Calculate the molar H3O* ions concentration of a solution that has a pH of (а) 4.31 (b) 4.48 (c) 0.59

Q: Calculate the hydrogen ion concentration of a Nitric acid solution with a pH of 2.11.

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Q: Carbonic acid, H,CO, is a diprotic acid with Ka1 = 4.3 × 107 and Ka2 = 5.6 × 1011. What is the pH of…

A: H2CO3 ⇌HCO3−  +   H+.........     ka1= 4.3x10-7 HCO3− ⇌CO3-2 ​+   H+..........    Ka2=5.6x10-11ka1…

Q: If the hydrogen ion concentration of a 0.100 M HClO solution is 0.000 055 M, what is the ionization…

A: The equation for the ionization of HClO is as follows. HClO(aq)↔ClO-(aq)+H+(aq)

Q: Chemical pH #1 2 #2 9 #3 12 # 4 Which of the following chemicals will be a strong base? 1 3 4

A: Given  PH of different chemical = 2 ,9 ,12,5  Strong Base = ?

Q: Which of the following does not represent a Lewis acid-base reaction?

A: According to the Lewis definition, the species which donates lone pair of electrons acts as a Lewis…

Q: The reaction of ammonia with copper(II) ions is an example of a Lewis Acid–Lewis Base reaction.…

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Q: The pH of a 0.0058 M solution of HNO, is

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

Q: How would the pH of a 0.175 M solution of NaC4H,O2 compare with that of a 0.175 M solution of…

A: The salt gets hydrolyzed when dissolved in water. Both salt have the same acid and similar strong…

Q: Calculate the pH of solutions with the following concentrations. [H3O+]= 1×10−8M

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

Q: What is the pH of a 0.720 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: 7. The pH of a 0.10 M solution of acetic acid (CH3COOH) is 2.39. What is the Ka of acetic acid?

A: H3O+ can be calculated as follows: pH=-log [H3O]+[H3O]+=10-pH[H3O]+=10-2.39[H3O]+=0.00407 M

Q: What is the pH of (a) a 0.028 M solution of NaOH, (b) a 0.0011 M solution of Ca1OH22?

A: What is the pH of (a) a 0.028 M solution of NaOH, (b) a 0.0011 M solution of Ca(OH)2?

Q: What is the pH of a 0.650 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: What is the pH of a 0.050M solution of (CH3)3N?

A: (CH3)3N is a weak base. The Kb of (CH3)3N is 6.5 x 10-5 at 25 0C When a weak base mixed with water…

Q: What is the pH of a 0.530 M solution of HNO₃?

A: Given information is as follows: The concentration of the HNO3 solution =0.530 M The pH of the HNO3…

Q: Why does boric acid function as such a very weak monobasic acid?

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Q: The pH of a 0.0041 M solution of HNO₃ is

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Q: calculate the ph of a 0.600 solution of Na2S

A: When Na2S dissolved in water - Na2S + 2H2O <===> 2NaOH + H2S Thus, sodium Sulfide is a salt of…

Q: Using data from Appendix D, calculate 3OH-4 and pH for each of the following solutions: (a) 0.10 M…

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Q: Calculate the acid ionization constant (Ka) if the pH of the 0.1 M acetic acid solution is 2.87?

A: We have given that  Concentration of acetic acid = 0.1M  pH = 2.87

Q: Use the References t The pH of an aqueous solution of 0.177 M sodium fluoride, NaF (aq), is This…

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Q: The pH of a 0.0031 M solution of HNO, is 3

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Q: What is the pH of a 0.605 M solution of HNO₃?

A: The given data is as follows: The concentration of HNO3 = 0.605 M The pH of HNO3 solution = ? The pH…

Q: The pH of a solution is 2.55. What is the [H3O+]?

A: We know that, pH can be expressed as negative logarithm of hydrogen ion concentration or hydronium…

Q: Using data from Appendix D, calculate 3OH-4 and pH for each of the following solution 0.035 M Na2S

A: 0.035 M Na2S hydrolyze in water to produce OH- ions. The ICE table is as follows:

Q: The pH of a 0.0046 M solution of HNO, is

A: Ph is the negative logarithm of the concentration of Hydrogen ion for dilute solutions. Thus, pH is…

Q: Given that the pH is 10.285 What is the: [H3O+] pOH [OH-] Is it an acid or base?

A: It is given that the pH of a solution is 10.285 and the [H3O+], the pOH and [OH-] needs to be…

Q: What is the pH of a 0.510 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

A: Given information: Concentration of solution = 0.510 M

Q: is HC2H3O2 an acidic ionic or a covalent bond?

A: HC2H3O2 this is a chemical formula of acetic acid (CH3COOH).It has one double bond between Carbon…

Q: If the [H3O+] concentration is 0.00047M, what is the pH?

A: Given, Concentration of H3O+ ion = [H3O+] = 0.00047 M pH of the solution = ? Note: pH: It can define…

Q: Explain the bond formation between NH3 and Ni2+ in terms of Lewis acid-base theory.

A: To explain: The bond formation between NH3 and Ni2+.

Q: What is the pH of an aqueous solution with a hydronium ion concentration of 1.75 × 10⁻⁵ M?

A: We know that, pH is the negative logarithm of hydronium ion concentration. i.e.,…

Q: The pH of a 0.0047 M solution of HNO, is

A: As HNO3 is a strong acid, it completely ionises in the solution.

Q: What is the pH of a 0.600 M solution of Na2S?

A: In this question, we want to determine the pH of the salt solution ( Na2S ) How we can calculate,…

Q: Calculate the pH of the following: a. [H*]=1x 10³ M %3D

A: Given that, [H+] = 1×10-3 M  pH = ?

Q: What is the pH of a 0.130 M solution of HNO₃?b

A:

Q: The pH of a 0.0065 M solution of HNO3 is

A: pH of a solution is the measure of its acidity or basicity. The values on the pH scale lie between 0…

Q: Write the reaction that occurs, and identify the conjugate acid-base pairs of the following…

A:

Q: Arsenic acid, H3AsO4, is used industrially to manufacture insecticides. Arsenic acid is a polyprotic…

A: Given, Arsenic acid is a polyprotic acid with Ka1 = 2.5 × 10–4 Arsenic acid is a polyprotic acid…

Q: What is the pH of a 0.500 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: Rank the following acids in order of increasing strength: ClCH2SH, CH3SH, H2S.

A: The acidic strength of any acid is proportional to the stability of the anion formed by removing the…

Q: In the following reaction, identify the Lewis acid. Co** (ag) + 6NH3 (ag) - Co(NH3),**(aq)

A: Lewis acid is an electron-pair acceptor. That is Lewis acid is any substance which can accept a pair…

Q: The pH of a 0.0080 M solution of HNO₃ is

A:

Q: Which of the following is the stronger Brønsted–Lowry acid, HClO3 or HClO2?

A: Any chemical species able to gain (receive) a proton (H+) ion from another species gets referred as…

Q: Rank the following in order of increasing acid strength: HIO₃, HI, CH₃COOH, HF.

A: Given, HIO₃, HI, CH₃COOH, HF.

Q: Arrange the following oxoacids in order of decreasing acid strength: HCIO, HCIO2, HCIO3, HBrO

A: Acidic strength is directly proportional to electronegativity  of the central atom. So HBrO is least…

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.