Which of the following dissociates completely (100%) into hydrogen ionsand anions in solution?aka) weak acidO b) strong acid27O c) strong baseongsaltd) weak base19 votes3011:44 AM4/23/2021PrtScInsertDeleteF8F9F10F11F12+BackspaceNumLock%3D89.78HomePgUp%3DKEnterM1Shift3EndPgDnPgUpCtrlInsEnd->4-+ ||1OV

Strong electrolytes are those which dissociates completely i.e. 100% into its ions. Acids are those…

Answered: Which of the following dissociates…

Which of the following dissociates completely (100%) into hydrogen and anions in solution? ak O a) weak acid O b) strong acid 27 O c) strong base ong _ salt d) weak base 19 votes 30 11:44 AM

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter16: Principles Of Chemical Reactivity: The Chemistry Of Acids And Bases

Section16.10: The Lewis Concept Of Acids And Bases

Problem 1RC: 1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot...

See similar textbooks

Related questions

Q: The [ H3O+] of a solution with pH = 5.60 is Group of answer choices 3 × 10-6 M. 2.5 × 10-8 M.…

A: Given, pH = 5.60.

Q: • Calculate the pH of water sample with hydrogen ion concentration of 3.16 * 10-8 mols/L • Calculate…

A: pH = - log [H+]

Q: e. Choose the strongest Lewis acid from among the boron halides BX3, (X = halogen). Explain your…

A: ANSWER IS DISCUSSED BELOW :

Q: 9. If only 1.6% of 0.20 M solution of a weak base was ionized. Calculate its Kb value? *

Q: ave 1 UNSAVED ANSWER - SAVE ALL ANSWERS Question 28 The weak acid HA is 10 % ionized (dissociated)…

Q: The 3-step ionization of phosphoric acid: H3PO4 = H + H2PO4 H2PO4 = H + HPO4² HPO4? = H* + PO4 Kal =…

A: We need to an acid whose pKa is close to 7.0. then we make a solution of the acid and its conjugate…

Q: 6. Which is a property of a base? (Choose all that apply) OCorrode metal O Sour taste Slippery…

A: Bases ca be defined as the substances which are having a bitter taste. Base turns the red litmus…

Q: The concentration of H* (or H3O*) from part A should be 1.02×10-2 mol L-1. What is the percent…

Q: 9. Calculate the pH corresponding to each of the concentrations given below, and indicate whether…

Q: Determine the concentration of CO32- ions in a 0.18 M H2CO3 solution. Carbonic acid is a diprotic…

A: In this question, we want to determine the Concentration of CO32- ion. You can see details Solution…

Q: What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with pH = 4.186? 6.52 -…

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: culate the [OH-]of the solution with pH=10.50 3.2 x 10-10 1.05 x 10-10

A: pH is defined as negative logarithm of hydrogen ions present in solution.

Q: The weak acid HZ has a Ka of 2.55x10-4.(a) Calculate the pH of 0.075 M HZ.(b) Calculate the pOH of…

A: Given: Ka for HZ = 2.55 x 10-4 Since HZ is a weak acid, it will not get dissociated completely into…

Q: Determine the pOH of a 0.188 M NH3 solution at 25°C. The Kb of NH3 is 1.76 × 10-5.

A: The concentration of OH- ions formed at equilibrium can be determined by constructing an ICE table.

Q: Part A Calculate OH in the following aqueous solution at 25 °C: H30*] = 2.2x10-8 M . Express your…

Q: a. Determine the pOH of a 0.119 M CH3NH3Br solution. Kb = 4.4 x 104 b. Determine the pH and OH…

Q: Four so v s of an acid dissolved in water are sketched below, as if under a micoscope so powerful…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: Determine the reaction of the salt in aqueous soln. Write A (if acidic), B (if basic).or C (if…

A: Given Salt is NaClO4 We know that following rule : Salt of [strong acid + strong base] : then…

Q: Concentration of Na2CO3 solution: I00 N Calculated pKa of HCO3: (show calculations) C2. Measured pH:…

A: Since Na2CO3(aq) or CO32-(aq) is a weak base, it undergoes hydrolysis to form HCO3-(aq) and OH-(aq).…

Q: Calculate the hydronium ion concentration in an aqueous solution with a pOH of 4.33 at 25°C. Select…

Q: The pH of an aqueous solution at 25°C was found to be 3.90. The pOH of this solution is The…

A: pH is defined as the negative logarithm of hydrogen or hydronium ion concentration present in the…

Q: Part C Calculate H30*| in the following aqueous solution at 25 ° C: [OH ]= 6.2x10-12 M Express your…

A: This Question contains two parts, in first part we determine the H3O+ ion Concentration and in…

Q: 5. A solution contains 0.0085 M ammonia. What is the pH of this solution? For ammonia: Kb=1.8×105.

Q: 12) Calculate the [H*], pH, and pOH for a 100.00mL of 0.00250M HCl at 25°C. [H*] = pH = pOH = _M %3D

A: Introduction: An acid is a substance that can donate H+ ions. The acidity of the substances is…

Q: the pH of a 0.1 M KNO3 solution

A: Potassium nitrate (KNO3) is a salt of strong acid(nitric acid;HNO3) and strong base(potassium…

Q: concentration of either the hydionium ion or the hydroxide lon is known then the concentration of…

A: we need to determine if the given hydroxide ion concentration is acidic, basic or neutral

Q: MasteringChemistry: CHE154 S X session.masteringchemistry.co This Mac can't connect to iCloud I a…

A: Concentration of OH- formed during the dissolution of NaF in water is determined as follows,

Q: If the pH ofa solution is 3. ОА. 1.23х10 5м о в. 2.24х104м о С. 3.65х10"м D. 4.47x10-11м

A: pH of a solution - It is a measure of hydrogen ion concentration in a solution or can say a measure…

Q: What the %Ionization of an acid with an initial concentration of 0.589M with a pH of 4.31.

A: 0.0141%

Q: Name: Date: Section: Prelaboratory Assignment: pH: Measurement and Application. 1. Calculate [H']…

A: We are given three different pH and we have to find the concentration of H+ and OH- ion. PH =…

Q: Part A Calculate (OH] in the following aqueous solution at 25 °C: [H3O*] = 1.6x10-8 mol - L Express…

A: Answer :- A) [OH-] = 6.7 × 10-7 (mol.L-1) B) The solution is Basic…

Q: <Chapter 16 - Attempt 3 Item 4 Consider two solutons, solution A and solution E H'] in solution Ais…

Q: What is the pOH of a 0.1563 M NH4NO3? Kb for NH3 is 1.86e-5.

A: Given: kb for NH3 = 1.86 * 10-5 concentration of NH4NO3 = 0.1563 M

Q: 13. According to Brönsted and Lowrry an acid and a base are species that behave respectively: A) as…

Q: What mass of HNO, is present in 211.0 mL of a nitric acid solution having a pH = 5.70? 5.96e-5

A: Given data : pH of solution = 5.70 Volume of Solution = 211.0 ml = 0.211 L

Q: Calculate the [OH] in 0.2110 M H3PO4. The stepwise dissociation constants are Ka1 = 7.50e-3 and Ka2…

Q: Question 5 of 5 Submit The pH of a basic solution is 11.65. What is [OH"]? M 1 2 3 4 6. C 7 8 +/- x…

Q: Determine Kb for the formate ion, CHO2−. In a 0.21 M solution, this base is 0.0016% unionized.…

A: Initial concentration = 0.21 M.Unionization = 0.0016% = 0.21× 0.0016/100 = 3.36 × 10-6.

Q: Calculate the percentage of ionize and unionized forms present in the following solution. Assume…

A: Weak acids partially dissociates so there is degree of dissociation alpha.

Q: 1. BF, is a weaker Lewis acid than BClg.

Q: D. Behavior of Salts in Solution Table 12.7 (data) Salt Solution pH Sodium acetate Ammonium chloride…

A: Bronsted acid is proton donor and Bronsted base is proton accceptor.

Q: Solve for the unknown parameters with the information given: Limit to 2 significant [H+]…

Q: Calculate the values of [OH-] , and PH from Kb and [B initial]. Calculate the values of [OH-], POH…

A: NH3 dissociates as: NH3 + H2O ⇋ NH4+ + OH-Initial mol…

Q: was determined that a solution contained a [H+] of 1 x 10-8M. What kind of solution is this?…

A: Given-> [H+] = 1 × 10-8 M

Q: Part A Find the pH of a 0.014 M solution of HCHO₂. (The value of K, for HCHO₂ is 1.8 x 10-4.)…

Q: Chemists use a number denoted by pH to describe quantitatively the acidity or basicity of solutions.…

A: The scale of the pH ranges between 0 to 14. This pH scale indicates the concentration of hydrogen…

Q: Calculate the percent ionization of a 0.313 M solution of hydrofluoric acid. % Ionization Submit…

A: Given that concentration of hydrofluoric aci solution HF = 0.313 M HF is a weak acid and dissociates…

Q: A solution has a [OH1-] = 4.40 x 10-11 M. Use the self ionization constant of water (Kw) to find the…

A: Water decomposes and gives hydroxide ion and hydronium ion and the equilibrium constant for this…

Q: [Review Topics] [References] Use the References to access important values if needed for this…

Q: in 2 liters of water dissolve a piece of sodium and release 2.24 liters of H2 measured under normal…

A: Whenever a sodium metal is dropped into water than being a metal it reacts with water to form base…

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

Which of the following dissociates completely (100%) into hydrogen ions
and anions in solution?
ak
a) weak acid
O b) strong acid
27
O c) strong base
ong
salt
d) weak base
19 votes
30
11:44 AM
4/23/2021
PrtSc
Insert
Delete
F8
F9
F10
F11
F12
+
Backspace
Num
Lock
%3D
8
9.
7
8
Home
PgUp
%3D
K
Enter
M
1
Shift
3
End
PgDn
PgUp
Ctrl
Ins
End
->
4-
+ ||
1O
V

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 has a pH of 4.5. What would be the color of the solution if each of the following indicators were added? (See Fig. 14-8.) a. methyl orange b. alizarin c. bromcresol green d. phenolphthalein
Two students were asked to determine the Kb of an unknown base. They were given a bottle with a solution in it. The bottle was labeled aqueous solution of a monoprotic strong acid. They were also given a pH meter, a buret, and an appropriate indicator. They reported the following data: volume of acid required for neutralization = 21.0 mL pH after 7.00 mL of strong acid added = 8.95 Use the students' data to determme the Kb of the unknown base.
1. Which of the following can act as a Lewis acid? (Hint : In each case, draw the Lewis electron dot structure of the molecule or ion. Are there lone pairs of electrons on the central atom? If so, it can be a Lewis base. Does the central atom lack an electron pair? If so, it can behave as a Lewis acid.) PH3 BCl3 H2S HS−
Classify each of the following statements as true or false: aAll Brnsted-Lowry acids are Arrhenius acids. bAll Arrhenius bases are Brnsted-Lowry bases, but not all Brnsted-Lowry bases are Arrhenius bases. c HCO3 is capable of being amphoteric. d HS is the conjugate base of S2. eIf the species on the right side of an ionization equilibrium are present in greater abundance than those on the left, the equilibrium is favored in the forward direction. f NH4+ cannot act as a Lewis base. gWeak bases have a weak attraction for protons. hThe stronger acid and the stronger base are always on the same side of a proton transfer reaction equation. iA proton transfer reaction is always favored in the direction that yields the stronger acid. jA solution with pH=9 is more acidic than one with pH=4. kA solution with pH=3 is twice as acidic as one with pH=6. lA pOH of 4.65 expresses the hydroxide ion concentration of a solution in three significant figures.
Are solutions of the following salts acidic, basic, or neutral? For those that are not neutral, write balanced chemical equations for the reactions causing the solution to be acidic or basic. The relevant Ka and Kb values are found in Tables 13-2 and 13-3. a. NaNO3 b. NaNO2 c. C5H5NHClO4 d. NH4NO2 e. KOCl f. NH4OCl
Each box represents an acid solution at equilibrium. Squares represent H+ ions. Circles represent anions. (Although the anions have different identities in each figure, they are all represented as circles.) Water molecules are not shown. Assume that all solutions have the same volume. (a) Which figure represents the strongest acid? (b) Which figure represents the acid with the smallest Ka? (c) Which figure represents the acid with the lowest pH?
. The concepts of acid-base equilibria were developed in this chapter for aqueous solutions (in aqueous solutions, water is the solvent and is intimately involved in the equilibria). However, the Brønsted-Lowry acid-base theory can be extended easily to other solvents. One such solvent that has been investigated in depth is liquid ammonia. NH3. a. Write a chemical equation indicating how HCl behaves as an acid in liquid ammonia. b. Write a chemical equation indicating how OH- behaves as a base in liquid ammonia.
A solution is made by dissolving 15.0 g sodium hydroxide in approximately 450 mL water. The solution becomes quite warm, but after it is allowed to return to room temperature, water is added to bring the volume to 500.0 mL of solution. (a) Calculate the pH and pOH in the final solution. (b) Why would we wait for it to return to room temperature? (c) If the mass of the water used to initially dissolve the sodium hydroxide were exactly 450 g and the temperature of the water increased by 8.865 C, how much heat was given off by the dissolution of 15.0 g of solute? Assume the specific heat of the solution is 4.184 J/g. K. What is the molar heat change for the dissolution of sodium hydroxide (known as the enthalpy of solution, Hsol)?
In the following net ionic reaction, identify each species as either a Brnsted-Lowry acid or a Brnsted -Lowry base: CH3COO(aq)+HS(aq)CH3COOH(aq)+S2(aq). Identify the conjugate of each reactant and state whether it is a conjugate acid or a conjugate base.
Note whether hydrolysis occurs for each of the following ions. If hydrolysis docs occur, write the chemical equation for it. Then write the equilibrium expression for the acid or base ionization (whichever occurs). a NO3 b OCl c NH2NH3+ d Br
State which of the following species are amphiprotic and write chemical equations illustrating the amphiprotic character of these species. (a) NH3. (b) HPO4-. (c) Br-. (d) NH4+. (e) ASO43-