The most basic solution from the following is: Pb(CH3CO0)2 FECL3 CH3COONA Al(CN)3

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.200 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: By using Henderson Hasselbalch equation the pH of the buffer solution is determined by using the…

Q: Calculate [H₂0%), (OH-) and % jonization FOR a 79 in solution of AND₂ K: FOR H₂U₂ = 5.1 X107

A: Given the molarity of HNO2 = 0.79 M  HNO2(aq) is a weak monoprotic acid with Ka = 5.1*10-4

Q: s the most acidic H

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Q: Account for the following : (a) La(OH)3 is more basic than Lu(OH)3 (b) Zn2+ salts are white. (c)…

A: a)  Due to lanthanide contraction, the size of Lu3+ is decreased, then, the covalent character of…

Q: Relative Acid Strength 2.51 Rank the following compounds in order of increasing acidity он NH2 HO,…

A: Since you have posted multiple independent questions in the same request, we will solve the first…

Q: Provide the products formed from the reaction below. Hl(aq) (one equivalent)

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Q: Which member of each pair produces the more acidic aqueous solution: CuCl or Cu1NO322,

A: Acidic strength determines the tendency of acid for the dissociation extent.

Q: Which of the following is an acidic salt? O a. Na2SO4 O b. NaCI С. КС O d. NH4CI O e. CH3COONa

A:

Q: Arrange the following compounds in order of increasing acidity но. HO, HO. F F (A) (B) (C) OC<A< B O…

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Q: Why is [Fe(OH2)6]³+ prepared in an acidic solution O A. It is a Bronsted acid in aqueous solution B.…

A: Answer - The correct option is (D)  All of these choice    The acidic character of an ionic compound…

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: An aq sn of a , leclysoe hasa feeing pointf8.20 C. TThe solution contains L4ol diolved in 7 O Whthe…

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Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.110 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

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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: 9. Write the balanced equation for the reaction between H2SO4(aq) and K2CO3(s).

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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: Classify the following reaction in as many waydal as possible S8+8O2 8SO2

A: Given reaction: Classification of Reactions: Chemical reactions can be classified as,…

Q: Predict which member of each pair produces the more acidic aqueous…

A: Acidic aqueous solution:

Q: D

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Q: Which of the following are the products of the reaction of a metallic oxide with an acid? a. a…

A: The oxide of an element (M) is formed by the combination of oxygen with the element. Based on the…

Q: ou have 10 mL of an 8% aqueous solution of H2Cl6Pt. The density of the solution is 1.05 kg.L-1…

A: Values given in the question are as follow: the volume of the solution is 10ml an 8% aqueous…

Q: Why is [Fe(OH2)6]3+ prepared in an acidic solution? A. It is a Bronsted acid in aqueous solution B.…

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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: What is the equilibrium constant for the reaction between HNO3 (aq) + F- (aq)?

A: When nitric acid and Fluoride ions combine, then following Equilibrium equation is obtained -…

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: What volume of0.317 M KOH solution will be required to titrations 25.00 mL of 0.285 M HN O3

A: The molarity of a solution is defined as the ratio of the number of moles of solute that are present…

Q: What is the pH of a 0.650 M solution of C5H;NHB (Kb of CsH;N is 1.7 × 10-º)?

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Q: D. NaCl (aq) + acidified MnO2 (s)

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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: 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 the pH of a solution of 0.300 M HNO2 containing 0.120 M NaNO2? (Ka of HNO2 is 4.5 × 10¬4)

A: The given data contains, Concentration of weak acid =0.300M Concentration of conjugate base =0.120M…

Q: 35. Which species can reduce Ag+(aq)? O SO4²- O None of the given. O Fe³+ O AU³+ O Br₂

A: Electron is required(accepted) during the reduction of Ag+(aq). The balanced reduction reaction of…

Q: Nahso3 titr. In neutral describe how the color goes from Mn04- to MnO2 In basic w NaOH describe…

A: Answer-1 In neutral medium, SO32- ion of NaHSO3 is oxidized by MnO4- ion into sulfate ion and MnO4-…

Q: D clhsy the folloy as solve ti prohe, Aprehic and Amphipratic Hd ly se N v, CHelz V CH COOH vi, CHe…

A: Since you have posted questions with multiple subparts, we will solve the first three sub parts for…

Q: If asolution hos a pH of O.800, the solution is concentration is ond the hylroagen a.) acidic,0.158M…

A: Given : pH = 0.800

Q: Calculate the sodium acetate/acetic acid ratio to prepare a buffered solution with a pH of 5.06.…

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Q: Which of the following would be the strongest acid? сон он cO.H Фн Нс но ON A в D A

A: Electron withdrawing groups present at the ortho and para positions of benzoic acid increase the…

Q: The most basic solution from the following is: * Pb(CH3C00)2 O CH3COONA O FECL3 O Al(CN)3

A: The acid-base nature of the salt solution depends on the nature of the acid and base from which the…

Q: Salt of anion X gives colorless gas when reacts with dil. HCl acid and can removes the color of…

A: Given statement is :  Salt of anion X gives colorless gas when reacts with dilute HCl acid and can…

Q: Calculate the concentration of CuS in a solution in which [H3O] is held constant at (a) 2.0 3 1021 M

A: The given data contains, concentration of H3O+ = 2.031021 M. Ksp of CuS= 8.0×10-37

Q: The following reaction has a AG° value of +8.43 kJ/mol at 25 °C. HA(aq) + H20(1) =H;0*(aq) +A (aq)…

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Q: Which of the following is an acidic salt? Provide an explanation Select one: а. FeCla b. NaBr с.…

A: There are different type of compounds, which may be acidic, basic or salty in nature.  But different…

Q: What is the pH of a 0.062 M NH4NO3 solution.  Kb for NH3 = 1.76e-5

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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: What is the molar concenuration of hydronium [H,O*] ions in a solution prepared at 25°C with a pH of…

A: The acidic or basic nature of a solution is determined by its pH value. pH measures the…

Q: What should be the minimum pH in order to extract Al(oH)3 from 0.01M Alcl3 solution? pKç Al(oH)3=33

A: Given data, Concentration of AlCl3 = 0.01M pKc of Al(OH)3 = 33

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…

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.