What is the pH of a 2.4 M solution of H2CO3? (Ka of H2CO3 = 4.3 x 10-7, Ka of HCO3- = 7x 10-11)

Q: Calculate the [H3O+] of a 0.390 M acid solution; Ka=4.52 x10-5

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Q: The hydronium ion concentration of an aqueous solution of 0.402 M hypochlorous acid (Ka = 3.50×10-8)…

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Q: What is the pH of a solution that contains 0.10 M HCl and 0.10 M acetic acid (HC2H3O2)? Ka for…

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Q: What is the pH when the [OH-] = 4.26 x 10-2 M at 25 oC?

A: 1- First we need to calculate the pOH of the solution :  We know that,  pOH = -log[OH-]  pOH = -log(…

Q: What is the percent ionization of H2NNH2 in a solution with a concentration of a 0.630 M? (Kb = 1.3…

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Q: What is the Ka of cyanuric acid if a 0.030 M cyanuric acid aqueous solution has a pH of 4.15? O…

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Q: 7. The [OH-] of a solution is 1 x 10-2 M. Which of the following is correct? (A) The solution is…

A: Given,  The concentration of OH- , [OH-] = 10-2 M We know that, pOH = - log [OH-]  pOH + pH = 14…

Q: A diprotic acid (H₂A) has Kai - 4.55 x 10-7 and K₁2 = 6.07 × 10-¹¹. What is the pH of a 0.463 M H₂A…

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Q: Calculate the pH of a 0.512 M solution of a triprotic weak acid, H3A, given the acid ionization…

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Q: What is the pH of 0.024M acetic acid solution at 25°C? (Ka=1.8×10^-5)

A: Given, [CH3COOH] = 0.024 M Ka = 1.8 × 10-5

Q: What is the pH of 0.75 M HC2H302 solution? K.= 1.8 x 105 and Kn=1.00 x 10-14 HC2H3O2 + H2O H3O* +…

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Q: Propanoic acid HC3H5O2, has a Ka of 1.3 x 10-5. What is the [H3O+] in a (1.51 x 10-1) M solution of…

A: The ionization of Propanoic acid HC3H5O2 takes place as,                             HC3H5O2 (aq)  +…

Q: A 1.00 L solution contains propanoic acid (C3 H5 O2 H) with a concentration of 0.350 mol/L, and…

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Q: What is the pH of a solution that is 0.400 M in NH3 and 1.450 M NH4*? Ka= 5.7x1010

A: Given :-  Concentration of NH3 = 0.400 M  Concentration of NH4+ = 1.450 M  Ka = 5.7 × 10-10  To…

Q: 2- Calculate the hydronium ion concentration and the pH of a 10-2 M NaH2A solution. Given: The…

A: pH of salt solution of weak acid and strong base is calculated using respective formulas.

Q: What is the concentration (in M) of hydroxide ions in a solution at 25.0 °C with a pH of 3.58? O…

A: pH is defined as negative logarithm of hydrogen ions present in the solution.

Q: What is the PH of a 0.13 solution of the salt NaX? Ka of HX= 1.5×10^-5

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Q: What is the pH of a 0.139 M solution of HF? Ka for Hf is 6.6 x 10-4

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Q: what is the pH of 0.12795M CH3COOH solution? Ka=1.8x10^-5

A: We have to calculate the pH.

Q: What is the pH of a solution with [H^+]= 6.95×10^-11M?

A: Given, [H+]= 6.95×10-11 M We know that, pH = -log(H+)

Q: For the diprotic weak acid H₂A, K₁1 = 3.8 x 10-6 and K₁₂ = 7.7 x 10-⁹. What is the pH of a 0.0750 M…

A: Given,  The concentration of H2A = 0.0750 M.  Ka1 = 3.8 × 10-6  and  Ka2 = 7.7 × 10-9  The pH of the…

Q: Chlorous acid, HC1O2, has a K. = 1.2 × 10-2.Calculate the pH when 0.15mol of HC1O2 is dissolved in 1…

A: The concentration of HClO2 is calculated as, Concentration = No. of molesVolume (L)Concentration =…

Q: What is the pH value of 1x10-3 M CH3COOH solution? (Ka: 1.75x10-5)

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Q: Determine the pH

A: The scale which is used to analyze the acidity and basicity of an aqueous solution is called as pH…

Q: What is the concentration of h3o+ in a solution with a ph of 4.0 ?

A: Given :- pH = 4.0  To calculate :- concentration of H3O+ i.e. [H3O+]

Q: The pH of a 0.25 M aqueous solution of HF at 25°C is 2.03. What is the value of Ka for HF?     3.7…

A: pH gives the information about the acidity or alkalinity of a solution. pH is determined from the…

Q: What is the percent ionization of H¿NNH2 in a solution with a concentration of a 0.530 M? (Kb = 1.3…

A: Weak base dissociate partially in solution. The degree of ionization is not complete in such…

Q: Trichloroacetic acid (CCl3COOH) is a corrosive acid that is used to precipitate proteins. The pH of…

A: Given information: Concentration of HClO4 solution = 0.040 M Concentration of CCl3COOH solution =…

Q: -3 Calculate the pH of a 3.6 x 10-M solution of H2SO4 (Ka, = 1.2 x 10-2). pH =

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Q: The Ka for hydrofluoric acid is 7.1 × 10−4. Calculate the pH of a 0.15-M aqueous solution of…

A: pH: It is defined by saying that power of hydrogen present in any solution. It can be calculated…

Q: Determine the [H3O⁺] in a 0.265 M HClO solution. The Ka of HClO is 2.9 × 10-8.  Determine the pH of…

A: Given,Concentration of HClO = 0.265 MKa = 2.9 × 10-8The chemical reaction of dissociation of…

Q: what is the pH of 10-12M H3O+ solution

A: The pH of a solution is calculated by the formula: pH=-logH3O+......(1)

Q: What is the pH of a 0.150 M NH4Cl solution? Kb of NH3 = 1.76 × 10−5

A: Given, Concentration of NH4Cl solution (C) = 0.150 M Kb for NH3 = 1.76 × 10-5 pH of a NH4Cl solution…

Q: Calculate the pH of a 0.236 M solution of a triprotic weak acid, H3A, given the acid ionization…

A: Given,   The pH of a 0.236 M solution of a triprotic weak acid, H3A is:   the acid ionization…

Q: What is the pH of a solution if [OH-]=2.4 x 10-6?

A: pH of any solution in terms of [OH-] is given by  pH = 14 + log[OH-] where [OH-] = concentration of…

Q: A solution of acetic acid has a pH of 3.45. What is the concentration of acetic acid in this…

A: Given: The pH of the given acetic acid solution is 3.45 The Ka of acetic acid is 1.8*10-5

Q: 5. What is the approximate ratio of [A]/[HA]ions in a 0.10 M aqueous solution of H2A? Assume that…

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Q: Calculate the pH of a 0.600 M solution of Na2S k1 of H2S=9.6x10^-8 k2 of H2S=1.3x10^-14

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Q: 3. What is the pH in a solution with [H*]=2.5x10-5? %3D

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Q: NH3(aq) + H₂O(1) ⇒ NH(aq) + OH- (aq) The equilibrium hydroxide concentration in a 0.0220 M NH3…

A: Concept based on the dissociation constant of an weak base.

Q: . What is the pH of a solution consisting of 0.85M HC2H3O2 and 0.60M NaC2H3O2? Ka of HC2H3O2 = 1.8 x…

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Q: Determine the pH of a 0.461 M C6H5CO2H M solution if the Ka of C6H5CO2H is 6.5 x 10-5.

A: Given,Concentration = 0.461M.Ka = 6.5×10-5Then,

Q: Calcualtw the pH of a 0.217 M HC7H5O2 aqueous solution. Ka for HC7H5O2 is 6.5 x 10^-5.

A: pH of an acid is equal to negative logarithm of concentration of H+ ions.

Q: What is the hydronium ion concentration [H3O+] of a 0.010 M acetic acid solution in water? (Ka for…

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Q: If a 0.06 M solution of a weak acid has a pH of 5.64, what is the Ka of the acid? HA    <=>…

A: since pH = -log[H+] where [H+] = concentration of H+ ions in the solution  => 5.64 = - log[H+]…

Q: For the diprotic weak acid H₂A, Kal = 2.8 x 10-6 M and K₁2 = 8.9 x 109 M. What is the pH of a 0.0450…

A: Introduction :  Diprotic acid are those acids which produces two moles of hydrogen when they are…

Q: What is the pH of a solution that is 0.11 M CH3NH2 (methylamine) and 0.15 M CH3NH3Cl (methylammonium…

A: Since the solution is having weak base CH3NH2 and its conjugate acid salt CH3NH3Cl  Hence the…

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.