Calculate the concentration of the molecules ionized in a 0.10 M HF given a Ka of 6.8 x 10-4 given:

Q: Calculate the pOH of a 6.0 M solution of HCl. 0.78 14.78 13.22 -0.78 -0.90

A: As we know, HCl is a strong acid and completely dissociates as follows:       HCl -----> H+ +…

Q: Identify the weakest acid from the following data: a. Hydrofluoric acid K₂ = 6.7 x 10-14 b. Acetic…

A: In this question, we will see which acid is weakest acid. Acid strength is depends on Ka value of…

Q: A 5.0M solution of acetic acid (pKa=4.75) has a pH of 6.75. The ratio of acid to conjugate base is?

A: The pH of a buffer is calculated by Henderson-Hasselbach equation. pH=pKa+log[conjugate…

Q: What is the equilibrium constant expression, Ki, for the following weak acid? H3PO4(aq) ↔ H+(aq) +…

A: We have to predict equilibrium constant expression for dissociation of weak acid.

Q: 37. Compute the concentration of hydroxide ion, [OH] in 0.2 M HF. Given Ka for HF is 6.6 x 10-4. * O…

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Q: Calculate the percent ionization of formic acid (HCO2H) in a solution that is 0.222 M in formic acid…

A: The pH of the solution is calculated in accordance with the Henderson-Hasselbach- equation.

Q: Determine the [H+] in a 0.0244 M HClO solution. The Ka of HClO is 2.9 × 10 -8.   a. 1.61   b.…

A: The dissociation behavior of a weak Bronsted acid in aqueous solution, is defined according to its…

Q: Calculate the pH and pOH of a 1.00 × 10-3 M solution of acetic acid (Ka = 1.75 × 10-5

A: We know                 CH3COOH + H2O ⇌H3O++CH3COO-t=0                 C                 -…

Q: What is the equilibrium constant expression, Ki, for the following weak acid? H3PO4(aq) + H*(aq) +…

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Q: What will be the Ka of an acid solution that is 0.012 % ionized when it is 0.20 M?

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Q: Phenol, C6H5OH, has a Ka of 1.3 x10-10.(a) Write out the Ka reaction for phenol.(b) Calculate Kb for…

A: Phenol is an aromatic alcohol.  The Ka value of phenol is given as 1.3×10-10.

Q: Calculate the [OH- and the pH of a solution with an [H*] = = 6.8 x 10-10 M at 25 °C. [OH]= %3D pH =…

A: The answer to the given three questions can be answered as follows -

Q: 11. What is [H*] in M for a solution with POH=1 ]1 × 10–12 |1 x 10-7 1 × 10–13 |1 x 10-9 |None of…

A: PH is defined as negative logarithm of concentration of [H+] ion.

Q: Calculate the molar concentration for acetic acid that ionized at 2.5%, ka=1 ×10-5

A: Let Molar concentration of acid is x percentage dissociation of Acetic acid = 2.5 %  Ka for acid = 1…

Q: Calculate the % ionizations of hydrofluoric acid having the following concentrations. 60M HF 0046M…

A: Ionization means dissociation of substance into ions. HF→H++F- Strong electrolytes dissociates…

Q: Calculate the hydrogen ion concentration of a solution containing 0.02M acetic acid and 0.01M sodium…

A:

Q: THE Ka for weak acid (HA) is knwon to be 1.9x10^-5. What is the ratio of [A-] to [HA] at a pH of 6?

A: Since it is given that the solution is having both HA and A- ion in the solution  hence the solution…

Q: Which one of the following is the weakest acid? O HF (Ka = 6.8 × 10-4) HCIO (Ka = 3.0 x 10-8) O HNO2…

A: Lower the value of acid dissociation constant (Ka), lower the concentration of H+ ions.  Hence, we…

Q: Find [H+], [HSO4-], and [SO4-2] in a 0.0250 M solution of sulfuric acid. (Ka of HSO4- = 1.30 x 10-2)

A: The sulfuric acid is considered as strong electrolyte thus it completely dissociates into H+ ion and…

Q: Consider the following reaction. HS- + H2O ↔↔  H2S +  OH- K = 5.09⋅10−35.09⋅10-3…

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Q: a) Calculate the percent ionization of 0.00490 M hypobromous acid (Ka = 2.5e-09). % ionization =…

A: a) Given: Concentration of hypobromous acid i.e. HBrO = 0.00490 M And Ka of HBrO = 2.5 × 10-9  Since…

Q: Rank the following acids in order of DECREASING acid strength Acid Ka I. HIO3 1.7e-1 II. HC3H503…

A: pKa is a negative log of acid dissociation constant(Ka). The mathematical expression is pKa = -log…

Q: What is the hydronium ion concentration in 0.275 M nitrous acid? Ka= 7.1x10^-4

A: We have to predict the hydronium ion concentration.

Q: Which of the following is the most basic?  A solution with [H+] = 1.0×10-3.  A solution with [OH-]…

A: The basic nature of a solution can be determined by comparing the concentration of the hydrogen ion…

Q: Decide whether solutions of the ammonium fluoride are acidic, neutral, or basic. a. K for NH3 is 1.8…

A: Kb  and Ka are dissociation constants of base and acid respectively . Greater is the dissociation…

Q: The Ksp for In(OH)3 is 1.3 x 10-37.…

A: We know that at pH= 6, [OH-] = 10^-8, therefore substituting the values in the Ksp formula, we find…

Q: For each value of Ka, calculate the corresponding value of pKa. Which compound is the stronger acid?…

A: pKa of any acid can be calculated as: pKa=-logKa Ka is dissociation constant of an acid. Larger the…

Q: The Ksp for In(OH)3 is 1.3 x 10-37.…

A: Given that Ksp for In(OH)3 is 1.3 x 10-37

Q: Calculate the concentration of OH- ions in a H2SO4 solution of 1.42 M at 100 oC

A:

Q: Which solution below is the most acidic? Group of answer choices [H3O+] = 1.0 × 10–10 M [H3O+] = 1.0…

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Q: Which of the following is true about a 0.10 M solution of the weak acid HX, which has a Ka of 1.0 x…

A: we have given that Concentration of [HX] = C = 0.1M = 10-1 Ka = 10-5 we have given [HX] is weak acid…

Q: Which of the following hydronium ion (H3O+) concentrations would produce a basic solution? a.…

A: The basic solution has a pH > 8.

Q: Morphine is an effective painkiller but isalso highly addictive. Codeine is a popular…

A: The pH of a solution is calculated by equation (1) in which H+ is the concentration of hydronium ion…

Q: The pH of a 0.464 M solution of phosphorous acid (H3PO3) is 1.11.  Using this information, calculate…

A: We have pH of H3PO3 as 1.11, also all H+ comes from the first dissociation of given acid. We have to…

Q: What is the Ka for a 0.1459 M acetylsalicylic acid solution, C9H7O4H, if it had a hydronium ion…

A: Using  the the Rate constant  expression  at equilibrium  we can find  the rate dissociation…

Q: Answer the following questions about acid-base equilibrium reactions (d)Based on the following…

A: A strong acid shows complete dissociation to respective anion and H3O+whereas a weak acid can only…

Q: A 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11.  What is the Ka…

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Q: If the Ka of a weak acid is 1.6 x 10-8, the Kb of its conjugate base partner must be which of the…

A:

Q: Choose the correct answer: Which of the following is the strongest acid? HO. HO. HOH CI Br II II Но…

A: COMPOUND SHOWN IN - OPTION -II (FLUORINE DERIVATIVE) IS THE MOST ACIDIC ONE AMONG THE MENTIONED…

Q: 8. Dimethylamine (CH;),NH is a weak base with a pKa of 11.0 a. Calculate the pH of a solution of…

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Q: Calculate the pH of the weak acid HF at equilbrium, if the inital concentration of  HF was 0.0340 M.…

A: Answer :- pH = 3.2  The pH of the 0.0340 M weak acid HF = 3.2…

Q: Calculate [OH ], [H*], and the pH of 0.42 M solutions of each of the following amines (K, for…

A: (a) When aniline dissolved in water, it gives - C6H5NH2 + H2O <===> C6H5NH3+ + OH- Then - Kb =…

Q: tic acid. 16.54 A 0.100M solution of bromoacetic acid (BrCH2COOH) is 13.2% ionized. Calculate [H*],…

A: The initial concentration of bromoacetic acid (BrCH2COOH) is 0.100 M or (mol/L). The percent…

Q: Determine the concentration of a solution of sodium fluoride (NaF) that has pH of 8.51 at 25C. HF…

A: Given that pH of NaF = 8.51  Ka of HF = 7.1x 10-4 [H+] = (Ka .C)1/2 pH = -log [H+]

Q: The base protonation constant K, of 1-H-imidazole (C;H,N,) is 9.0 x 10-8. Calculate the pH of a 0.57…

A: We have to predict the pH of solution.

Q: Which of the following is the correct expression for Ka? Assume the acid dissociation is…

A: An acid dissociation constant, Kₐ, is a quantitative measure of the strength of an acid in solution.…

Q: Calculate the [H3O+] for a solution with pOH of 7.17. Express your answer to two significant…

A: Given that: pOH = 7.17 We know, pH + pOH = 14 So, pH = 14- pOH              = 14-7.17…

Q: Identify which of the acids below will yield the stronger conjugate base and why.  a) HOCl (K a =…

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Q: Given that pKb for nitrite ion (NO-2) is 10.85, find the quotient [HNO2]/[NO-2] in a solution of…

A: Given  pKb for NO2- = 10.85  For HNO2 pKa = pKw - pKb = 14 - 10.85 = 3.15  Ka = 7.1 x 10-4  Chemical…

Q: 0.785M solution of the weak acid, hypoiodous acid, HOI, has a Ka of 2.32x10-11.  What is the…

A:

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.