Be sure to answer all parts.Calculate the concentrations of H₂C₂O4, HC₂0, C₂02, and H* ions in a 0.271 M oxalic acid solutionat 25°C. (K₁-6.5 x 102 and Ka, -6.1 x 105 for oxalic acid.)[H₂C₂O4] 0.71X[HC₂041 0.13 x[C₂021-[H] 0.133(Enter your answer in scientific notation.)

[C2H4O2]=0.271 MKa1=6.5×10-2Ka2=6.1×10-5

Be sure to answer all parts. Calculate the concentrations of H₂C₂O4, HC₂0, C₂02, and H ions in a 0.271 M oxalic acid solution at 25°C. (K 6.5 x 102 and K₁, 6.1 x 105 for oxalic acid.) [H₂C₂O4 0.71 [HC₂041-0.139 [C₂021- [H] 0.133 (Enter your answer in scientific notation.) х 100

Be sure to answer all parts. Calculate the concentrations of H₂C₂O4, HC₂0, C₂02, and H ions in a 0.271 M oxalic acid solution at 25°C. (K 6.5 x 102 and K₁, 6.1 x 105 for oxalic acid.) [H₂C₂O4 0.71 [HC₂041-0.139 [C₂021- [H] 0.133 (Enter your answer in scientific notation.) х 100

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: Consider an aqueous solution that is 0.050 M in H2Se (Ka = 1.29 x 10-4) and 0.075 M in NaHSe. Out…

A: Given, 0.050 M in H2Se 0.075 M in NaHSe

Q: Consider the Ka information to answer parts a-b. Ka 7.2 x 10 * K 4.2 x 10- Formula Kat 6.3x 10 a.…

A: Answer:- This question is answered by using the simple concept of calculation of Ka and Kb value…

Q: Which of the failowingis the reaction quotient expression for the ionization of NH, n water? The…

Q: A solution is prepared that is initially 0.19M in methylamine (CH3NH₂), a weak base, and 0.48M in…

A: Buffer solution is a type of solution that resists the change in its pH on adding small quantity of…

Q: A solution is prepared that is initially 0.27M in hypochlorous acid (HCIO) and 0.34M in sodium…

A: The concentration of the hypochlorous acid The concentration of the sodium hypochlorite We have to…

Q: A diprotic acid, H, A, has acid dissociation constants of Kal concentrations of H, A, HA, and A2- at…

Q: V2. A student prepared a 0.855 M solution of chloro acetic acid, CH2CICOOH, and measured the pH to…

Q: A student is told by their chemistry professor that he thinks he remembers that the ion product…

A: Hydrogen ion concentration is calculate as shown below where [H+], [OH-], and [Kw] are the…

Q: Calculate the concentrations of H2C2O4, HC2O4−, C2O42−, and H+ ions in a 0.165 M oxalic acid…

A: The dissociation of oxalic acid takes place as , H2C2O4 (aq) --->…

Q: Tartaric acid is found in many fruits including grapes. Tartaric acid is partly responsible for the…

A: The dissociation of tartaric acid can be represented as: H2C4H4O6+H2O↔HC4H4O6-+H3O+…

Q: Calculate the [NH₃] in a solution of 0.330 M ammonium fluoride (NH₄F). Hint: Use the Ka of HF (6.8 ×…

A: From given Calculating NH3 from the concentration of ammonium fluoride

Q: What is the pH of a solution that is 0.20 M potassium cyanate, KCNO and 0.16 cyanic acid HCNO? The…

Q: A diprotic acid, H₂A, has acid dissociation constants of K₁₁ = 3.75 x 10 and K₂ = 5.10 × 10-¹¹.…

A: To calculate the concentration of H2A, HA- and A2-, for the following solutions: (a) 0.195 M…

Q: Assume the following substances form solutions at the same concentration, whicch one would provide…

A: According to Arrhenius concept, an acid is a substance i.e. when dissolved in water gives H+ ions.…

Q: An acid of the formula, HC6H5O, is a weak monoprotic acid. Its Ka is 1.1 x 10-10. A solution of this…

A: Given : Mass of HC6H5O = 14.5 g Volume of solution = 892 mL = 0.892 L…

Q: For a 0.0494 M aqueous solution of cyanic acid, HCNO (Ka = 3.5*10-4), determine the following. What…

A: Given Data : 1. Molarity of cyanic acid solution = 0.0490M 2. Dissociation constant of cyanic acid…

Q: . The equilibrium constant for the dissociation of a weak acid of the type, HA⇌H++ A-, would be:…

Q: A sample of gas is at 45.0 °C. At what temperature would the volume of this gas be the double of the…

A: Dear student , since you have posted multiple questions we will allow to solve only first question…

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: Calculate the equilibrium concentrations of the following in a 0.100 M oxalic acid, (COOH)2…

Q: A solution contains 0.321 M potassium fluoride and 0.165 M hydrofluoric acid (K₁ = 7.20 x 10-4). The…

A: A buffer solution is formed by the mixing of weak acid and its conjugate base. The pH of a buffer…

Q: 13.2) a) A 0.439-M aqueous solution of a weak acid has a pH of 4.56. Calculate Ka for the acid.…

A: Please find the solution as hand written note.

Q: Write the equilibrium-constant expressions and obtain numerical values for each constant in a. the…

Q: What will the concentrations be for a, b, and c? What is the pH of the solution?

A: Concentration = moles/volume.[pyridine] =mol/volume = 0.3mol/1 L = 0.3M.

Q: Calculate the pH and fraction of dissociation (a) for each of the acetic acid (CH, COOH, pK, -…

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: A 1.00 M solution of fluoroacetic acid is 10.0% dissociated in water at a certain temperature. The…

A: Dissociation of fluoroacetic acid is given We have to calculate pOH Ka pH on dilution

Q: For the diprotic weak acid H₂A, K₁1 = 3.5 x 10-6 and K₁2 = 8.3 × 10-⁹. What is the pH of a 0.0500 M…

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: Part 3 - Put it all together. Calculate the concentrations of all species in a 1.47 M Na₂SO3 (sodium…

A: Given,Molarity of Na2SO3 = 1.47 MKa1 ( H2SO3 ) = 1.4 x 10-2Ka2 ( H2SO4 ) = 6.3 x 10-8…

Q: A diprotic acid, H, A. has acid dissociation constants of K₁1 = 4.63 x 10 and K₂ = 5.82 x 10-12.…

Q: NH3 is a weak base (Kp = 1.8 x 10³) and so the salt NHĄCI acts as a weak acid. What is the pH of a…

A: At Temperature 25°C Kb (NH3) = 1.8 × 10-5 [NH4Cl] = 0.028 M

Q: Sodium bicarbonate gives solutions that are slightly alkaline (approximately pH 8.3), and similar…

A: Here we have to determine the pH of 0.26M Sodium carbonate solution.

Q: The propionate lon, CH CH,COO", reacts with water as a weak base: CH CH,COO", (aq) + HO)…

Q: The value of K, for hypochlorous acid , HCIO , is 3.50x10-8. Write the equation for the reaction…

A: Equilibrium reaction of HClO, HClO(aq) + H2O(l) -------> ClO-(aq) + H3O+(aq)

Q: What equation would you use for the percent ionization /dissociation of a weak base?…

A: A weak base is a weak electrolyte and it does not dissociate completely in the aqueous solution. The…

Q: 85. Formic acid (HCO₂H) was first isolated by the destruc- tive distillation of ants. In fact, the…

A: Answer:HCOOH is a weak organic acid and when added in water, its partial ionization takes place and…

Q: C6H4NH2COOH, para-aminobenzoic acid (PABA), is used in some sunscreen agents. Calculate the…

A: Consider the given information is as follows; Concentration of C6H4NH2COOH = 8.0×10-2 MKa =…

Q: Aqueous solutions of a particular mono basic acid HX have the following pH values (see figure…

A: The equation of dissociation of acid is as follows: HXaq +H2O(l) →H3O+(aq) + X-(aq) The dissociation…

Q: Part A Find [H3O]* at equilibrium of a 0.110 mol ·L' solution of a weak monoprotic acid (HA) with Ka…

A: (A) Given: The dissociation of HA is written as follows: HA(aq)+H2O(l)------>H3O+(aq) + A-(aq).…

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: You have 50.0 mL 0.10 M NazPO4 to which you add 50.0 mL 0.19 M NaH PO4. What is the pH of this…

A: We can calculate the pH of the solution using the formula, Calculate the total volume of the…

Q: etermine [H3O+] and [OH] concentrations (in M to two decimal places) for each: (a) Pure water at 10…

A: pH of a solution is defined as negative logarithmic of concentration of hydrogen ions

Q: HCN

A: When we add NaCN in HCN then pH will change .

Q: A diprotic acid, H,A, has acid dissociation constants of Ka = 4.88 x 10-4 and K2 = 5.41 x 10-12.…

A: The dissociation of diprotic acid H2A can be written as; H2A (aq)⇔H+(aq) + HA-(aq)…

Q: Calculate the pH of a solution that is a mixture of 0.030M HNO3, 0.55M CH3COOH, and 0.015M HI. Ka…

A: Given data : HNO3 = 0.030 M HI = 0.015 M CH3COOH = 0.55 M

Q: The pH of a 0.0200 M solution of an unknown acid is 2.56. What is the Ka of this acid? To solve this…

A: Weak acid does not dissociate completely HA(s) + H2O(l) ⇔ H3O + (aq) +…

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

Be sure to answer all parts.
Calculate the concentrations of H₂C₂O4, HC₂0, C₂02, and H* ions in a 0.271 M oxalic acid solution
at 25°C. (K₁-6.5 x 102 and Ka, -6.1 x 105 for oxalic acid.)
[H₂C₂O4] 0.71X
[HC₂041 0.13 x
[C₂021-
[H] 0.133
(Enter your answer in scientific notation.)

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: Given values.

VIEW

Step 2: Construct an ICE table for the first dissociation of oxalic acid.

VIEW

Step 3: Construct an ICE table for the second dissociation of oxalic acid.

VIEW

Step 4: Calculation of concentration of ions.

VIEW

Solution

VIEW

Step by step

Solved in 5 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

H₂PO4 is a weak, triprotic acid. The acid dissociation constants are K₁1-7.1 x 10³, K₂2-6.2 x 10%, and K-4.5 x 10-13. Calculate the equilibrium constant for the reaction below. H₂PO4(aq) PO4 (aq) + 3H (ag) O 7.1 x 10-3 2.0 x 10-22 044 x 10-10 8.7 x 10-6 O 20 x 10
A diprotic acid, H, A, has acid dissociation constants of K₁1 = 4.76 x 10-4 and K₁2 = 3.59 x 10-12. Calculate the pH and molar concentrations of H₂A, HA, and A2- at equilibrium for each of the solutions. A 0.205 M solution of H₂A. pH = [HA] = A 0.205 M solution of NaHA. pH= [HA] = M M [H₂A] = [A²-] = [H₂A] = [A²-] = M M M M
From the equilibrium concentrations given, calculate Ka for each of the weak acids. a) CH3CO2H: [H3O+]= 1.34 x 10^-3 [CH3CO2H]= 9.866 x 10^-2 [CH3CO2-]= 1.34 x 10^-3 b) ClO- [OH-]= 4.0 x 10^-4 [HClO]= 2.38 x 10^-5 [ClO-]= 0.273 M
If the carbonic acid (H2CO3) concentration in a sample of blood is 0.0050 M, determine the bicarbonate ion (HCO3-) concentration required to buffer the pH of the blood at pH = 7.35. Show all calculations including equation(s) used. H2CO3(aq) ⇌ HCO3-(aq) + H+(aq) Ka = 4.3 × 10-7
A solution is prepared that is initially 0.087 M in benzoic acid (HC6H5CO2) and 0.11 M in potassium benzoate (KC6H5CO2). Complete the reaction table below, so that you could use it to calculate the pH of this solution. User to stand for the unknown change in [H3O+] You can leave out the M symbol for molarity
please help with this problem
A solution is made by mixing exactly 500 mL of 0.147 M NaOH with exactly 500 mL of 0.100 MCH3COOH. Calculate the equilibrium concentration of the species below. Ka of CH3COOH is 1.8 × 10−5 [ H+ ] × 10 MEnter your answer in scientific notation. [ OH− ] M [ CH3COOH ] × 10 MEnter your answer in scientific notation. [ Na+ ] M [ CH3COO− ] M
A solution contains 0.363 M HA (Ka = 6.74:10-46.74:10-4) and 0.677 M NaA. What is the pH of this solution? What is the pH of this solution after 0.178 mol of HCl are added to 1.00 L of this solution? What is the pH of this solution after 0.356 mol of HCl are added to 1.00 L of this solution?
Calculate the pH when 45.0 mL of 0.100 M NaOH is added to 50.0 mL of 0.100 M CH3COOH (acetic acid) solution. CH3COOH (aq) + H2O (l) CH3COO - (aq) + H O + (aq) K a = 1.8 x 10 -5 4.12 8.21 2.97 5.69 9.15 4.06 4.87
Calculate the concentrations of all species in a 0.760 M Na₂SO₂ (sodium sulfite) solution. The ionization constants for sulfurous 1.4 x 10-2 and K₁2 6.3 × 10-8. acid are Kal = [Nat] = [HSO] = [OH-] = = M M M [so-] = [H₂SO3] = [H+] = M M M
A diprotic acid, H, A, has acid dissociation constants of Kal 4.76 x 10-4 and Ka2 5.22 x 10-12. Calculate the pH and molar concentrations of H, A, HA¯, and A2- at equilibrium for each of the solutions. A 0.124 M solution of H, A. [H,A] = pH = M [HA¯] = [A²-] = М M A 0.124 M solution of NaHA. pH= [H,A] = M [HA¯] = [A²-] = M M A 0.124 M solution of Na, A. pH= [H,A] = M [HA¯] = M [A²-] = M
Muscles produce lactic acid, CH₂CH(OH)COOH(aq), during exercise. Calculate the percent ionization (deprotonation), pH, and pOH of a 0.1120 M solution of lactic acid. The acid-dissociation (or ionization) constant, K₁, of this acid is 8.40 × 10-4. percent ionization = pH = pOH = %