (aq) 0.426 A (s) 0.292 2 H20 (1) + 2 e G2+ (aq) + 2 e M²+ (aq) + 2 e¯ H2 (g) + 2 OH¯ (aq) - 0.828 G (s) - 1.245 M (s) - 1.893 A student constructs a voltaic electrochemical cell with two metal electrodes [metal G and metal A] in their respective aqueous nitrate solutions [G(NO3)2 and A(NO3)3]. Use this information, as well as the reduction potentials in the table above to complete each statement below. Consider the same cell from the above prompt. Calculate A E°. cell for this galvanic cell given the reference information given at the top of the quiz. Report your answer with 3 decimal places. You do not need to report units with your answer.
Calculate the equilibrium constant (Kc) for the following reaction: CH3COOH(aq) + OHlaq))= CH3CO0 (aq) + H2O() The K, of acetic acid is 1.75 x 105; and Kw, (H2O(1) + H20() HO (aq) + H30*(aq)) for auto-ionization of water = 1x 10 14 Hint: First write the equilibrium expressions for acetic acid and the authorization of water separately then apply manipulation rules of Kand find the answer) BIU A- A 工E三 xx,三三 12pt Paragraph
The solubility of salts that contain the conjugates of weak acids increase in acidic solution. Given the reaction of CUCN (Ksp = 3.47 x 10-20) with an acid in the form H3O+ shown below, find the equilibrium constant for this reaction given that Ka HCN = 4.9 x 10-10. CUCN(s) + H:O*(aq) = Cu"(aq) + HCN(aq) + H2O(1)
7-43. Supply the missing data in the table below. Molar Analytical Concentration, c- (ct = Cha + cx-) pH (A"] Acid (HA] Hypochlorous 0.280 7.00 Nitrous 0.105 0.413 0.587 0.145 0.221 Hydrogen cyanide Sulfamic 0.250 1.20
7-43. Supply the missing data in the table below. Molar Analytical Concentration, c- Acid (Ct = CHa + Ca-) pH (HA] [A^] Lactic 0.120 0.640 Iodic 0.200 0.765 Butanoic 5.00 0.0644 Hypochlorous 0.280 7.00 Nitrous 0.105 0.413 0.587 Hydrogen cyanide Sulfamic 0.145 0.221 0.250 1.20
Calculate the pOH of a 0.0461 M HCIO, solution at T (°C) Kw each temperature. 1.15 x 10-15 5 1.88 x 10-15 10 2.97 x 10-15 0°С рОН 3 15 4.57 x 10-15 20 6.88 × 10-15 30 1.46 x 10-14 45 °С рОН %3D 35 2.07 × 10-14 40 2.88 x 10-14 45 3.94 x 10-14 50 5.31 x 10-14 100 5.43 x 10-13