What is the total molar concentration of ions in 0.750M solution of K2CO3 assuming complete [3] dissociation?

Q: What is the pH of a 0.350 M solution of HF (Ka = 6.8 × 10⁻⁴)?

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Q: Carbonic acid, H2CO3 is a diprotic acid with Ka1 = 4.3 × 10-7 and Ka2 = 5.6 × 10¯11. What is the pH…

A: The Ka1 is greater than Ka2 by a fraction of 10-4.  In a diprotic acid, firstly the first hydrogen…

Q: 3. Calculate the pH of a 0.600M solution of Na2S

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Q: For a 0.0037 M solution of HCIO4, the dissociation of water produces the following concentrations of…

A: HClO4 is a strong acid, so, it undergoes complete ionization in the aqueous solution. HClO4 -->…

Q: What is the pH of a solution composed of 0.20 M NH3 and 0.15 M NHẠCH (Pkb of NH3=4.75) O 2.15 4.62…

A: Given:- NH3 = 0.20M = BaseNH4Cl = 0.15M = Saltpkb of NH3 =4.75pH = ?

Q: What is the pH of a 0.370 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: Given : Concentration of Ca(NO2)2 = 0.370 M And Ka of HNO2 = 4.5 X 10-4  Since Ca(NO2)2 is a…

Q: Ethylammonium chloride, CH;CH;NH3CI, is an acidic salt. (i) Write equations to show the dissolving…

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Q: What is the concentration of Ag(NH₂)* in solution?

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Q: What is the pH of a 0.590 M solution of C₅H₅NHBr (Kb of C₅H₅N is 1.7 × 10⁻⁹)?

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Q: What are the [H3Oʻ] and pH of 0.085M weak base C2HSNH2?

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Q: 27G. A solution that is 0.010 M of the salt triethanolammonium bromide, (CaH,ONHJBr. (Kb, (CsH9OsN)…

A: Nature of salt: 1. If a salt is made by reacting strong base and strong acid then it's nature would…

Q: What is the pH of a 0.0250 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: pH can be calculated as follows

Q: Write a net ionic equation to represent the reaction of (a) aqueous strontium hydroxide with nitric…

A: A net ionic equation for the reaction of strontium hydroxide with nitric acid has to be written.

Q: How many moles of nitric acid would you have if you had 0.550 L of a 0.025 M nitric acid solution?…

A: The number of moles of nitric acid (n) is calculated as shown below where M is the concentration of…

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: Arrange the following in order of INCREASING acidity. I. II. III. IV. ... ÇI CI HO HO HO HO

A: Given question of mainly phenol group.    We have difine a increasing acidic order.    Attached a…

Q: What is the concentration of ion or molecule in the solution of 0.0150 M C6H12O6?

A: Given: 0.0150M C6H12O6The given molar solution contains molecules of C6H12O6 since no ions are…

Q: What is the pH of a 0.1055 M CH3COOH solution (Ka = 1.75 × 10−5)?

A: Given concentration of CH3COOH = 1.75 × 10-5

Q: What is the pH of a 0.820 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: The pH of the solution is equal to the negative logarithm of hydronium ion while pOH of the solution…

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: pH of a 0.48 M solution of carbonic acid = 3.35

Q: Assuming complete dissociation, what is the pH of a 3.39 mg/L 2Ba(OH)2 solution?

A: Given, Mass of Ba(OH)2= 3.39 mg/L= 3.39 × 10-3 g/L We know , pH = -log[H+] Kw = [OH-] × [H+]

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: What is the pH of a 0.0760 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: Given salt is a mixture of W.B + SA  HONH3Cl it undergo salt hydrolysis  It's  pH = 7 - 1/2(pkb +…

Q: What is the concentration of sodium ions in 0.250 M Na₂CO₃?

A: Given that:  [Na2CO3] = 0.250M  Weak electrolyte partially dissociate into aqueous medium. Whereas ,…

Q: Calculate the concentrations of HF, OH−, and H3O+ in a 0.19 M KF solution (for which…

A: Given: The concentration of KF solution = 0.19 M Ka for HF = 6.8 × 10-4 We have to calculate the…

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

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Q: 1. Calculate pH and concentrations of the ions for ammonia aqueous solution with concentration 0.010…

A: Given that : The concentration of ammonia = 0.010 M The pKb of ammonia is 4.76. We have to calculate…

Q: What is the pH of a 0.560 M solution of Ca(NO₂)₂ (Ka of HNO₂ is 4.5 × 10⁻⁴)?

A: Given : Concentration of Ca(NO2)2 = 0.560 M And Ka of HNO2 = 4.5 X 10-4  Since Ca(NO2)2 is a…

Q: Carbonic acid, H₂CO₃ is a diprotic acid with Ka1 = 4.3 × 10⁻⁷ and Ka2 = 5.6 × 10⁻¹¹. What is the pH…

A: The carbonic acid is a diprotic acid. The major release of hydrogen ions occurs in the primary…

Q: what is the molar concentration of Br- ions in a 0.210 M aqueous solution of FeBr3 assuming complete…

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Q: Calculate the concentration of each of the ions in a solution of 0.850 M K2SO4. (Hint: write the…

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Q: Calculate the potassium ion (K+) concentration for a 0.289 M K2CO3 solution.

A: The concentration of K2CO3 is 0.289 M. It dissociates as per the following reaction,

Q: Define the equilibrium constant Ka (1.3 × 10–2) for the dissociation of the weak acid, HSO4–. Assume…

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Q: What is the pH of a 0.0380 M solution of HONH₃Cl (Kb of HONH₂ is 1.1 × 10⁻⁸)?

A: pH = 3.73

Q: Assuming full dissociation in water, what concentration of the following ionic compounds would have…

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Q: What is the pH of a 0.460 M solution of HF (Ka = 6.8 × 10⁻⁴)?

A:

Q: Calculate the concentration of S2- in an aqueous solution of 0.239 M hydrosulfuric acid, H2S (aq).…

A: Given :  0.239 M Hydrosulfuric acid . To find : concentration of S2-

Q: What is the pH of the solution containing 0.20 M NH3 and 0.15 M NH4Cl?

A: In an aqueous solution that consist of a mixture of the conjugate base of a weak acid along with the…

Q: The net ionic equation for the reaction of NaOH with HCIO4 is:

A: A balanced chemical reaction is the representation of the elements involved in the reaction along…

Q: What concentration of KNO2 must be added, at 25 degrees Celsius, to 0.50 M HNO2 to result in a…

A: The solution mixture is a buffer solution of weak acid HNO2 and conjugate base NO2- ( as KNO2…

Q: Calculate the pH of a solution of 0.25M Nacio(ag). The Ka of HCIO is 2.9 x 108.

A: NaClO is a salt of weak acid HClO. It has pH greater than 7 as it is base.

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: What is the concentration of each ion in each of the following solutions? (assume complete…

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Q: Calculate the equilibrium concentration of H3O+H3O+ in a 0.20 MM solution of oxalic acid

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Q: What is the molar concentration of ions in a solution that is 0.292 M in MgCO3?

A: The given solution is 0.292 M MgCO3. The molar concentration of ions is =?

Q: What is the concentration of sodium ions in 0.315 M Na₂CO₃?

A: Given: Concentration of Na₂CO₃ = [Na₂CO₃] = 0.315 M

Q: 2. Calculate the molarity of the resulting solution if 0.629 grams of Hydrogen ion [H*] is dissolved…

A: In the given question we have to calculate the molarity and pH of the hydrogen ion. given data:…

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.