Formic acid, HCHO2, is used to make methyl formate (a fumigant for dried fruit) and ethyl formate (an artificial rum flavor). What is the pH of a 0.30 M solution of formic acid? What is the degree of ionization of HCHO, in this solution? K.(HCHO2) = 1.7 x.10-4 pH = Degree of ionization =

Formic acid, HCHO2, is used to make methyl formate (a fumigant for dried fruit) and ethyl formate (an artificial rum flavor). What is the pH of a 0.30 M solution of formic acid? What is the degree of ionization of HCHO, in this solution? K.(HCHO2) = 1.7 x.10-4 pH = Degree of ionization =

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: Determine the H3O+ of a .230 M solution of formic acid. (Ka for formic acid 1.8•10^-4) Determine the…

A: Given that: initial concentration of formic acid = 0.230 M Ka for formic acid= 1.8×10-4 To find:…

Q: 0.85 g of hydrogen chloride (HCI) is dissolved in water to make 7.5 L of solution. What is the pH of…

Q: vingegar is 5.0% (w/v) solution of acetic (CH3COOH) in water, Acetic Acid's molar mass is 60.032g/…

A: We must convert the specified weight/volume percentage concentration to molarity in order to obtain…

Q: What is the molar concentration of H3O+ in an aqueous solution with a concentration of OH- that…

A: We have to calculate the molar concentration of H3O+ in an aqueous solution with a concentration of…

Q: The Kb of C6H5NH3+ is 3.98x10-10 What is its Ka? What is the [H3O+] concentration in a solution…

Q: ..A 1.68 M solution of a weak acid HA is found to have a pH of 2.09. Determine K, of the acid…

Q: Allylamine, C3H5NH2, is a weak base. A 0.46 M aqueous solution of allylamine has a pH of 12.10. What…

Q: Consider the following data on some weak acids and weak bases: name acetic acid hydrofluoric acid…

Q: Consider the following data on some weak acids and weak bases: formula hypochlorous acid HCIO…

A: The question is based on the concept of salt hydrolysis.We need to arrange the given salts…

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: Ascorbic acid (vitamin C) is a diprotic acid, H₂C6H6O6. Calculate [H*], pH, and [C6H6062] in a 0.45…

A: Given, Molarity of ascorbic acid [H2C6H6O6] = 0.45 M Note : acid dissociation constants of ascorbic…

Q: Consider 0.50 M HC₂H3O₂ (K₂ = 1.8 × 10-5). What are the major species in the solution? HC₂H302 H₂O

A: Where given compound HC2H3O2 is a weak acid and it's name is acetic acid It is an organic acid ,…

Q: What is the pOH of the solution in Part B? Express the pOH numerically to two decimal places. VD…

Q: Determine the [OH−] , pH, and pOH of a solution with a [H+] of 6.0×10−5 M at 25 °C. Determine the…

A: pH, pOH are related through the below formulas: pH + pOH = 14 (or) pH = 14 - pOH (or) pOH = 14 - pH…

Q: Constants I Periodic Tabl typical aspirin tablet contains 324 mg of aspirin mcetylsalicylic acid, C,…

A: From given data mass of aspirin = 324 mg = 0.324 g Ka = 3.0 ×10-4 Volume = 350 mL = 0.350 L Also,…

Q: Calculate the [OH-] of each of the following solutions at 25°C. Identify each solution as neutral,…

A: It is based on the concept of Arrhenius theory of acid and base. Here we are required to find the…

Q: Determine the [OH−] , pH, and pOH of a solution with a [H+] of 1.5×10−8 M at 25 °C. Determine the…

A: To solve these problems, we can use the equations relating pH, pOH, [H+], and [OH-] in water For a…

Q: Ethanolamine, HOC₂H4NH₂, is a viscous liquid with an ammonia-like odor; it is used to remove…

A: Answer is given below in two part

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: To calctulate the pH, we would use Ka or Kb expression. “Since you have posted multiple questions,…

Q: A solution is prepared by adding 49.7 mL concentrated hydrochloric acid and 19.1 mL concentrated…

A: Given: The volume of concentrated hydrochloric acid (HCl) is 49.7 mL The volume of concentrated…

Q: Formic acid, HCHO2, is used to make methyl formate (a fumigant for dried fruit) and ethyl formate…

A: The ICE table for the dissociation of formic acid into formate ions and hydrogen ion can be drawn as…

Q: Consider a solution with a concentration of H3O+ of 10-3 M. What is the concentration of OH- in…

A: concentration of solution is defined as moles of solute dissolved in per l volume of solution

Q: What is the hydroxide ion, pH, and pOH of a solution with a hydrogen ion concentration of 3.25 x…

A: Given: [H+] = 3.25 x 10-3 M Kw = 10-14 Since [H+] < 10-7 M so solution is acidic in nature.…

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

A: Given,The solutions: Solution pH 0.1 M KCl…

Q: Determine the pH of an HF solution of each of the following concentrations. In which cases can you…

A: We need to calculate pH of HF. 1) 0.240 M 2) 0.0530 M 3) 0.0300 M

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: Consider the following data on some weak acids and weak bases: name hydrofluoric acid acid acetic…

A: The question is based on the concept of pH of the solution.It is defined as a negative logarithm of…

Q: Calculate the [OH-] and [H+] for a 0.065 M Ba(OH)2 solution. Is the solution basic, acidic or…

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

Q: solution with [H+]= 1 x 10-3 M has pH . Is this solution an acid, base, or neutral? A…

A: Given-> [H+] = 1× 10-3 pH =-log[H+] = -log(1× 10-3) = -log10-3 = 3log 10 = 3 pH =3<7 =>…

Q: a. Calculate the pH corresponding to the hydrogen ion concentration given below. [H+] = 0.00576 M pH…

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: Calculate the pH of a formic acid solution that contains 1.42% formic acid by mass. (Assume a…

A: Molarity of formic acid, C = moles of solutevolume of solution = 1.42 x 1.01 x 100046 x 100 = 0.312…

Q: Consider the following data on some weak acids and weak bases: K name formula acetic acid HCH,CO₂…

A: The question is based on the concept of salt hydrolysis .we need to arrange the given salts in…

Q: Tartaric acid (H₂C4H4O6) is found in many fruits, including grapes, and is partially responsible for…

Q: Question Aniline, C6H5NH2, is a very weak organic base that is used in the production of…

Q: der the following data on some weak acids and weak bases: name acetic acid acid hydrofluoric acid…

A: Given data :

Q: A solution of methylamine (CH³NH₂), a weak base, has an initial concentration of 0.477 M.…

Q: Which pair of chemical species is NOT a conjugate acid-base pair? A) H,CO3 and CO, В) ОН аnd H,О C)…

A: Hi, Since you have posted multiple questions, we will solve first only. If you want the answer for…

Q: The pH of a solution is 8.75. What is its [OH-]?

A: The relationship between pH and pOH is given by: pH + pOH = 14

Q: Determine the [OH-]. pH, and pOH of a solution with a [H*] of 0.014 M at 25 °C. [OH-] = M pH = POH =…

A: At 25∘C, Kw = OH-H+ = 1 × 10-14 pH = -logH+ pOH = -logOH-…

Q: What is the pH of a bleach solution that has a [OH-] = 6.0 x 10-6 M? pH Incorrect Is bleach acidic,…

A: The pH of the solution shows that the solution is acidic, neutral or basic. If the pH is less than…

Q: Consider the following data on some weak acids and weak bases: acid name hydrofluoric acid nitrous…

Q: Find the concentration of hydroxide, OH-, ions in a 0.100 M solution of HOAc, acetic acid

Q: 5. a. Determine the hydrogen ion concentration, [H*] for a solution with a pH of 3.42. Is this…

Q: The ?a value for acetic acid, CH3COOH(aq), is 1.8×10−5. Calculate the pH of a 2.40 M acetic acid…

Q: Consider the following data on some weak acids and weak bases: name hydrofluoric acid acid acetic…

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

Formic acid, HCHO,, is used to make methyl formate (a fumigant for dried fruit) and ethyl formate (an artificial rum flavor). What is the pH of a 0.30 M solution of
formic acid? What is the degree of ionization of HCHO, in this solution?
K.(HCHO2) = 1.7 x.104
pH =
%3D
Degree
of ionization =

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

VIEW

Step 2

VIEW

Step by step

Solved in 2 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

A solution is 0.705 M HNO2. What is the concentration of HNO2molecules and H3O+ ions molecules in this solution? What is the concentration of OH- and pH of this solution? What is the % ionization?
Formic acid, HCHO2, is used to make methyl formate (a fumigant for dried fruit) and ethyl formate (an artificial rum flavor). See the table for Ka. What is the pH of a 0.14 M solution of formic acid? What is the degree of ionization of HCHO2 in this solution?
What are the concentrations of hydrogen ion and hydroxide ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50? What is the concentration of hydroxide ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50? M OH- What is the concentration of hydrogen ion in household ammonia, an aqueous solution of NH3 that has a pH of 11.50? M H+
Consider the following data on some weak acids and weak bases: acid formula hypochlorous acid HCIO hydrofluoric acid HF name solution 0.1 M NaF 0.1 M CH3NHCI 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. 0.1 M KBr 0.1 M HONH3Br Explanation 1 Check K₁ 3.0 × 108 6.8×104 I W S choose one PH choose one X 2 choose one choose one E 5 4 КЫ formula -9 pyridine C₂H₂N 1.7x109 hydroxylamine HONH₂ 1.1 x 108 C base name R *** F 5 T 80 6 I B © 2023 McGraw Hill LLC. All Rights Reserved. M Terms of Use | Privacy Center | Accessibility L
Suppose 5.00 g of propanoic acid (HC3H5O2) is dissolved in enough water to yield 100.0 mL of solution. For lactic acid, Ka = 1.3 x 10^-5. (a) Calculate the % dissociation, [H+], and pH for this solution. (b) Suppose 100.0 mL of water is added to this solution in (a). Calculate the % dissociation, [H+], and pH.
For the diprotic weak acid H2A, ?a1 = 2.3×10−6 and ?a2 = 6.8×10−9. What is the pH of a 0.0500 M solution of H2A? pH= What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]= M [A2−]= M
Calculate the OH concentration and pH of a 7.7 x 10-³ M aqueous solution of sodium cyanide, NaCN. Finally, calculate the CN concentration. ( K₂ (HCN) = 4.9 × 10-¹⁰) [OH-] M pH = [CN] = 3
Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid at 25°C. The acid is followed by its K, value. HF, 3.5 x 104 O HNO₂, 4.6 x 10 O HCN, 4.9 x 10-10 O HCHO, 1.8 x 104 O HCO₂, 1.1 x 10-²
For the diprotic weak acid H2A, ?a1=3.6×10−6 and ?a2=8.5×10−9. What is the pH of a 0.0800 M solution of H2A? pH= What are the equilibrium concentrations of H2A and A2− in this solution? [H2A]= M [A2−]=[A2−]=
The hydroxide ion concentration, [OH-], of an aqueous solution of 0.406 M ammonia is ______ M. The pH of an aqueous solution of 0.595 M dimethylamine (a weak base with the formula (CH3)2NH) is _________.
What is the hydrogen ion concentration, pH, and pOH of a solution with a hydroxide ion concentration of 1.23 x 10-6 M? Is the solution acidic or basic?
A solution is prepared by adding 51.0 mL concentrated hydrochloric acid and 19.9 mL concentrated nitric acid to 300 mL water. More water is added until the final volume is 1.00 L. Calculate H+], [OH ], and the pH for this solution. [Hint: Concentrated HCl is 38% HCI (by mass) and has a density of 1.19 g/ mL; concentrated HNO3 is 70.% HNO3 (by mass) and has a density of 1.42 g/ mL.] [H] = M [OH ]= pH =