What are the [H3O*] and pH of 0.085M weak base C2H5NH2?

Q: Which is the stronger acid in each of the following pairs?

A: Acid is a substance which can donate H+ in the solution. (a) The second compound given is the…

Q: What is the pH of a 0.360 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹

A: Given data--> C= 0.360 M solution of C5H5NHBr Kb=1.7*10-9   pkb = - log10(1.7*10-9) pkb= 9 -…

Q: What is the pH of a 0.710 M solution of C5H5NHB (Kb of C5H5N is 1.7 x 10-9)?

A: pH is used to determine the concentration of hydronium ion.

Q: Calculate the pH and concentrations of CH3NH2 and CH3NH+3 in a 0.0341 M methylamine (CH3NH2)…

A: The given data contains, Concentration of methylamine = 0.0341 M. Kb of CH3NH2 is 4.47×10−4.

Q: Write the chemical equation and the Ka expression for theionization of each of the following acids…

A: a)  HBrO2 l → H+ aq +BrO2- aqand writing the Ka expression :Ka=H+ BrO2-HBrO2The reaction to…

Q: What is the pH of a 0.590 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: What is Ka for the conjugate acid of CH₃NH₂ (Kb = 4.4 × 10⁻⁴)?

A: Conjugate acid of any base is formed when the base accepts a proton i.e H+ ion. Hence the conjugate…

Q: The base ethylamine, C2H5NH2 , has a pKb equal to 3.30. Calculate the hydroxide concentration, the…

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Q: The pKa of acetic acid (CH3COOH) is 4.76. If a solution of acetic acid is at a pH of 6.56, the ratio…

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Q: A solution with a pOH of 11.70 has an [H+] of a. 5.0 × 10−3 M.b. 3.2 × 10−4 M.c. 2.0 × 10−12 M. d.…

A: Given data, pOH of the solution =11.70

Q: The conjugate acid of HSO₃⁻ is

A: Given : HSO3-  To determine : conjugate acid of HSO₃⁻

Q: What are the concentrations of H3O+ and OH− in tomatoes that have a pH of 4.06?  [H3O+] = ×10__ M…

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Q: What is the pH of a 0.050M solution of (CH3)3NHC1?

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Q: What is the pH of a solution containing both 0.10 M CH₃COOH and 0.20 M CH₃COONa? The Ka of CH₃COOH…

A: We have to predict the pH of the given solution.

Q: What is the hydronium concentration [H3O+] of a solution with a pOH of 2.47?

A: Given data is as follows: The pOH of the solution = 2.47 As we know that;  pH + pOH =…

Q: If not, which direction does it need to move (right or left) to reach equilibrium? Explain.

A: For the reaction   C6H5NH2(aq)+ H2O (l)------>C6H6NH3+(aq)+OH- Q= reaction coefficient =…

Q: Rank the following substances in order of increasing acid strength. (1 as least and 4 as most in…

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Q: What is the pH of a 0.420 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)

A: Given, Concentration of C₅H₅NHBr = 0.420 M Kb = C₅H₅N is 1.7 × 10⁻⁹   pKb=-[logkb]pKb=-[log 1.7 ×…

Q: What is the pH of a 0.22M NaH2PO4 solution?

A: NaH2PO4 is a weak.Ka for NaH2PO4 is 6.23×10-8.Calculate concentration of H3O+:

Q: 1. Calculate the ratio of CH₂COOH/NaCH₂COO to give a buffer solution at pH 5.

A: given, pH of the buffer solution = 5

Q: Morphine is an effective pain killer but is also highly addictive. Calculate the pH of a 0.115 M…

A: Given, Molarity of morphine solution = 0.115M. pKb = 5.79.

Q: 5. Calculate the pH, % hydrolysis, and [H2SO3] in a 0.250 M solution of K2SO3

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Q: Which one of the following solutions is basic?  a. A solution for which [OH-] = 8.3x10-12  M  b.…

A: We know that, pH is greater than 7, then solution is basic. So,

Q: What is the conjugate base of H2S?

A: After observing this question we can say that, given problem is checking our basic concept of…

Q: Calculate the PH of4.6M formic acid (CHOOH)  solution given a ka value of 1.787*10^-4

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Q: Write the formula of the conjugate acid of CH₃CO₂⁻

A: A chemical compound formed by the reception of a proton by a base is known as a conjugate acid.  In…

Q: Which one of the following will form an acidic solution in water? Select one: O a. KNO3 O b. Lil c.…

A: Whenver an acid and base reacts with each other than they form salt and water and the process is…

Q: What is the pH of a 0.510 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Given information: Concentration of solution = 0.510 M

Q: What is the pH of a solution that is 0.33 M CH3NH2 (methylamine) and 0.52 M CH3NH3Cl (methylammonium…

A: Since we have weak base CH3NH2 and its conjugate acid CH3NH3Cl in the solution. Hence the solution…

Q: Calculate the pH at 25°C of a 0.64M solution of anilinium chloride C6H5NH3Cl. Note that aniline…

A: The pKb of C6H5NH2 is 4.87. The pKa of C6H5NH3+ is calculated using equation (1).

Q: What is the concentration of a solution of Ca1OH22 for which the pH is 11.68?

A: Ca ( OH)2 ------> Ca + 2 OH - pOH = 14 - 11.68 = 2.32 pOH = - log [ OH-] 2.32 = - log [OH-] [OH-]…

Q: What is the pH of a 0.618 M carbonic acid (H2CO3) solution given Ka1=4.4×10−7 and Ka2=4.7×10−11?

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Q: What is the pH of a 0.430 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: pH= 1/2(pKb-logc) Here given Kb=1.7×10-9,hence pKb=-logKb=-log(1.7×10-9) given c=0.430 M

Q: Eメーツ colculate the pH of o-2M a monium. hy droxide solution if pKb=4:7· ニ

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Q: What is [H3O+] of a softdrink that has a pH of 3.400?

A: Given-> pH = 3.400

Q: What is the predominant form of ammonia in a solution at pH 7.0? Approximately what fraction is in…

A: pH of compound is the negative logarithm of its hydrogen ion concentration. The pH  of a compound…

Q: Estimate the pH of 0.0025 M NH(CH3)3Cl(aq) at 25°C. It is given that trimethylamine ((CH3)3N) has a…

A: Given : Concentration of salt = 0.0025M pKb = 4.19

Q: If the [H^ 1+ ] solution at 25°C is 4.9 x 10 ^ - 4 * m * o * l / L , calculate the [O H ^ -1] in * m…

A: The word pH stands for the potency of hydrogen and it is used to measure the concentration of…

Q: How many milliter of 0.200M NaOH will be required to neutralize 75.0mL of 0.215M H2SO4? a.161…

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Q: Calculate [H+], PH and POH respectively of CH3COOH solution has concentration 1.0 x 10-3 M and the…

A: Here i have calculated all the things

Q: Least acidic F Br CI А. "СООН В. COOH COOH "СООН С. "СООH D. COOH

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Q: Which one of the following substances is/are amphoteric? (2) HS-1 (3) PO43- 1-*OSH (1) 2 only 3 only…

A: 1. HSO4-1 : - This compound is  amphoteric meaning that in water it can behave as both a proton…

Q: Which of the following is FALSE ? HBr is a strong acid O C2H5NH2 is a weak base O C2H5COONa is a…

A: The species increases the concentration of hydrogen ion or hydronium in an aqueous solution act as…

Q: Calculate the pH of 0.050 M aqueous solutions of the compounds below at 25 °C: a. NaOH b. CH3NH2…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: Question attached

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Q: Calculate the pH at 25°C of a 0.91 M solution of anilinium chloride (C6H5NH3Cl). Note that aniline…

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Q: Which of the following describes H3PO3? monoprotic diprotic

A: H3PO3 has three hydrogen atoms and when we draw the structure it is clear that in H3PO3 only two…

Q: Calculate the pH of a 0.41 M CH3COONa solution. (Ka for acetic acid = 1.8 ×10−5.)

A: The reaction is written below. CH3COO - + H2O ⇌ CH3COOH - + OH- The ICE table is shown below.

Q: The pH for 0.0850 M solution of C6H5CH2COOH is 2.68. Determine the value of Ka for C6H5CH2COOH.

A: Given pH of C6H5CH2COOH is = 2.68. We Know, pH = - log[H3O+] So, 2.68 = - log[H3O+] Or, log[H3O+] =…

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.