Answered: What is the concentration needed of…

What is the concentration needed of hypochlorous acid (a weak organic acid) needed to reach a pH of 4.75? The Ka of hypochlorous acid is 2.9*10-8.

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.101EP

See similar textbooks

Related questions

Q: Consider the following data on some weak acids and weak bases: acid base K. Kb name formula name…

A: The question is based on the concept of salt hydrolysis. by observing the hydrolysis of salts, we…

Q: Which of the following statements is correct? In a neutral solution always pH = 7 In a neutral…

A: Given options,

Q: Consider the following data on some weak acids and weak bases: acid base K K₂ name formula name…

A: Here, we have to rank the given solutions in order of increasing pH.

Q: H*, OH-, and pOH of a solution with a pH of 1.79 at 25 °C. Enter numeric value [H*] = M [OH-] = M…

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

Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid…

A: The pH is used to determine the alkalinity or acidity of a solution. The pH is given as the negative…

Q: The Ka of propanoic acid (C2H5COOH) is 1.34×10-5. Calculate the pH of the solution and the…

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

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

Q: The pH of a 0.89M solution of 3-hydroxypropanoic acid (HC₂H5O₂) is measured to be 2.28. Calculate…

Q: Calculate the pH of 9.3×10−2 M propionic acid (C2H5COOH). Ka= 1.3x10-5

Q: Calculate the pH of a solution that is prepared by diluting 0.140 moles of sodium benzoate to 1.00…

Q: A solution that has a hydrogen ion concentration equal to 9.61 x 10-7 has a pH =

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

A: Answer:

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

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: acid base K. K3 name formula name…

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

Q: Calculate the pH of a 0.0159 M aqueous solution of formic acid (HCOOH, Ka 4). = 1.8×10

Q: Calculate the pH for a 0.0183 M pyrophosphoric acid solution (H4P2O7). Pyrophosphoric acid has…

A: Pyrophosphoric acid has three dissociable protons. The dissociation reactions are as follows:…

Q: Calculate the pH of a solution that is prepared by diluting 0.140 moles of sodium benzoate to 1.00…

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

Q: The base protonation constant K₁ of lidocaine (C₁4H₂₁NONH) is 1.15 × 10¯⁹. 14 Calculate the pH of a…

A: The concentration of the lidocaine solution = 1.4 MThe base protonation constant of lidocaine = We…

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

A: The objective of the question is to classify the solutions in order of increasing pH.

Q: What is the pH of a solution that is 0.31 M in ethylammonium chloride? The Kb(ethylamine) = 4.3…

A: Answer:When salt of weak base and strong acid is added in water it gets hydrolyzed to produce H3O+…

Q: Calculate the pH and concentrations of CH₂NH₂ and CH3NH in a 0.0443 M methylamine (CH3NH₂) solution.…

A: Answer:When weak base is added in water, its partial ionization takes place and an equilibrium…

Q: The pH of a 1.1M solution of propanoic acid (HC,H,0,) is measured to be 2.41. Calculate the acid…

Q: Calculate the [H+] for: (a) black coffee with a pH of 4.88 (Enter your answer as follows: 1.0E-2…

Q: Morphine, C17H19NO3, is a weak base. An 0.150 M solution of morphine has a pH of 10.5. What is the…

A: Morphine, C17H19NO3 is a weak base. The concentration of morphine = 0.150 M pH of morphine = 10.5…

Q: The pKa of formic acid (HCO2H) is 3.75. What is the pH of a solution of 0.2 M formic acid?

A: The pKa for the formic acid is = 3.75 The concentration of the formic acid solution is = 0.2 M The…

Q: If 10.0 mL of glacial acetic acid (pure HC2₂H3O2; K₁ = 1.8 x 10-5) is diluted to 1.35 L with water,…

A: We have to calculate the pH of the solution

Q: Consider the following data on some weak acids and weak bases: name nitrous acid acid -10…

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

Q: acid base K K₂b name formula name formula 10 nitrous acid HNO₂ 4.5 x 10 aniline |C HạNH, | 4.3 × 10…

A: Ka value of acetic acid = 1.8×10-5 Ka value of HNO2 = 4.5×10-4 Kb value of aniline = 4.3×10-10…

Q: Write the conjugate base of each acid in HNO2, Ka = 4.6 x 10-4; HClO2, Ka = 1.1 x 10-2; HCN, Ka…

A: If an acid lose one proton, then the formed species is a conjugated base.

Q: 2-12 If 200 mg of HCI is added to water to achieve a final volume of 1.00 L, what is the final pH?

Q: -10. What is the pH of a 0.70 M potassium cyanide (KCN) solution at 25°C? (hydrocyanic acid, HCN, K₂…

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

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

100%

What is the concentration needed of hypochlorous acid (a weak organic acid) needed to reach a pH of 4.75?

The Ka of hypochlorous acid is 2.9*10-8.

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 1 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

The pH of a 0.10-M solution of propanoic acid, CH3CH2COOH, a weak organic acid, is measured at equilibrium and found to be 2.93 at 25 °C. Calculate the Ka of propanoic acid.
Classify each of the acids in Problem 10-20 as a strong acid or a weak acid. a. H2SO4 (sulfuric acid) b. HC2H3O2 (acetic acid) c. H2C5H6O4 (glutaric acid) d. HCN (cyanic acid)
Two strategies are also followed when solving for the pH of a base in water. What is the strategy for calculating the pH of a strong base in water? List the strong bases mentioned in the text that should be committed to memory. Why is calculating the pH of Ca(OH)2 solutions a little more difficult than calculating the pH of NaOH solutions? Most bases are weak bases. The presence of what element most commonly results in basic properties for an organic compound? What is present on this element in compounds that allows it to accept a proton? Table 13-3 and Appendix 5 of the text list Kb values for some weak bases. What strategy is used to solve for the pH of a weak base in water? What assumptions are made when solving for the pH of weak base solutions? If the 5% rule fails, how do you calculate the pH of a weak base in water?
Classify each of the acids in Problem 10-19 as a strong acid or a weak acid. a. HClO3 (chloric acid) b. HC3H5O4 (glyceric acid) c. H3C6H5O7 (citric acid) d. H3PO4 (phosphoric acid)
8-17 For each of the following, tell whether the base is strong or weak. (a) NaOH (b) Sodium acetate (c) KOH (d) Ammonia (e) Water
Without writing an equation, specify the molecular ratio in which each of the following acidbase pairs will react. a. HCl and KOH b. H2CO3 and KOH c. HCl and Ca(OH)2 d. H2CO3 and Ca(OH)2
Without writing an equation, specify the molecular ratio in which each of the following acidbase pairs will react. a. HNO3 and NaOH b. H2SO4 and NaOH c. H2SO4 and Ba(OH)2 d. HNO3 and Ba(OH)2
8-15 Write an equation for the reaction that takes place when each base is added to water. (a) LiOH (b) (CH3)2NH (c) Sr(OH)2 (d) CH3CH2NH2
How is acid strength related to the value of Ka? What is the difference between strong acids and weak acids (see Table 13-1)? As the strength of an acid increases, what happens to the strength of the conjugate base? How is base strength related to the value of Kb? As the strength of a base increases, what happens to the strength of the conjugate acid?
Consider the following four solutions: (1) apple juice, pH 3.8, (2) pickle juice, pH 3.5, (3) carbonated beverage, pH 3.0, and (4) drinking water, pH 7.2. a. Which solution has the highest [H3O+]? b. Which solution has the highest [OH]? c. List the solutions in order of increasing acidity. d. List the solutions in order of decreasing basicity.
In each of the following acid-base reactions, identify the Brnsted acid and base on the left and their conjugate partners on the right. (a) HCO2H(aq) + H2O() HCO2(aq) + H3O+(aq) (b) NH3(aq) + H2S(aq) NH4+(aq) + HS(aq) (c) HSO4(aq) + OH(aq) SO42(aq) + H2O+()
8-111 The volume of an adult's stomach ranges from 50 mL when empty to 1 L when full. On a certain day, its volume is 600. mL and its contents have a pH of 2.00. (a) Determine the number of moles of present. (Chapter 4) (b) Assuming that all the H+ is due to HCl(aq), how many grams of sodium hydrogen carbonate, NaHCO3, will completely neutralize the stomach acid? (Chapter 4)