Aniline, C₆H₅NH₂, is a weak base with \( K_b = 3.8 \times 10^{-10} \).What is the pH of 0.750 M anilinium chloride (a salt), C₆H₅NH₃Cl?Express your answer in decimal notation rounded to three significant figures.

Anilinium chloride is a salt made from strong acid HCl and weak base aniline. So, solution of…

Aniline, C6H5NH2, is a weak base with K, = 3.8 x 10-10. What is the pH of 0.750 M anilinium chloride ( a salt), C6H5NH3CI? Express your answer in decimal notation rounded to three significant figures.

Aniline, C6H5NH2, is a weak base with K, = 3.8 x 10-10. What is the pH of 0.750 M anilinium chloride ( a salt), C6H5NH3CI? Express your answer in decimal notation rounded to three significant figures.

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: KOH(aq) is classified as a + base. The reaction equation with water would utilize which of the…

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: Find the PH of 0.20 M solution of sodium propionate (C5H5OONa) ,where the Ka of propionic acid= 1.34…

A: The objective of the question is to calculate the pH of a 0.20 M solution of sodium propionate.…

Q: Acid Ка Base Kb hypochlorous acid, HCIO 4.0 x 10°8 methylamine, CH3NH2 5.0 x 104 hydrofluoric acid,…

A: pH of different solution can be calculated using respective formulas.

Q: Determine the pH of a 0.20 M solution of weak base pyridine C5H5N.Kb=1.7×10−9.

A: PH is defined as power of hydrogen,it is calculated as negative logarithmic value of hydrogen ion…

Q: The base protonation constant K, of allantoin (C,H,N,O,NH,) is 9.12 x 10. Calculate the pH of a 1.3…

A: Reaction: C4H4N3O3NH2 + H2O ⇌ C4H4N3O3NH3+ + OH- Kb of allantoin = 9.12×10-6 Concentration = 1.3…

Q: A diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.23 M solution…

A: The PH of diprotic acid can be calculated as follows

Q: Indicate acids and bases 1) HCl(aq)= H+(Aq) + Cl- (aq) -I know HCl would be an acid, so would that…

A: This is acid base reaction.

Q: What is the pH of a solution prepared by adding 0.0 mL of 1.51 M nitric acid (HNO3) to 165.0 mL of…

A: The Kb for dimethylamine is 5.4×10−4 x 0.150x^2= 8.1 x 10^-5find the square root = 9.0 x 10^-3the…

Q: What is the pH of a solution of 0.79 M acid and 0.55 M of its conjugate base if the ionization…

Q: The pH of an aqueous solution of 0.477 M benzoic acid , C6H5COOH is

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: The acid dissociation K of propionic acid (C₂H₂CO₂H) is 1.3 × 105. Calculate the pH of a 2.2 x 10 M…

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: The pH of 0.65 M aqueous solution of a weak base (monoprotic) is 10.24. Determine the pKb of this…

Q: Calculate the pH and percent ionization of a 0.730 M HNO₂ solution. Note: Reference the K of acids…

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

Q: The acid dissociation constant K of acetic acid (HCH₂CO₂) is 1.8 × 10°. a Calculate the pH of a…

Q: What molar concentration of hydrazine, N2H4 (Kb = 1.7 x 10^-6) yields a solution with a pH of10.46?

A: The objective of this question is to find the molar concentration of hydrazine, N2H4 that yields a…

Q: A diprotic acid (H₂A) has Kal = 4.12 × 10-7 and K₂2 = 5.14 x 10-¹¹. What is the pH of a 0.332 M H₂A…

A: A diprotic is the one which is capable of donating 2 H+ ions in aqueous solution .

Q: |Calculate the pH of a 18 M NH,Cl(aq) (ammonium chloride salt of ammonia) at 25°C. The base…

A: The given chemical reaction is: NH4+aq + H2Ol ⇔ NH3aq + H3O+aq The given information is: Conc. of…

Q: The acid dissociation constant Kof alloxanic acid (HCH³N₂O²) is 2.24 × 10 Calculate the pH of a 4.0M…

A: The concentration of = 4.0 MThe dissociation constant for acid = pH of the solution = ?

Q: A solution of hydrofluoric acid, HF, has a pH of 2.20. Calculate the initial molarity of HF, whose…

A: pH of the solution = 2.20 Ka of HF = 7.2 × 10-4 Initial molarity of HF (C) = ? Note: HF is a weak…

Q: Calculate the pH of pure water

A: Given :- Kw = 2.4 × 10-14 To calculate :- pH of pure water at 37°C

Q: Determine the pH of a 0.62 M NH,NO3 solution at 25°C. The K, for NH3 is 1.8 x 10-5. Express your…

Q: The Ka of a weak acid is 3.33 x 10-5, what is the pKb of it's conjugate base?

A: The objective of this question is to calculate the pKb of the conjugate base of a weak acid given…

Q: The base protonation constant K₁ of lidocaine (C14H21 NONH) is 1.15 × 10 Calculate the pH of a 0.88…

A: Step 1: The base lidocaine (C14H21NONH) is a weak base, which is obvious from its small value of the…

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

Q: Ka for acetic acid, CH3COOH, is 1.80x105. Ką for benzoic acid, CgH3COOH, is 6.30×105. Ka for…

A: Acid dissociation constant: Ka, CH3COOH is 1.8 * 10-5 Ka, C6H5COOH is 6.3 * 10-5 Ka, HClO is 3.5*…

Q: Determine the pH of a 0.20 M solution of CH3NH3Cl at 25 °C. K₁ for CH3NH₂ = 3.7 x 10-4 K₂ for HCI =…

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: The pH of saliva is normally in the range of 6.4 to 7.0. However, when a person is ill, the person's…

A: pH is defined as negative logarithm of hydrogen ion concentration pH= -log[H+] If pH<7 then the…

Q: The pH of a 0.80 M solution of propanoic acid (HC_3H_50_2) is measured to be 2.48. Calculate the…

A: The objective of this question is to calculate the acid dissociation constant of propanoic acid.

Q: Determine the pH of a 1.30 M solution of CH3COOK. Ka(CH3COOH) = 1.8×10-5 Express your answer to

A: 1- First Calculate the OH- ion concentration : CH3COO- + H2O <------> CH3COOH + OH- The…

Q: The acid dissociation constant K, of alloxanic acid (HC H₂N₂O) is 2.24 x 10 Calculate the pH of a…

A: Ka of alloxanic acid HC4H3N2O5 = 2.23×10-7Concentration of alloxanic acid = 3.9 MpH of the solution…

Q: Ką for formic acid, HCOOH, is 1.80×10-4. Ką for acetylsalicylic acid (aspirin), HC,H,04, is…

A: ->conjugate base of strong acid is weak base. ->Ka is proportional to acidity. ->conjugate…

Q: stimate the pH of 0.175 M HCOOH(aq) at 25°C. Ka(HCOOH) = 1.7 × 10−4. Write your answer with two…

A: The acid dissociation constant of HCOOH is .The concentration of HCOOH is .To find the pH of the…

Q: The base protonation constant K,, of allantoin (C H₂N₂O₂NH₂) is 9.12 x 10 Calculate the pH of a 0.25…

Q: a) Write the formula for the conjugate base of HPO, -2 b) Write the formula for the conjugate acid…

Q: Aniline (C6H5NH₂) is an organic base used in the manufacture of dyes. Calculate the pH and the…

A: Given, The concentration of Aniline ( C6H5NH2 ) = 0.15 M. The Kb of aniline = 4.3 × 10-10 M. The…

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

Q: What is the pH of a 0.370 M aqueous solution of methylammonium chloride, CH3NH3Cl? The Kb of methyl…

Q: Hypochlorous acid, HOCI(aq), is a weak acid (Ka = 4.0 x 10-8) used in the chlorination of drinking…

A: a.) To calculate pH , we would draw an ICE table and use its Ka value. b.) Percent ionization is…

Q: The pH of a 1.0M solution of hydrofluoric acid (HF) is measured to be 1.58. Calculate the acid…

A: pH = -log[H3O+] The expression for dissociation constant of weak acid can be determined from ICE…

Q: The pH of a 1.2M solution of acetic acid (HCH₂CO₂) is measured to be 2.33. Calculate the acid…

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

Aniline, C₆H₅NH₂, is a weak base with \( K_b = 3.8 \times 10^{-10} \).

What is the pH of 0.750 M anilinium chloride (a salt), C₆H₅NH₃Cl?

Express your answer in decimal notation rounded to three significant figures.

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

Trending now

This is a popular solution!

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 diprotic acid, H₂A, has Ka1 = 3.4 × 10⁻⁴ and Ka2 = 6.7 × 10⁻⁹. What is the pH of a 0.35 M solution of H₂A?
What is the final pH of a 2.86 M solution of arsenic acid, H3AsO4, where Ka1 = 5.5 x 10^-3, Ka2 = 1.7 x 10^-7, and Ka3 = 5.1 x 10^-12 Give your final solution to two decimal places (i.e. x.xx)
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
pHpH is a logarithmic scale used to indicate the hydrogen ion concentration, [H+], of a solution: pH=−log[H+] Due to the autoionization of water, in any aqueous solution, the hydrogen ion concentration and the hydroxide ion concentration, [OH−], are related to each other by the Kw of water: Kw=[H+][OH−]=1.00×10^−14 where 1.00×10^−14 is the value at approximately 297 K. Based on this relation, the pH and pOH are also related to each other as 14.00=pH+pOH The temperature for each solution is carried out at approximately 297 K where Kw=1.00×10^−14 A. 0.20 g of hydrogen chloride (HCl) is dissolved in water to make 5.5 L of solution. What is the pH of the resulting hydrochloric acid solution? B. 0.20 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 3.0 L of solution. What is the pH of this solution? C. Calculate the concentration of HSO4− ions in a 0.010 M aqueous solution of sulfuric acid.
Ką for acetic acid, CH3COOH, is 1.80×105. Ka for hypochlorous acid, HC10, is 3.50x10-8. Ka for nitrous acid, HNO,, is 4.50x104. What is the formula for the weakest conjugate base?
The pH of a 0.84 M solution of barbituric acid (HC₂H₂N₂O3) is measured to be 2.04. Calculate the acid dissociation constant K of barbituric acid. Be sure your answer has the correct number of significant digits. K = 0 a x10 × Ś
Ka for benzoic acid, C6 H; COOH, is 6.30 × 10-5. Ka for phenol (a weak acid), C6H5 OH, is 1.00 × 10¬10. Ka for formic acid, HCOOH, is 1.80 x 10-4. What is the formula for the strongest acid? Drag and drop your selection from the following list to complete the answer: C6 H; OH C,H; COOH HCOOH
Ka for formic acid , HCOOH , is 1.80×10-4 . Ka for nitrous acid , HNO2 , is 4.00×10-4 .Ka for phenol (a weak acid) , C6H5OH , is1.60×10-10 .What is the formula for the weakest conjugate base? Ka for acetic acid , CH3COOH , is 1.80×10-5 Ka for nitrous acid , HNO2 , is 4.00×10-4 Ka for hypochlorous acid , HClO , is 3.50×10-8 What is the formula for the strongest acid?
Determine the pH of each of the following solutions. 0.19 M CH3NH3I(Kb(CH3NH2)=4.4×10^−4) Express your answer to two decimal places.
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−]=
pH is a logarithmic scale used to indicate the hydrogen lon concentration, [H], of a solution: pH = -log[H] Due to the autoionization of water, in any aqueous solution the hydrogen lon concentration and the hydroxide ion concentration, (OH], are related to each other by the K of water K.-HOH -1.00 x 10-¹4 where 1.00 x 104 is the value at approximately 297 K Based on this relation, the pH and pOH are also related to each other as 14.00 pH + POH The temperature for each solution is camned out at approximately 297 K Part A ▸ 0.55 g of hydrogen chloride (HCT) is dissolved in water to make 55L of solution. What is the pll of the resulting hydrochionc acid solution? Express the pH numerically to two decimal places. View Available Hint(s) 10 ΑΣΦ pH-2.42 Submit Previous Answer X Incorrect; Try Again; 2 attempts remaining Part B pH- K.-1.00×10 0.55 g of sodium hydroxide (NaOH) pellets are dissolved in water to make 5.5 L of soution What is the pill of thon? Express the pH numerically to two…
An environmental technician collects a sample of rainwater.Back in the lab, her pH meter isn’t working, so she uses indicatorsolutions to estimate the pH. A piece of litmus paper turns red,indicating acidity, so she divides the sample into thirds and ob-tains the following results: thymol blue turns yellow; bromphe-nol blue turns green; and methyl red turns red. Estimate the pHof the rainwater.