The acid-dissociation constant for chlorous acid, HClO2, at 25C˚ is 1.0×10-2 . Calculate the concentration of H+ if the initial concentration of acid is 0.100 M

Q: Determine the pH of a 0.120M solution of lithium lactate. The Ka for lactic acid is 1.38x10-4.

A: Concentration of lithium lactate = 0.12 M Ka for lactic acid is 1.38x10-4Determine pH of solution

Q: The acid-dissociation constant, Ka, for a particular acid is 4.57 x 10. What is the…

A: We know that,  Ka × Kb =10(-14) Given that, Ka = 4.57 × 10(-3) So,

Q: The

A: Phosphoric acid is a polyprotic acid. It's last dissociation so slow so that's why we can not…

Q: 2. 50 x 10-5 , wha

A: Given data are as follows: Concentration of acidic solution = 0.05 M Ionization constant = 2. 50 x…

Q: A solution of sodium acetate (NaCH3COO) has a pH of 9.44. The acid-dissociation constant for acetic…

A:

Q: Citric acid, C6H8O7 (aq), is sued to add a sour taste to foods and soft drinks. It is prepared in a…

A: Given  Concentration (c)= 0.52 M pH = 1.72 Ka =?

Q: What is the percent ionization of a monoprotic weak acid solution that is 0.171 M? The…

A: We will first construct the ICE table. It will help us to write the equilibrium expression of the…

Q: The weak base (CH3)2NH has a Kb = 5.9 x 10−4 at 25 °C. a) Write out the chemical equation for the…

A: We have to write chemical reaction for protonation of given amine.   We have to predict the…

Q: The pH of an aqueous solution of 0.324 M diethylamine (a weak base with the formula (C₂H5)2NH) is

A: we have to calculate  pH of diethylamine  hydroxide ion concentration for hydroxylamine

Q: What is the ionization constant at 25 ◦C for the weak acid (CH3)2NH3 +, the conjugate acid of the…

A: The expression for the ionic product of water is as follows,                                   Kw =…

Q: A sample of Ca(OH)2 with a mass of 0.151 g is dissolved in water so that the volume of the solution…

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Q: What is the pH (to two decimal places) of pure water (at 25 °C)? 2H2O(l)⇌H3O+(aq)+OH−(aq)…

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Q: Ammonium (NH3) has Kb = 1.8 x 10–5. What is the pH of a solution that contains the molar ratio of…

A: The equilibrium between the weak acid and its conjugate base allows the solution to resist changes…

Q: The compound dimethylamine, (CH3),NH, is a weak base when dissolved in water. Write the K expression…

A: The ionization of weak base can be given by, Where B is the weak base and HB+ is its conjugate…

Q: Determine the OH-, pH, and pOH of a solution with a H+ of 4.5 x 10-6 M at 25 °C. [OH"] = pH = pOH =

A: Solution pH and pOH defined as the   negative log of concentrations of hydrogen or hydronium ions.…

Q: What is the percent ionization of a monoprotic weak acid solution that is 0.165 M? The…

A: Interpretation -  To determine the percent ionization of a monoprotic weak acid solution that is…

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

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Q: Ka for nitrous acid, HNO2, is 4.50 × 10-4. Ka for hydrofluoric acid, HF, is 7.20 × 10-4. Ka for…

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Q: The pH of a 0.0040 M solution of Ca(OH)₂ is

A: Given, Concentration of Ca(OH)2 solution = 0.0040 M So, [OH-]= 2×0.0040 M= 0.0080 M

Q: The Ka of hydrazoic acid (HN3) is 1.9 × 10−5 at 25.0 °C. What is the pH of a 0.35 M aqueous solution…

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Q: Calculate the concentrations of all species in a 0.510 M NaCH, COO (sodium acetate) solution. The…

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Q: A chemist must prepare 550.0 mL of nitric acid solution with a pH of 0.80 at 25 °C. He will do this…

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Q: Calculate the concentrations of all species in a 0.990 M NaCH,COO (sodium acetate) solution. The…

A: NaCH3COO is salt and hence dissociates completely. The concentration of CH3COONa is 0.990 M. So the…

Q: What is the pH (to two decimal places) of a 0.15 M NH3 and 0.15 M ammonium chloride aqueous solution…

A: The pH of buffer can be calculated by using Handerson equation . Ammonia and ammonium chloride forms…

Q: Calculate the equilibrium concentration of the nonionized bases and all ions in a solution that is…

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Q: molarity

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Q: HClO is a weak acid (?a=4.0×10^−8) and so the salt NaClO acts as a weak base. What is the pH of a…

A: Given : Concentration of NaClO = 0.014 M Since NaClO is a weak conjugate base of weak acid HClO.…

Q: Write the expression for the acid-dissociation constant Ka for HC4H7O2. (Concentration equilibrium…

A:

Q: The acid dissociation constant K, of acetic acid (HCH,Co,) is 1.8 × 10. Calculate the pH of a 0.48M…

A: Given :  Concentration of acetic acid = 0.48 M  Ka of acid = 1.8 x 10-5   To calculate :  pH of…

Q: calculate the percent ionization of nitrous acid in a solution that is 0.249M in nitrous acid. the…

A: [HNO2] = 0.249 M Ka = 4.50 x 10-4

Q: concentration

A: pH + pOH = 14  pOH = 14 - pH  pOH = 14 - 4.282  pOH = 9.718

Q: Calculate the magnitude of the equilibrium constant for benzoic acid, HC7H5O2, if a 0.100 M solution…

A: The benzoic acid represented as C6H5COOH. It is a weak acid and dissociate into hydrogen and…

Q: What is the ionization constant of a weak acid [HA], when its conjugate pair has a Kb value of 4.4 x…

A: In the ionization of a weak acid HA, A- is produced as a conjugated base.  HAAcid →Ionization…

Q: The acid dissociation constant K, of acetic acid (HCH3CO,) is 1.8 x 10. Calculate the pH of a 0.52M…

A: Given that : The acid dissociation Ka of acetic acid = 1.8 x 10-5 We have to calculate the pH of a…

Q: HClO is a weak acid ( ?a=4.0×10^−8 ) and so the salt NaClO acts as a weak base. What is the pH of a…

A: pH of a solution of a salt of weak acid and strong base:pH = 7 + (pKa + logC)/2

Q: B/ The acid-dissociation constant for chlorous acid, HClO2, at 25C° is 1.0×10-2. Calculate the…

A: Given the acid dissociation constant of HClO2, Ka = 1.0*10-2  Initial concentration of HClO2 = 0.100…

Q: What is the pH of a 0.025 M aqueous solution of sodium propionate, NaC3H5O2? The Ka of propionic…

A: Sodium propionate is a salt of weak acid and strong base. Given, Ka of propionic acid = 1.3x10-5…

Q: Calculate the pH of a 0.218 M solution of NaNO₂. The ionization constant, K,, for the acid, HNO₂, is…

A: Molarity of NaNO2 = 0.218 M Ka for HNO2 = 4.60×10-4 pH of NaNO2 solution = ?…

Q: What is the pH of a 0.0930 M solution of methylamine (CH₃NH₂, Kb = 4.4 × 10⁻⁴)?

A:

Q: The pH of water should be around 7. What does this mean about the concentration of H+ and  OH- ions…

A: Given : pH of water is 7  To find : Relate it to Concentration of H+ and OH- Solution : pH stands…

Q: A 9.5×10−2 MM solution of a monoprotic acid has a percent dissociation of 0.56%. Determine the acid…

A:

Q: The compound methylamine, CH3NH2, is a weak base when dissolved in water. Write the K₁ expression…

A: Since, Weak base equilibrium constant or Kb is the ratio of the equilibrium concentrations of…

Q: The Bronsted-Lowry definition of acids and bases refers to the transfer of a "proton" from the acid…

A: The acid that donates a proton is known as Bronsted Lowry acid. The base that gains a proton is…

Q: NH3 is a weak base ( ?b=1.8×10−5 ) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Ammonium chloride (NH4Cl) is a salt of a weak base (NH3) and a strong acid (HCl).When NH4Cl…

Q: Find the H3O+H3O+ concentration of a 0.220 MM  hypochlorous acid solution (whose acid dissociation…

A:

Q: For questions 7-9 state which species (chemical) is the acid, which is the base, and which are the…

A: Bronsted Lowry acid-base theory. Acid is the chemical species that donates protons in the solution…

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.