Calculate the (Ka) value for the reaction of CH3COOH with NH3 that the pHof the solution is (6.46) and the (Kb = 1.75 x 10 5).

The Ka for the reaction of acetic acid (CH3COOH) is calculated as shown below.…

Answered: Calculate the (Ka) value for the…

Calculate the (Ka) value for the reaction of CH3COOH with NHạ that the pH of the solution is (6.46) and the (Kb -1.75 x 10 *).

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter16: Acids And Bases

Section: Chapter Questions

Problem 19QAP: . How is the strength of an acid related to the fact that a competition for protons exists in...

See similar textbooks

Related questions

Q: Basic solution Potassium permanganate, KMnO, is a powertul oxiding agent. The products ot a given…

A: Answer: Unbalanced redox reaction in basic medium is shown below: MnO4-(aq)+F-(aq)→MnO2(s)+F2(aq)

Q: Calculate the pH and % ionization for a .44 molar solution of CN-(aq).

A: Cyanide ion hydrolyzes in water to form HCN and hydroxide ion. The concentration of hydroxide ion…

Q: Which of the following is an acidic salt? O NaBr O KNO3 HI O NH4CI O NACIO

A: Acidic salt : strong acid and weak base combination.

Q: A mixt. weighing ) wt. of NogCOs ond KaCOg It is disasolued in woter and 1.000 g consistu of equal…

A: NOTE : it will be 17.36 mL of 1.075 acid added not 17.36 g Sol : Since the mass of K2CO3 and Na2CO3…

Q: Please Answer my question from the picture im send... And note With same dengan.. God bless you ..…

A: The question is based on the concept of qualitative analysis. We have to distinguish the molecules…

Q: Calculate the pH of a 0.125 M solution of KN3 at 25°C. Ka for HN3 is 2.5 x 10*

A: KN3 is a salt of weak acid HN3 and strong base KOH This salt undergo a anionic salt hydrolysis…

Q: (a) How many grams of H2O2 are contained in a solution that requires for titration 14.05 mL of KMNO4…

A: Answer is as follows, hope it would help

Q: Sodium acetate, CH3COONA was hydrolysed in water, HzO. Show the reaction equations involved. What is…

A: Hydrolysis of reaction of salt of the weak acid with strong acid can be written as, A- (aq) + H2O…

Q: What is valence-state electronegativity? Explain the changein acidity of the oxides of Mn with…

A: The tendency of an atom to attract the pair of electrons which are bonded and its measurement is…

Q: What are the respective concentrations (M) of Fe3+ and I- afforded by dissolving 0.200 mol FeI3 in…

A: Molarity is defined as moles of solute per liter volume of solution. It is represented as M. M=no.…

Q: Using Table 1, rank the following species from the strongest to the weakest agent: I' (aq), Fe(s),…

A: We can use the data present in Table 1 to compare the oxidative and reductive strengths of…

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: What of the following options describes the term "strong acid/base"? O a. A pair of species which…

A: A strong acid or strong base is a strong electrolyte.

Q: Calculate the concentration of sulfide ions in a solution that is 0.050M in hydrogen sulfide and…

Q: The molar concentration of H3O+ was measured at 25 ° C. The pH and pOH should be calculated for the…

Q: Assuming a bicarbonate ion concentration [HCO3-]of 1.00 × 10−3 M and a value of 3.5 × 10−11 for the…

A: The equilibrium composition of a redox system involving H+ depends on both the pH and the pE. The…

Q: HO HOʻ V

A: The ionization of an acid HA can be shown as: HA = H+ + A- So, greater the stability of A-…

Q: Calculate the [H+] and pH of a 1.97 × 10-4 M nitrous acid solution. The K, of nitrous acid is 7.10 x…

A: Given, Concentration of the nitrous acid (HNO2) solution (C) = 1.97 × 10-4 M Ka of nitrous acid…

Q: IFs undergoes autodissociation into IF4 and IF6. SbFs acts as an acid and KF acts as a base when…

A: Autodissociation of IF5 take place into IF4 & IF6. SbF5 is an acid & KF is a base. The…

Q: Which one of the following compounds in aqueous solution would be best described by the picture…

A: The aqueous solution of ionic solids contains all the ions in same proportion as that in formula.

Q: Calculate the Ka of a 0.50 M HC4H7O2 with a pH of 2.56

A: The concept used here is based on the acid dissociation constant of an acid which is used for…

Q: (Calculate the molar (M) concentration of H2S04 solution of 0.250 N, to produce sulphate ion S04^(-2…

A: Given concentration of H2SO4 = 0.250 N where "N" indicated for Normality We know that…

Q: Calculate the AH for the reaction (6 points)

A: Calculate the ∆H for the reaction., NO(g) + O(g) → NO₂(g)

Q: Calculate the PH and the POH FOR a solution that is ISM IN Hellz and .04M IN HALO₂, Heloz K; FOR…

A: HClO3(aq) is a strong acid, whereas HClO2(aq) is a weak acid with Ka = 1.1*10-2 Given [HClO3(aq)] =…

Q: ol, what is AG for the following reaction?

A: The energy associated with a chemical reaction that can be used to do work. The free energy of a…

Q: (a) How many grams of H202 are contained in a solution that requires for titration 14.05 mL of KMNO4…

A: Hii there, As there are multiple question posted. we are answering first question. If you need…

Q: What's the ppting agent of ferric ion and why nitric acid and hydrogen peroxide are added to…

A: The technique by which the ion amount or ions in a specific analyte are determined is called…

Q: When solid CrO3is dissolved in water, the solution is or-ange rather than the yellow of H2CrO4. How…

Q: Estimate the Ph of a .20M solution of CH3COOH with of Ka=1.8x10^-5

Q: The pH for a solution with a [H3O]+ of 1.0 x 10^-6 is

Q: Nitrous acid is a weak acid and has a concentration of 0.65 mol/L. What is the pH of the solution…

Q: A 0.200 M solution of nitrous acid (HNO2) had a pH of 2.07. What is the Ka value for nitrous acid.

A: Nitrous acid is a weak acid.

Q: Calculate the molar concentration of OH- in a 0.724 M solution of hypobromite ion 1BrO-; Kb = 4.0 *…

A: Since the BrO- will get hydrolysed by water as per the reaction => BrO- (aq) + H2O (l)…

Q: A sample of water in contact with solid Fe(OH)3 is found to have a pH of 7 .5. If no other dissolved…

A: To calculate the pOH of the solution, the equation used is: pH + pOH = 14 ........(1) pOH is…

Q: A groundwater contains 2.00 mg/L copper as Cu²*. What concentration (mol/L) of hydroxide is required…

A: Given: Groundwater containing copper ions Cu2+= 2.00 mg/L To Find: Concentration of hydroxide…

Q: An aqueous solution of will produce a neutral solution. O RbBr O NH,CI O LINO2 O NaF O Li2 CO3

A: Salt containing anion of a strong acid and cation of a strong base resulting a neutral solution.…

Q: determine the ph of a buffer solution which contains 0.6 mole of ammonium nitrate and 0.40 mol of…

A: Given: The number of moles of ammonium nitrate and ammonia in the buffer solution is 0.60 mol and…

Q: 3. Hypochlorous acid (HCIO) is a weak acid. A 1.00M aqueous solution of this acid gives has a pH of…

A: Recall the data, Molarity of HClO=1.00 M pH=3.77 pKa of HClO ?

Q: give balance equation showing oxidation of H2S into S.

A: Oxidation is defined as process of addition of oxygen or an electronegative element to the…

Q: For the equilibrium H2O (l) = H2O (g), Aps® = 118.9 J/(mol K) and A,H®= 44.0 kJ/mol. Calculate the…

Q: Calculate the pH of a 0.013 M NaF solution. (Ka for HF = 7.1 × 10−4.)

A: It is required to calculate the pH of 0.013 M NaF solution. This can be done by constructing the ICE…

Q: A buffer solution is 0.318 M in HClO and 0.217 M in KClO . If Ka for HClO is 3.5×10-8 , what is the…

A: pH = pKa + log [salt]/[acid]

Q: One method of de ter minin the concentration of hydrosen poroxide CH 202) ina sdutioh is thrush…

A: Volume of H2O2 = 50 mL = 0.050 L Molarity of KI = Molarity of I- = 0.1500…

Q: The Ka for HF is 7.0 x 10-4 Kb for the fluoride ion is

A: at 25°C Ka x Kb = 10-14 Given that Ka = 7 x 10-4 HF is weak acid and its conjugate base is…

Q: rank the following species from the strongest to the weakest reducing agent: I - 1aq), Fe1s2, Al1s2.

A: A compound or species that can easily lose or donate an electron is called Reducing agent.Smaller…

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

Calculate the (Ka) value for the reaction of CH3COOH with NH3 that the pH
of the solution is (6.46) and the (Kb = 1.75 x 10 5).

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

. How is the strength of an acid related to the fact that a competition for protons exists in aqueous solution between water molecules and the anion of the acid?
. Which component of a buffered solution is capable of combining with an added strong acid? Using your example from Exercise 60, show how this component would react with added HC1.
Potassium hydrogen phthalate is a solid, monoprotic acid frequently used in the laboratory as a primary standard. It has the formula KHC8H4O4. This is often written in the short-hand notation as KHP. If 25.0mL of a potassium hydroxide solution are needed to neutralize 2.26g of KHP, what is the molarity of the potassium hydroxide solution? Potassium hydrogen phthalate sometimes called potassium biphthalate, as shown on this bottle is an acid that is convenient to store and use because it is a solid.
The sec-butyl cation can react as both a Brnsted-Lowry acid (a proton donor) and a Lewis acid (an electron pair acceptor) in the presence of a watersulfuric acid mixture. In each case, however, the product is different. The two reactions are as follows: (a) In which reaction(s) does this cation react as a Lewis acid? In which reaction(s) does it react as a Brnsted-Lowry acid? (b) Write Lewis structures for reactants and products and show by the use of curved arrows how each reaction occurs.
The pH of an aqueous solution of 0.0655 M ammonium bromide, NH4 Br(aq), is (Assume that K₁ (NH3) = 1.80 x 10-5.) This solution is Submit Answer Retry Entire Group 1 more group attempt remaining
(ii) Ph. - COOH
Ule the Keferences to access important values if needed for this yestinn When a 23.2 mL sample of a 0.386 M aqueous hypochlorous acid solution is titrated with a 0.438 M aqueous bariem hydroside solution. (1) What is the pH at the midpoint in the titration? (2) What is the pH at the equivalence point of the titration? (3) What is the pH after 15.3 ml. of barium hydroxide have been added? Submit Answer 2 question attempts remainng
What is the pH of a 0.124 M aqueous solution of sodium nitrite, NaNO₂? This solution is Submit Answe acidic basic neutral pH = Entire Group 9 more group attempts remaining
The hypochlorite ion, ClO-, acts as a weak base. (a) Is ClO-stronger or weaker base than hydroxylamine? (b) WhenClO- acts as a base, which atom, Cl or O, acts as the protonacceptor? (c) Can you use formal charges to rationalize youranswer to part (b)?
The pKa of Cl3CCO2H is 0.64. What is the pH of a 0.580 M solution? What percentage of the Cl3CCO2H is dissociated?
Calculate the pH and the pOH of these solutions: (c) 0.957 M HC2H3O2 (Ka = 1.8 x 10-5) pH = pOH =
The hypochlorite ion, ClO-, acts as a weak base. (a) Is ClOa stronger or weaker base than hydroxylamine? (b) When ClO- acts as a base, which atom, Cl or O, acts as the proton acceptor? (c) Can you use formal charges to rationalize your answer to part (b)?