1- Calculate the equilibrium concentrations of A and B in 0.10M solution of AB with equilibrium constant 3 x 10%.

Q: What is the pH of a 3.50 M solution of NH4CI (Ká of NH3= 1.8 x 105)?

A:

Q: 4. Calculate the pH of a salt solution of NH,CI with molar concentration 0.1 M (Kh = 5.71 x 101")

A: Given, The molarity of NH4Cl = 0.1M            Kh = 5.71 × 10-11

Q: Calculate the pH of a 0.381 M NH, solution. NH, has a Kp = 1.8 x 10-.

A: pH: The negative logarithm of H+ ion concentration is known as pH. Ammonia in water behaves as a…

Q: 1. Calculate the value of K for the reaction

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Q: What is the pH of a solution of 0.300 M HNO2 containing 0.210 M NANO2? (Ka of HNO2 is 4.5 x 10-4)

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: What is the pH of a solution with a fluoride concentration of 0.18 M ? The Kb for F– is 1.47×10-11 .

A: pH: It measures hydrogen ion concentration, which helps in a measure the acidity of the solution,…

Q: The acid ionization constant for Fe(H20)63+(aq) is 7.7x10-3. Calculate the pH of a 0.4630 M solution…

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Q: What is the pH of a 0.680 M solution of Ca(NO2)2 (Ka of HNO, is 4.5 x 104)?

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Q: What is the pH of a 0.40 M solution of sodium nitrate, NaNO2 ? The pKa for nitrous acid (HNO2) is…

A: Base dissociation constant Kb is utilized to determine the basic nature of a solution. It refers to…

Q: Calculate the pH of a 0.10 M solution of sodium hypochlorite (NaCIO; Ka 2.90 x 10-8). Also,…

A:

Q: Calculate the pH of a solution containing 0.1M NH,OH and 0.01M NH.CI, K = 1.76 x 10$. %3D

A: Given, [NH4OH] = 0.1 M [NH4Cl] = 0.01 M Kb = 1.76 × 10-5

Q: The first step in the preparation of magnesium metal is the precipitation of Mg(OH)2 from sea water…

A: At certain temperature, the mixing property of components is determined by their solubility product…

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.170 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: pH of a solution is defined as the negative logarithm of H3O+ ion concentration. Here the given…

Q: The pKa for the first protonation of nicotine (2) is 8.02. What is the pH and the fraction of…

A:

Q: Determine the pH and pOH of 0.25 L of a solution that is 0.0201 M boric acid and 0.0366 M sodium…

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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 is the pH of a solution of 0.300 M HNO₂ containing 0.140 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: Given : Concentration of HNO2 = 0.300 M Concentration of NaNO2 = 0.140 M And Ka of HNO2 = 4.5 X 10-4…

Q: Calculate the pH at equivalence. The p K of nitrous acid is 3.35.

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Q: The acid ionization constant for Ga(H20)63+(aq) is 2.5x10-3. Calculate the pH of a 0.1120 M solution…

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Q: What is the pH of a 0.570 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 10-4)?

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Q: 5. A solution is initially 0.050 M in ammonia, NH3 (Kp = 1.8 x 10°). (a) Write the equilibrium…

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Q: What is the pH of a 0.36 M solution of HNO2 (Ka = 4.5 x 10-4)?

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Q: Calculate the pH of a 0.363 M NH, solution. NH, has a Kp 1.8 x 10-5. %3D pH

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Q: 3. What is the value of k"?

A: OH- + C24H30N3+  C23H30N3-OH The general rate law is   [rate] = k [OH-]^x [ C24H30N3+]^y For the…

Q: You have a solution of nitrous acid (HNO2). What effect will addition of sodium nitrite (NaNO2) have…

A: Common ion effect The shift in equilibrium to a ion common to ion already present in the solution is…

Q: Calculate the pH of a 0.500 M aqueous solution of NH3. The Kp of NH3 is 1.77 x 10-5 O 8.95 O 11.47 O…

A: Given: Molarity of aqueous solution of NH3 = 0.500 M Kb of NH3 = 1.77×10-5

Q: If the Kp of a weak base is 2.5 x 10-6, what is the pH of a 0.23 M solution of this base?

A: pH +  pOH = 14 For a weak base solution: [OH-] = (Kb x C)1/2 Where, C = molar concentration of weak…

Q: What is the percent ionization of nitrous acid in a solution that is 0.230 M in nitrous acid (HNO2)…

A: The percent ionization of nitrous acid in a solution is to be calculated

Q: For the following reaction, ide Xo 요 i 1 || IV Acid Base Acid I and II B. I and III I and IV D. II…

A: 2) Bronsted-Lowry base is a base which accepts a proton(H+). Compound I accepts a proton from…

Q: What is the pH of a 0.660 M solution of C3H;NHB (Kb of C5H5N is 1.7 x 10-9)?

A: Given information, [C5H5NHBr] = 0.660 M Kb of C5H5N = 1.7*10-9 Calculate: pH = ?

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.150 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: In this question, we will calculate the pH of this solution ( this is a buffer solution ). For…

Q: Phenoxide ion (C,HsO) is a weak base, with Kp = 7.70 x 10. Calculate the pH of a 0.50 M aqueous…

A: Given that  Kb = 7.70 × 10-5  Peroxide ion is a weak base

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: What is the pH of a 0.64 M solution of NH3 (Kb = 1.2 × 10-5)?

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Q: Calculate the pH of a solution containing 0.085 M nitrous acid (HNO2, Ka = 4.5 * 10-4) and 0.10 M…

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Q: Calculate the pH of a solution prepared by dissolving 0.040 moles of sodium nitrite (NaNO2) in 200…

A: When HNO2 and NaNO2 are mixed, they form buffer solution HNO2/NO2-. And the pH of a solution is…

Q: Which of the following K values would indicate the weakest base of the group? O 1.2 x 109 O 6.3 x…

A: Ans:- (1.2×10-9 is the weakest base of the group).

Q: 16.72 Calculate the molar concentration of OH in a 0.724 M solu- tion of hypobromite ion (BrO"; K, =…

A:

Q: Alizarin yellow R, Ka = 7.9 x 1012, is yellow in its protonated form (HX) and red in its ionized…

A: Alizarin yellow (R)  be a distinct orange color when,…

Q: Calculate the molar concentration of OH- in a 0.724 M solution of hypobromite ion 1BrO-; Kb = 4.0 *…

A: Since the BrO- will get hydrolysed by water as per the reaction => BrO- (aq) + H2O (l)…

Q: A 0.0834 M solution of a weak ačid has a pH of 2.07. Calculate K, for the acid. O 5.9 x 102 O 3.4 x…

A: Write the expression for pH. pH=-log[H+] [H+]=Ka(HA) where Ka is the acid dissociation constant.

Q: If the equilibrium constant for A + B  C is 0.175, then the equilibrium constant for 2C  2A + 2B is

A: Given data,K=0.175,for the reaction :A+B→C

Q: Calculate the pH of 0.0470 M LiBrO. Ka of HBrO = 2.8 x 10-9

A: The molarity of LiBrO solution is = 0.0470 M The dissociation constant of the weak acid HBrO is =…

Q: The acid ionization constant for Sc(H2O)63+ (aq) is 5.0×10-5 . Calculate the pH of a 0.0043 M…

A: Given , acid ionisation constant , Ka= 5.0×10-5 concentration of the Sc(NO3)3= 0.0043 M

Q: You have a solution of nitrous acid (HNO2). What effect will addition of sodium nitrite (NaNO2) have…

A: We know that, HNO2 is nitric acid and it is dissociate partially in water to given H+ ion and NO2-…

Q: Determine the pH of a 0.0525 M Fe(NO3)3 solution. The Ka for Fe3+ is 6.3 x 10^-3. What is the pH?

A: Reaction of ferric nitrate in water is given below Fe3+ is formed from Fe(NO3)3.

Q: What is the pH of a 1.20 M nitrous acid solution? (Ka = 4.50 x 10-4)

A:

Q: The acid dissociation K, of acetic acid (HCH,Co, is 1.8 x 10 a Calculate the pH of a 2.6 x 10 M…

A: Acetic acid is a weak acid. hence it will dissociate partially as per the reaction  CH3COOH ---->…

Q: What is the pH of a 0.680 M solution of Ca(NO2)2 (Ka of HNO2 is 4.5 x 104)?

A: Given, The pKa value of HNO2=4.5×10-4 Molarity of Ca(NO2)2= 0.680M.

Q: 34. The equilibrium constant for the autoionization of water at some temperature below the room…

A: Given data, Kw=1.2×10-15 pOH = ?

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.