Which one of  the following 1 M solutions is  acidic?

Q: Calculate [H+] and [OH-] for each solution at 25°C. Identify each solution as neutral, acidic, or…

A: The question is based on the concept of PH and pOH calculations.   pH is defined as negative…

Q: -) Describe each of the following solutions as basic, acidic or neutral. a. pH = 4.5 b. pH = 13.1 с.…

A: PH =7 (Neutral) PH >7 Basic  PH < 7 Acidic

Q: 4. From the following list of salts, identify a writing a hydrolysis equation for each of the

A: As Q3 has been answered and explained in original answer, we will answer Q4 for you. Salt hydrolysis…

Q: Multiple Choice 1. A certain solution has a pOH of 6. How is this solution best described? a.…

A: 1.  POH = 6  Thus [OH-] = 10-6  PH = 14- 6 = 8  Thus solution is weakly basic  Correct answer is( d)…

Q: In each reaction, identify the Brønsted-Lowry acid, the Brønsted- Lowry base, the conjugate acid,…

A: Since we answer up to 3 sub-parts, we will answer the first three subparts only. Please resubmit the…

Q: 29. In, HF(aq) + H2O(1) 2 H3O+ (aq) + F-(aq), what are in the denominator of acid dissociation…

A: Given; Acid dissociation constant (Ka):

Q: the solution acidic or basic? How did you know?

A:

Q: Which of the following salts will be Acidic? A. Fe(NO3)3 B. AlCl3 C. NH4Br D. All of them Group of…

A: The salt of strong acid and weak base is acidic in nature. All the given salt is product of a…

Q: Write the acidic equilibrium equation for HNO,

A: A question based on equilibrium concept, which is to be accomplished.

Q: The Kw of water at 0°C is 1.12 x 10-15. A solution at this temperature has a pH of 7.20 .  a)Find…

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Q: 5. Acetic acid, CH3COOH is the main component of vinegar, apart from water. CH3COO(aq) + H3O* (aq)…

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Q: In which one of the following reactions does an H2O molecule behave as a Lewis base?   A.  H2O(l) +…

A: On the basis of Lewis concept, acid-base behavior can be defined as follows: 1. Lewis acid: Those…

Q: Consider the reaction below. Which species are the Brønsted-Lowry bases? HCO, (aq) + NO₂ (aq) =…

A: ->Bronsted acid is acid which can donate H+ to the base . -> Bronsted base is base which can…

Q: A- is a weak base. Which equilibrium corresponds to the equilibrium  constant Ka for HA? A. A-(aq) +…

A: A- is a weak base. Therefore , Equilibrium corresponds to the equilibrium constant Ka for HA is –…

Q: Which of the following is the correct equation for the dissociation of a weak acid in water ? A .…

A: A weak acid is the one which doesn't dissociate completely and have low Ka value.

Q: Solution X has a pH of 9.80, and solution Y has a pH of 7.2. a.) Which solution is more acidic?…

A:

Q: A solution contains 0. 01 M of NH3. Which of the following best describes this solution? A. Basic:…

A: 0.1 M NH3 is a Basic Compound

Q: The solution has [H+] = 2.2x10^-7M.  The solution is A. acidic B. basic

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

Q: 3. Identify the Acid, Base, Conjugate Acid, and Conate Base in the following equations: a) HCN (aq)…

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Q: From the choices below, select the statements that correctly describe acidic aqueous solutions. A.…

A: A neutral solution is one in which the concentrations of H+ and OH- are equal. [H+] = [OH-] An…

Q: 1142 PM Fri Apr 30 testnavciont.psonsvc.net 100% RETAKE S2 Chem Unit 9 Common Unit Assessment /4 of…

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Q: Which of the following statements is true about a solution of ammonium acetate, NH4C2H3O2? [Ka(NH4+)…

A: Given :  Ka(NH4+) = 5.56x10-10  Ka(HC2H3O2) = 1.8x10-5

Q: Q5. Identify the following solutions if they are strong/weak acid/base. A C D

A: Electrolytes are those Substances which are Dissolved in their aqueous solutions to give their…

Q: Are each of the following 0.100 M aqueous solutions: Acidic, Basic, or Neutral? 1. KCI [Select] 2.…

A: Given salts: KCl NH4Br Na2CO3 KClO (CH3)3NHCl We have to find whether the 0.100 M aqueous solution…

Q: Part C. Classify whether the parameter shown in each item is describing an acidic or basic. Legend:…

A: For an acidic solution pH < 7 while for basic solution pH > 7  Since , pH + pOH = 14  So, for…

Q: What is the correct relationship between Ka and Kb for a weak acid and its conjugate base…

A: We know, Ka × Kb  = Kw Kw is the ionisation constant of water.

Q: Propionic acid, which can be symbolized HC2H5CO2, is weakly acidic with a Ka in water of 1.3 x 10–5…

A:

Q: Nitrous acid, HNO₂, has a Kₐ of 7.1X10⁻⁴. What are[H₃O⁺], [NO₂⁻], and [OH⁻] in 0.60 M HNO₂?

A: First of all we have to write the equation for nitrous acid.     HNO2+H2O⇔H3O++NO-2…

Q: A. Which acid is stronger: HF (Ka=6.4x10-4) or NH4+(Kb for NH3 is 1.8x10-5)? B. Decide whether…

A: Answer:- This question is answered by using the simple concept of determination of nature of the…

Q: Given: HCO_3-(aq) + H_3O+(aq) = H_2CO_3(aq) +H_2O a. What is the conjugate of H_2CO_3(aq)? b.…

A: A conjugate acid has one more hydrogen and positive charge than the base that created it. A…

Q: HX (M=150. g/mol) and HY (M=50.0 g/mol) are weakacids. A solution of 12.0 g/L of HX has the same…

A: Given data contains, Density of HX is 12.0g/L. Molar mass of HX is 150.0g/mol. Density of HY is…

Q: Calculate the pH and pOH of an aqueous solution that is 0.75 % HCI, by mass, and has a density of…

A: Given :-  % by mass of HCl = 0.75%  density of solution = 1.04 g/mL  To calculate :-  pH and pOH for…

Q: The pH of an acidic solution is 4.77. What is [OH-]?

A: Given :- pH of solution = 4.77  To calculate :- concentration of OH- i.e. [OH-]

Q: ) 3a. Using ARIO, determine which reactant will act as the acid. Briefly explain your choice. Een…

A: The objective of the question is to complete the given reaction and label the species.The reacting…

Q: 5. a. Determine the hydrogen ion concentration, [H*] for a solution with a pH of 3.42. Is this…

A:

Q: Decide whether aqueous solutions are acidic, basic or neutral. Ka Zn(H2O)62+ = 1x10-9 Kb HCOO- =…

A: The question is based on the concept of salt hydrolysis. We have to identify the nature of the given…

Q: Identify each solution as acidic, basic, or neutral. [H3O+ ] = 3 × 10−13 M [OH−] = 4 × 10−11 M…

A: The concentrations given are, [H3O+ ] = 3 × 10−13 M [OH−] = 4 × 10−11 M [H3O+] = 1 × 10−8 M   [OH−]…

Q: he conjugate base of

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Q: Sodium nitrite (NaNO2) is a common ingredient added to processed meats and fish to preserve food and…

A: Answer:- This question is answered by using the simple concept of hydrolysis of salt of weak acid…

Q: Consider the following reactions: SO32 (aq) + H2O(1) HSO3 (aq) + H2O(1) HSO3(aq) + OH(aq) H2SO3(aq)…

A: In the given question we have to calculate the pH of the given solution.The pH is the negative…

Q: CaCO3 (aq) + 2H2O+ (aq)  -->  Ca2+ (aq) + CO2 (aq) + 3H2O (l) A.) How many moles of stomach acid…

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Q: Determine if each solution is acidic, basic, or neutral. [H3O*] b. [H3O+] =1x 10-5 M; [OH ]=1 x 10-9…

A: We’ll answer the first three subparts of the question. Please submit a new question to get remaining…

Q: What salt is produced in each of the following neutralization reactions? A HNO₂ (aq) + KOH(aq)…

A: Neutralization reaction: When acid reacts with base, salt and water are formed. This reaction is…

Q: he hypobromous acid, HBrO, and nitrous acid, HNO2, below. Which of the given statements is FALSE?…

A: Here we have to predict the false statements about Ionization of weak acids HBrO and HNO2 having…

Q: Indicate if the following solutions are acidic or basic. Consider 25 °C. a. pH = 2.50 b. [H*]>1.0 x…

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Q: 6. A substance has a [H,O'] of 5.21 x 10³, determine [OH], pH and pOH and determine if the substance…

A: [H3O+][OH-] = 1 x 10-14 pH = -log[H3O+] pOH = -log[OH-] pH < 7 , acidic pH > 7 , basic pH = 7,…

Q: Part A 0.28 M HC1 Enter your answers numerically separated by a comma. Express your answer using two…

A: Check the reaction of strong acid with water and then use the formula to calculate the pH of the…

Q: The pOH of a basic solution is 2.93. What is [OH-]? 1 4 7 +/- 2 M 8 3 5 6 9 0 X с x 100

A: As we know , pOH = - log [ OH- ] where [ OH- ] = molar hydroxide ion concentration.

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.