For a 0.315 M solution of H₂C6H606, calculate both the pH and the C6H₂06²- ion concentration.=7.9x10-5H₂C6H6O6 + H₂O — H3O+ + HC₂H0¯ Ka¹HCH6O6 + H2O=H3O+ + CoH6O2- Ka2 = 1.6×10-12pH=[C6H606²-] =M

Given,Molarity of HC6H6O6 = 0.315 M

For a 0.315 M solution of H₂CH², calculate both the pH and the C6H606²- ion concentration. = 7.9x10-5 1.6x10-12 H₂C6H₂O6 + H₂O ⇒ H3O+ + HCH₂0₁¯ ₂¹ HC₂H₂O6 + H₂O — H³O+ + C6H606²- ₂² = pH = [C6H606²-] = = M

For a 0.315 M solution of H₂CH², calculate both the pH and the C6H606²- ion concentration. = 7.9x10-5 1.6x10-12 H₂C6H₂O6 + H₂O ⇒ H3O+ + HCH₂0₁¯ ₂¹ HC₂H₂O6 + H₂O — H³O+ + C6H606²- ₂² = pH = [C6H606²-] = = M

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: Hydrofluoric acid, HF, unlike hydrochloric acid, is a weak electrolyte. What is the hydronium-ion…

Q: Calculate the pH of the solution. Assume 5.0 L of solution. You must identify the type of solution…

A: Given that: volume of solution = 5 L moles of NH3 = 0.190 moles of HCl = 0.120 Kb(NH3) = 1.8 x…

Q: Determine the pH of each of the following solutions. Part A 0.14 moll -1 C6H5NH3CI (Kb(C6H5NH2) =…

A: The pH of a solution is the negative logarithm of H+ ion concentration.So,

Q: None

A: Step 1:Since H2A is a weak diprotic acid, it can donate two H+ ions. We will find the concentration…

Q: A beaker holds a mixture of 0.40 M HIO3 and 1.0 M HCOOH. Ka(HIO3) = 1.6 x 10-¹ Ka(HCOOH) = 1.77 ×…

A: We know weak acids having lower value of dissociation constant Ka ionise weakly so can ignore their…

Q: Triflourobenzoic acid (C₂H₂F3COOH) is a very uncommon weak acid. If the solution pH is 1.62, the…

Q: The Reg for the H₂O + H₂O → Kw [H3O+¹][OH-¹] tion of water with Wal is called Zw H3O+1 + OH-1 [H₂O]²…

Q: X = .011 - X pOH = -log(011) - 1.96 14-1,96= [pH = 12.041 2-x 4. Codeine (C18H21 NO3) is a…

Q: How many grams of NH4Cl (53.49 g/mol) must be dissolved in 0.639 L of solution in order to obtain a…

A: we need to find mass of NH4Cl in the solution for a pH 4.79

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: If we used H2C4H4O5 as the weak diprotic acid, which of the four species, H2C4H4O5, HC4H4O5^-,…

A: Given that, H2C4H4O5 is a weak diprotic acid & the four species are H2C4H4O5, HC4H4O5-,…

Q: Benzoic acid, HC6H5CO₂, is a monoprotic acid (only one H* ionizes) with a K₂ = 6.5 x 10-5. Calculate…

Q: The hydronium ion concentration of an aqueous solution of 0.43 M formic acid, HCOOH is [H3O+] =…

Q: * pH of a Strong Acid, a Weak Acid The pH of a solution is the negative logarithm of the molar…

A: Ph of given solution= 1.

Q: Calculate the pH of a 0.40 M H2SO3, solution that has the stepwise dissociation constants Ka1 = 1.5…

Q: What is the K₂ reaction of HCN? K₂ reaction: The K₂ of HCN is 6.2 x 10-¹0. What is the K value for…

A: Since you have posted multiple questions, we will provide the solution only for the first question…

Q: Determine the pH of solution if 0.085g of acetylsalicylic acid, HC9H7O4, (Ka = 3.0 x 10-5) is…

Q: Consider the following data on some weak acids and weak bases: name acid solution 0.1 M KCN 0.1 M…

A: pH of a solution is defined as the negative logarithm of Hydrogen ion concentration. pH = -log(H+)

Q: 0.21 М CН3NH3І (Къ(СH3NH2) — 4.4 x 10-4)

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: Consider the following data on some weak acids and weak bases: acid base Ka name formula name…

Q: pH and pOH of [H+] = 7.23×10-4 M

A: Given : [H+ ] = 7.23 X 10-4 M

Q: determite ph of 0.11 molL−1molL−1 NH4Cl 0.12 molL−1molL−1 CH3COONa 0.11 molL−1molL−1 NaClNaCl…

A: #1: NH4Cl or NH4+(aq) is a weak acid with Ka = 5.62x10-10 The dissociation equation is: NH4+(aq) ⇌…

Q: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

A: Given, Based on pH scale we can classify type of solution as acidic, basic or neutral. If pH of a…

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

Q: Calculate [OH-] for a solution where [H3O+]=0.00461 M. [OH-J= Calculate the hydronium ion…

A: Note: As per our guidelines, we are supposed to answer only one question. Please repost the other…

Q: Trimethylamine,(CH3)3N , is produced when plants and animals decompose and has a very unpleasant…

Q: What is the pH of a 0.200 M solution of ammonium chloride (NH4Cl) Refer to these equations NH3(aq)…

A: The pH of a 0.200 M solution of ammonium chloride (NH4Cl) is to be calculated. Refer to these…

Q: The pH of a 0.12-M solution of phosphoric acid (H3PO4) is measured to be 1.60. Use this information…

A: In this question, we want to determine the Ka value of Phosphoric acid. You can see below step by…

Q: The pH of a 8.3×10-2-M solution of phthalic acid (H2C8H4O4) is measured to be 2.03. Use this…

Q: For the diprotic weak acid H2A, ?a1=2.9×10−6 and ?a2=8.2×10−9. What is the pH of a 0.0650 M solution…

A: Diprotic acid is dibasic acid which has two acidic H+. This will dissociate two times.

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: A triprotic acid (H3Y) has the following acid ionization constants: Ka1 = 5.3 x 104 Ka2 = 1.7 x 10-8…

A: Given: pH=6.93Ka1=5.3x10−4;Ka2=1.7x10−8;Ka3=3.2x10−11Step 1: Solve for the pKa values of each…

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: Each value represents a different aqueous solution at 25 °C. Classify each solution as acidic,…

Q: A student planned an experiment that would use 0.10 M propionic acid, HC3H₂O₂. Calculate the value…

Q: The substance benzoic acid (C6H5COOH) is a weak acid (K₂ = 6.3x10-5). What is the pH of a 0.230 M…

Q: The Ka of propanoic acid (C,H,COOH) is 1.34 x 10-5. Calculate the pH of the solution and the…

Q: Diisopropylamine, C6 H14NH, is a weak base. A 0.66 M aqueous solution of diisopropylamine has a pH…

A: We have to predict the Kb and the pH of Solution.

Concept explainers

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.

Question

For a 0.315 M solution of H₂C6H606, calculate both the pH and the C6H₂06²- ion concentration.
=
7.9x10-5
H₂C6H6O6 + H₂O — H3O+ + HC₂H0¯ Ka¹
HCH6O6 + H2O=H3O+ + CoH6O2- Ka2 = 1.6×10-12
pH
=
[C6H606²-] =
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: Determine the pH and C6H6H6 2- ion concentration from the given data:

VIEW

Step 2: Calculation for hydronium ion concentration :

VIEW

Step 3: Calculation for pH and C6H6O6 2- concentration:

VIEW

Solution

VIEW

Step by step

Solved in 4 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

A solution has a pH of 3.76. What is the molarity concentration of H3O+ and OH¹ in this solution? A) [H3O+] = 5.8 x 10-11, [OH] = 1.7 x 10-4 B) [H3O+] 1.7 x 104, [OH] = 5.8 x 10-11 = [H3O+] = 1.7 x 104, [OH] = 5.8 x 10-10 D) [H3O+] = 5.8 x 10+³, [OH] = 1.7 x 10+10
Consider the following data on some weak acids and weak bases: acid base Ка K, name formula name formula 8- 3.0 × 10 - 8 hypochlorous acid HCIO hydroxylamine HONH, 1.1 × 10 -4 6.8 × 10 ethylamine C2H5NH2 | 6.4 × 10 alo -4 hydrofluoric acid HF Ar Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to thể"s will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 М KСІ choose one v 0.1 M KCIO choose one v 0.1 M HONH3Br choose one v 0.1 M NaF choose one v
The ionization of benzoic acid is represented by this equation. C6H5COOH(aq) ↔ H+(aq) + C6H5COO–(aq) If a 0.055 M solution of benzoic acid, at a certain temperature, has an [H+] =2.7 × l0−3, what is the Ka of benzoic acid?
Stuck on this :(
Assuming 0.1 M concentrations, arrange the following acid solutions in order of increasing pH. benzoic acid, HC7H5O2, Ka ≡ 6.3 × 10−5 chlorous acid, HClO2, Ka ≡ 1.1 × 10−2 formic acid, HCHO2, Ka ≡ 1.8 × 10−4 hydrofluoric acid, HF, Ka ≡ 6.8 × 10−4
Consider the following data on some weak acids and weak bases: acid base Ka name formula name formula HNO, 4.5 x 10 CgH;NH2|4.3 × 10 - 10 -4 nitrous acid aniline 4 -8 hydrofluoric acid HF 6.8 × 10 hydroxylamine HONH, 1.1 x 10 Use this data to rank the following solutions in order of increasing pH. In other words, select a '1' next to the solution that will have the lowest pH, a '2' next to the solution that will have the next lowest pH, and so on. solution pH 0.1 M HONH3CI choose one v 0.1 M Nal choose one v 0.1 M KNO2 choose onev 0.1 M NaF choose one v
The pH of a 0.56M solution of hexanoic acid (HCH0,) is measured to be 2.55. Calculate the acid dissociation constant K, of hexanoic acid. Be sure your answer has the correct number of significant digits. K. = 0 -10 The acid dissociation constant K, of boric acid (H,BO,) is 5.8 x 10 . a Calculate the pH of a 0.42M solution of boric acid. Round your answer to 1 decimal place. pH =
For propanoic acid, a weak monoprotic acid (HC3H5O2, Ka = 1.3 x 10-5), calculate [H+] and pH of a 0.10 M solution.
Calculate the pH of a 0.29 M H2SO3, solution that has the stepwise dissociation constants Ka1 = 1.6 × 10-2 and Ka2 = 6.4 × 10-8.
Find the H3O+H3O+ concentration of a 0.220 MM hypochlorous acid solution (whose acid dissociation constant is Ka=2.9×10−8Ka=2.9×10−8). Express the concentration to two significant figures.
H3PO4 is a weak polyprotic acid with K₁ = 7.2x10³, K₂= 6.3x10^-8, and K3 = 4.2x10^-13. What is the pH of a 0.275 M solution of KH₂PO4? Simplifying assumptions may be made. Give answer to 2 decimal places.
For the diprotic weak acid H2A, Kal =3.4 •10^-6 and Ka2=8.5 •10^-9. what is the pH of a 0.0700M solution of H2A? pH=What are the equilibrium concentrations of H2A and A2- in this solution? [H2A]=M [A2-]=M