Part A: Please calculate pKa of formic acid below: (HCOOH  H+ + HCOO-) Part B: What is pH of a solution containing 10 mM formic acid? G°f HCOOH = -372 kJ/mol G°f HCOO- = -351 kJ/mol G°f H+ = 0 kJ/mol

Part A: Please calculate pKa of formic acid below: (HCOOH  H+ + HCOO-) Part B: What is pH of a solution containing 10 mM formic acid? G°f HCOOH = -372 kJ/mol G°f HCOO- = -351 kJ/mol G°f H+ = 0 kJ/mol

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: 3. 3. Label the acid, base, conjugate acid and conjugate base in each of the following reactions: +…

Q: 10. Arrange the following acid from weakest to strongest: CH.COOH (Kh= 5.56 x 10-1) HNO2 (Kh = 2.17…

A: We have given that Kb for CH3COOH = 5.56×10-10 Kb for HNO2 = 2.17 ×10-11 Kb for HCN =…

Q: 2. The hydrogen ion concentration, [H*], of a solution, given its pH, can be calculated by taking…

A: The substances present in the environment can be classified into three categories base on the power…

Q: Given the reaction: CO32-+ H2PO4--HCO3+ HPO4², identify the conjugate acid in the reaction co3- HCO3…

A: In the Bransted-Lowry definition of acid and bases, a conjugate acid-base pair consists of two…

Q: Calculate the pH of each solution. A solution containing 0.0313 M maleic acid and 0.044 M disodium…

A: ANSWER-1The pH for the maleic acid and disodium maleate solution is approximately 2.07.ANSWER-2The…

Q: For each of the following reactions, identify which reactant is the acid, which reactant is the…

A: Acid is a substance which donates proton i.e H+ ion in the reaction. Bases are those substances…

Q: when the pH of a solution containing 15mL of 0.10 M CH3COONa and 10 mL of 0.10M CH3COOH (pKa=4.74)?…

Q: Given the Kb of C6H5NH3+ is 3.98x10-10 : 1.) What is the [H3O+] concentration in a solution that is…

A: Given, Given the Kb of C6H5NH2 is 3.98x10-10 : The [H3O+] concentration in a solution that is…

Q: . Arrange the following solution from lowest pH to highest pH: 0.20 М СH:CООН (Ка 3D 1.8 х 10 5)…

A: Given data, Molarity of CH3COOH = 0.20M Ka of CH3COOH = 1.8 x 10-5 Molarity of NH3 = 0.05M Kb of NH3…

Q: Name Period Directions: read each section and answer the questions accordingly. Show all…

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

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

A: The given incomplete reaction is NaClO aq+H2SO4 aq→. To write the complete balanced molecular…

Q: Calculate the [H+] and pH of a 1.39×10-4 M butanoic acid solution. The Ka of butanoic acid is…

A: The objective of this question is to calculate the concentration of hydrogen ions [H+] and the pH of…

Q: What is the conjugate base in the following reaction: H2CO3 + H2O --> H3O* + HCO3 O H2O O HCO, O…

A: Conjugate base can be defined as the substance (an acid) which loses a proton. Conjugate acid-base…

Q: What is the concentration of a weak acid if its Ka = 3.7 x 10-7 and its pOH = 11.62?

Q: A HCOOH (formic acid) solution contains 1.35% formic acid by mass (assume density of 1.01 g/mL for…

Q: Please answer the pOH, [H3O+], [OH-]

A: Given,

Q: What is pH of H2SO4 solution of 10 mg/L?

A: pH :- It is a scale to measure the acidic or basic property of any substance . That tells…

Q: 4. Give the products from the following acid-base reactions and identify the acid and base on the…

A: The given reactions are represented as follows:

Q: Calculate the pH of a 0.0712 M aqueous solution of piperidine (C5H₁1N, Kµ = 1.3×10-³). pH =

A: pH can be defined as the negative logarithm of hydrogen ion concentration. It can be given as…

Q: 4) In which of the following equations does HSO4 act as an acid? a. HSO4 + H20 H2SO4 + OH b. HSO4 +…

Q: I need help with number 9

Q: Ascorbic acid (vitamin C) is a diprotic acid, H₂CH₂O6. Calculate [H*], pH, and [C₂H₂O6²-] in a 0.34…

Q: 8. Fill in the following table: PH A 1.97 В с D E 8.49 [H301+] 9.84 х 10-² м POH 4.68 [OH11 2.64 x…

A: pH : it can define have the negative logarithm of H+ ion concentration. When pH > 7 solution is…

Q: What is the conjugate base in the following reaction: HCI (aq) + H₂O (1) CI (aq) + H3O+ (aq)? O a)…

A: Given -> HCl(aq) + H2O(l) <-----> Cl-(aq) + H3O+(aq) -> Conjugate acid is formed when…

Q: Which base is stronger, pKb = 3 or pKb = 4?

A: The greater the value of Kb, the stronger the base. The smaller the value of pKb, the stronger the…

Q: Consider the reaction HOCI + F- HF + OCI". Given that K, for HOCI is 3.0 × 10-8 and the K, for HF is…

A: HOCl + F- <......> HF + OCl- Value of Ka tells the acidic strength of an acid.

Q: Chloroacetic acid, CICH₂COOH, has a pK, of 2.87. What are [H3O+], pH, [CICH₂COO-], and [CICH₂COOH]…

Q: 10. Arrange the following acid from weakest to strongest: CH:COОH (Кь %3D 5.56 х 10-10) HNO2 (Kb =…

A: Given data: The basic dissociation constant of CH3COOH Kb=5.56×10-10. The basic dissociation…

Q: Ascorbic acid, H2C6H6O6, is a weak diprotic acid (Ka1 = 9.1 x 10-5, Ka2 = 5.0 x 10-12). In a 0.10M…

Q: Decide whether solutions of the ammonium fluoride are acidic, neutral, or basic. a. K for NH3 is 1.8…

A: Kb and Ka are dissociation constants of base and acid respectively . Greater is the dissociation…

Q: O Find out the Lewis acid and Lewis base in the following reaction. H + H-N-H NH3

A: The reaction given is,

Q: What is the conjugate acid of the Brønsted-Lowry base, C,H¸NH,?

Q: Consider an acid HA dissolved in water at 25°C. HA(aq) + H2O(l) ⇌ H3O+(aq) + A-(aq) Ka =…

A: An acid is a substance that gives H+ ions in its solution whereas a basic substance gives OH- ions…

Q: Constituents DOUBLE INDIC ATOR METHOD Na,CO3 NaHCO3 Vo»ph = Vph»m.o. Vo-ph =0; Vph-m.o>0 Vo-ph >0;…

A: The ions carbonate, bicarbonate, and hydroxide found in the solution are represented as CO32-,…

Q: 1. What is the conjugate acid for the following? а. НРО3 -2 b. HCO31 с. ОН О^-2 d. 04 e. S03-2

A: To solve this problem we will use the Bronstead-Lowry acid-base theory

Q: Calculate the [H+] and pH of a 2.93x 10- 4 M hydrazoic acid solution. The Ka of hydrazoic acid is…

A: Answer:Ostlwald's dilution law is applicable for the dilute solutions of weak electrolytes and it…

Q: A 0.1000 M of 1-naphthoic acid solution has a pH of 2.35. What is the Ka of 1-naphthoic acid?

A: Given information, [1-naphthoic acid] = 0.1000 M pH = 2.35 Find Ka = ? Molecular formula of…

Q: Identify the acid and base in the following reaction: HNO2 + KOH H2O+ KNO2

A: Given :- HNO2 + KOH → H2O + KNO2 To identify :- Acid and base in given reaction

Q: Question 16 Calculate the pH of a formic acid (HCO2H) solution if the concentration of formic acid…

A: Buffer solution is a solution whose pH remains constant and it does not change even on addition of…

Q: Using the following acids and Ką values: HCIO4 1x107 1.76 x 10-5 What is the order of increasing…

Q: Q20 Given: K₁ of HF = 6.8 x 10-4 Ka of NH4+ = 6.3 × 10-10 Ka of HCN = 4.9 × 10-10 According to the…

A: The question addresses the determination of which salt, when dissolved in a 0.10 M solution, would…

Q: Rainwater with a pH = 3 contains 1 and is 2 times more acidic than pH 7. a) 1-carbonic acid; 2-4…

A: we have, pH = -log[H3O+], [H3O+] = 10-pH If pH = 3, then [H3O+] = 10-³ If pH = 7, then [H3O+] = 10-⁷…

Q: What is [OH-] of a solution consisting of 1.05 M NH3 and 0.98 M NH4NO3?

Q: butanoic acid is a weak monobasic acid Ka = 6.3 × 10-⁵. a) Calculate the mass of butanoic acid…

A: The question is based on the concept of solutions and chemical equilibrium. we have to calculate pH…

Q: Which solution has the highest concentration of H3O+: a 0.50 M solution of acetic acid (CH3CO2H),or…

A: ∝=Degree of Dissociation HA⇌ H+ + A-t=0 C 0 0t=eq…

Question

Part A: Please calculate pKa of formic acid below:

(HCOOH  H+ + HCOO-)

Part B: What is pH of a solution containing 10 mM formic acid?

G°f HCOOH = -372 kJ/mol
G°f HCOO- = -351 kJ/mol
G°f H+ = 0 kJ/mol1

Calculate the pK, of formic acid (HCOOH E> H* + HCOO-).

AG°;HCOOH= -372 kJ/mol
AG°;HCOO- = -351 kJ/mol
AG°;H+ = 0 kJ/mol

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step 3

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Similar questions

Acids and bases have been defined in different ways. Arrhenius defined an acid as a compound that dissolves in water to increase the concentration of H*, and a base as a compound that increases the concentration of OH-. Later, Brønsted and Lowry modified the definition: Acids are proton donors, and bases are proton acceptors. The Brønsted-Lowry definition of acids and bases is represented generically by this reaction, where HA is an acid and B is a base: НА + В — А+ BH- An acid that has lost a proton is that acid's conjugate base (A¯). A base that has accepted a proton is that base's conjugate acid (BH†). For each acid-base reaction, there are two conjugate acid-base pairs. The word conjugate is related to the word conjugal, which means "having to do with marriage." A wife is only a wife to her husband, and a husband is only a husband to his wife. Similarly, a conjugate acid is defined as "conjugate" only in relation to the base from which it is derived, and a conjugate base is so…
13.Which of the following is the weakest acid? Group of answer choices H2SO4 HClO4 H3PO4 H4SiO4 14. Calculate Kb for [A-] if the ionization constant of HA is 3.0 x 10-8. Group of answer choices 3.0 x 10-4 3.3 x 10-6 3.3 x 10-7 3.0 x 10-5
Choose the correct answers from among the alternatives to make the sentence correct: They are powerful bases A) RbOH, Al (OH) 3, CH3NH2 B) RbOH, CH3NH2, NaOH C) RbOH, Al (OH) 3, NaOH D) Al (OH) 3, CH3NH2, NaOH
I need the answer as soon as possible
[H+] [OH-] pH Acid, Base, Neutral [OH] = (1 x 10 -14):1 x 10- %3D pH = (-)log(10^-5) 1 x 10-5 10^-14:(10^-5) [H+] = (1 x 10 -14): (4.5 x 10-3 ) 4.5 x 10-3 [H+] = 2nd log (-)8.7 %3D 8.7 neutral
Decide whether aqueous solutions are acidic, basic or neutral. Ka Zn(H2O)62+ = 1x10-9Kb HCOO- = 5.6x10-11 KCl NaF Zn(NO3)2 NH4NO3 KNO3 Al(NO3)2 Zn(HCOO)2 Which acid is stronger: HF (Ka=6.4x10-4) or NH4+(Kb for NH3 is 1.8x10-5)?
The [OH1-] with a pH of 5 is Group of answer choices 1 x 10-5 M 1 x 10-7 M 1 x 10-9 M 1 x 10-10 M
Thank you!
Weak acids are not equally weak! Rank the following acids fromstrongest to weakes. For theacids in problem #14, please calculate the pKa of each of them. What pattern do you see between strengthand pKa? HCN Ka = 6.2x10-10 HCOOH Ka = 1.8x10-4 H2CO3 Ka = 4.5x10-7
Oxalic acid (HOOC-COOH) is the simplest diprotic carboxylic acid. Its commercial uses include bleaching straw and leather and removing rust and ink stains. Calculate the equilibrium values of [H2C2O4], [HC2O4- ], and [C2O42- ], and find the pH of a 0.150M H2C2O4 solution using Ka values from appendix C in your textbook.
#2
1 A triprotic acid (H3A) has p?a values of 3.653.65 (p?a1), 6.396.39 (p?a2), and 9.139.13 (p?a3).