why are Ka values difficult to evaluate for acids like HBr, HCl, and HNO3?

Q: . Write the base dissociation reaction (equilibrium) for benzoate ion (C,H$CO2) in water; (remember,…

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Q: Consider a weak acid "HA". What is the pH of a 0.626 mol L¯' solution of HA? The KA of HA is 6.5 x…

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Q: 2) A 0.10 M solution of which of the following salts would be predicted to exhibit a pH of 7.46 at…

A: Henderson Hasselbalch equation The equation that is used to calculate the pH of a buffer system is…

Q: The acid ionization constant (Ka) for HI is estimated to be 1 x 109. What is the value of Kb for I–

A: Given, Acid ionization constant for HI, Ka = 1 × 109

Q: For the acid HNO2 identify its conjugate base, write the dissociation reaction and write the acid…

A: Bronsted-Lowry concept of an acid and base, the conjugate base can be differentiated by a proton as;…

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

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

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Q: Use the following acid dissociation constants to identify the correct decreasing order of acid…

A: More is the value of Ka more stronger is the acid .

Q: What is the pH of the hypothetical diprotic HydroRoseburgic acid with a concentration of o.75M? You…

A: Assume diprotic acid as H2A First dissociation of acid is         H2A (aq)+ H2O(l) -->HA-(aq) +…

Q: A solution of 0.100 M bromoacetic acid (BrCH;COOH) is ionized by 13.2%. Calculate the (H'],…

A: Given that, 0.1 (M) bromoacetic acid (BrCH2COOH) solution is ionized by 13.2% We have to calculate…

Q: Construct the expression for Ka for the weak acid, HCN. HCN(aq) + H20(1) = H;0*(aq) + CN"(aq) 1…

A: Given: balanced chemical equation HCN and H2O. To find: Expression of Ka. Solution: As we know that,…

Q: A strong acid has a large or small Ka value?

A: Strong acid is a type of acid which has a high tendency to dissociate into ions in the aqueous…

Q: A 0.466 M solution of the salt NaA has a pH of 11.84.  Calculate the Ka value for the acid HA.…

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Q: Use the following data to determine what is the base dissociation constant for hydrogen carbonate…

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Q: What is the pH of the solution obtained when 130 mL of 0.610 M NaOH is diluted to 16.0 L with water?…

A: Given: Initial concentration of NaOH = 0.610 M Initial volume of solution = 130 mL = 0.130 L…

Q: Construct the expression for Ka for the weak acid, HC,H,04. HC,H,0,(aq) + H,0(1) = H,0*(aq) +…

A: Given, given chemical reaction as follows,HC9H7O4(aq)+H2O(l)⇌H3O+(aq)+C9H7O4-(aq)we are asked to…

Q: Construct the expression for Ka for the weak acid, HCN. HCN(aq) + H:O(I) = H.O(aq) + CN (aq Based on…

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Q: Calculate the Ka of a weak acid if a 0.065 M solution of acid has a pH of 2.96 at 25 degrees…

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Q: HCIO, (aq) + KOH(aq) KCIO, (aq) + H,O(1) AHan kJ/mol %3D HBr(aq) + KOH(aq) · KBr(aq) + H,O(1) AHn =…

A: In neutralization reaction, acid and base react together to give corresponding salt and the solvent.…

Q: Acids & Bases: Understanding Connections Between Descriptions of Weak Acid Dissociation When a…

A: The acid can be represented as HA. Acid dissociation constant of the reaction is given.

Q: The K, for hydrofluoric acid HF is 6.8 x 104. (4 points) Calculate K, for its conjugate base F…

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Q: HA, a weak acid with a single proton in a 0.050 M acid solution, ionizes by 16%. The ionization…

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Q: Calculate the [HA] of 0.0644M anilinium chloride solution.  Calculate the concentrations of the…

A: Structure of anilinium chloride: pKa value for anilinium ion = 4.6 Since pKa = -logKa Ka = 10-4.6 =…

Q: A 0.055 M solution of HX is 6.7% ionized. Calculate Ka of this acid.

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Q: Rank the following salts in order of increasing pH of 0.1 M aqueous solutions. (Hint: write out the…

A: We are given a combination of acidic, basic, and neutral salts.  Each salt has a concentration of…

Q: Use the Kb for the nitrite ion, NO2−, to calculate the Ka for its conjugate acid.

A: Ka x Kb = Kw =  1 x 10-14   Conjugate acid of NO2− is HNO2

Q: 10. The pH of 0.25 M aqueous solution of a weak acid HA is observed to be 4.15. Determine the acid…

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Q: The pka values of a weak acid is directly proportional to basicity. O True O False

A: The given statement is True. It can be explained as below:

Q: -69 The acid dissociation constant K, of hypobromous acid (HBrO) is 2.3x 10. Calculate the pH of a…

A: Consider the dissociation of hypobromous acid is as follows:                       HBrO   →     H+…

Q: Construct the expression for Ka for the weak acid, CH;COOH. CH;COOH(aq) + H2O(1) = H;O*(aq) + CH;COO…

A: Chemical equilibrium is defined as the dynamic condition, reached by a reversible reaction when rate…

Q: A weak monoprotic acid, HA dissociates by 2.416 % and has a pH of 3.61. Calculate the Ka value for…

A: percent dissociation of HA is 2.416% pH = 3.61

Q: Important equations: Ka × Kb = KwpKa= −logKa   A key component of understanding weak acids is…

A: HBr ,HCl,HI etc are strong acid so dissociation constants will be very high.

Q: Construct the expression for Ka for the weak acid, NH,. NH, (aq) + H,0(I) = H;O*(aq) + NH(aq) Based…

A: Dissociation constant for acid, ka, is defined as ratio of product of concentration of products to…

Q: Kw = [Ka][Kb]. Verify this relation using formic acid. [HCO2H]

A: Here is your answer........

Q: Acids & Bases: Understanding Connections Between Descriptions of Weak Acid Dissociation In an…

A: pH;Negative logarithm of base 10 Hydrogen ion concentration is known as pH.The concentration of…

Q: Construct the expression for Ka for the weak acid, HCN. HCN(aq) + H2O(1)=H;O*(aq) + CN (aq) 1 Based…

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Q: Show by computation which acid is the weakest based on its % ionization. The lesser its %…

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Q: Complete the following table, which lists information about the measured acid dissociation constants…

A: Pka can be calculated by using formula pKa= -logKa

Q: Predicting acid or base strength from the conjugate species 0.1 M aqueous solution НСООН HC,04…

A: pH is used to determine the alkalinity or acidity of a reaction. The pH is determined as the…

Q: Calculate the Ka of a 0.400 M acid solution with [H 3 O^ + ]=1.4*10^ -4 M

A: Given,  The concentration of an acid =0.400 M.  and the [H3O+] = 1.4×10-4 M

Q: Construct the expression for Ka for the weak acid, HC3H;O4. HC,H,04(aq) + H20(1) = H3O*(aq) + C9H,O4…

A: The given chemical reaction is- HC9H7O4(aq)+H2O(l)↔H3O+(aq)+C9H7O4-(aq) Weak acids partially…

Q: Complete the following table, which lists information about the measured acid dissociation constants…

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Q: Acids & Bases: Understanding the Connection Between Descriptions of Weak Acid Dissociation When…

A: Given,Concentration of Acid = 0.013MPercent dissociation of acid = 0.23%The concentration of…

Q: Construct the expression for Ka for the weak acid, NH,*. NH, (aq) + H,O(1) =H,Oʻ(aq) + NH,(aq) 1…

A: Construct the expression for Ka for the weak acid NH4+ ----

Q: Choose the correct answer from among the alternatives; To make the sentence true: hydrocyanic acid…

A: The correct option is  c) ka=[CN-]/[H2O][HCN]

Q: 13. Write the Ka expression for the following HF

A: We know that HF is a weak base. When dissolved in water.   HF (aq) + H2O   → H3O+ (aq) + F- (aq)

Q: A solution is prepared at 25 °C that is initially 0.26M in methylamine (CH,NH,), a weak base with…

A: this is a basic buffer , so we will use the formula of basic buffer.

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.