The pH of a basic solution is 12.83. What is [OH ]?

Q: The pH of a basic solution is 12.03. What is [H⁺]?

A: Given: pH of solution = 12.03

Q: 69. A 0.185 M solution of a weak acid (HA) has a pH of 2.95. Calculate the acid ionization constant…

A: A weak acid are those which does not completely dissociate to liberate H+ ion

Q: What are the pH and pOH of a solution of 2.0 M HI, which ionizes completely?

A:

Q: 12.9 g of NaOH was dissolved in water affording a final volume of 250 mL. What is the pH of the…

A: Given :-  mass of NaOH = 12.9 g  volume of solution = 250 mL  To calculate :-  pH of solution

Q: About 12% of the acid in a 0.10 M solution of a weak acid dissociates to form ions. What are the…

A: Given information: Dissociation = 12% Concentration = 0.10 M

Q: The hydronium ion concentration in an aqueous solution at 25°C is 1.1×10-3 M. The hydroxide ion…

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 5.3x10-2 M. The hydronium ion…

A: Ionic product of water ( Kw ) :-  The product of hydronium ion concentration and hydroxide ion…

Q: The hydronium ion concentration of vinegar is approximately 4 × 10−3 M. What are the corresponding…

A: Given : hydronium ion concentration i.e [H3O+ ] = 4 X 10-3 M

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 1.1×10-2 M. M. The hydronium ion…

A: The pH of a substance can be expressed as the negative log of the hydrogen ion concentration. It is…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 8.3×10-2 M. The hydroxide ion…

A: The pH is a method that helps in determining whether the given solution is acidic or basic. Given…

Q: The compound methylamine is a weak base like ammonia. A solution contains 0.263 M CH,NH3* and 0.204…

A:

Q: The hydronium ion concentration in an aqueous solution at 25°C is 6.3×10-2 M. The hydroxide ion…

A: EXPLANATION: At 25oC ,It is always true. GIVEN: To Solve: Hydroxide ion concentration(M)=?pH of…

Q: The pH of a basic solution is 9.03. What is [H*]?

A:

Q: Calculate the pH of an aqueous solution that is 0.70 M sodium hypochlorite.

A: The given compound Sodium hypochlorite (NaClO) is a strong electrolyte. So, it dissociates…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 4.2×10² M. The hydroxide ion…

A: Given that:  [H3O+] = 4.2×10-2 M

Q: Calculate the pH of an aqueous solution of 0.0448 M potassium sulfite.

A: PH is defined as negative logarithms of hydrogen ion concentration.

Q: The pH of a basic solution is 12.49. What is pOH?

A:

Q: The compound methylamine is a weak base like ammonia. A solution contains 0.199 M CH3NH3* and 0.117…

A: TThe base is the substance that gives OH- or accepts H+ ions in solution. The Henderson Hasselbalch…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 1.4×10-4 M. The hydroxide ion…

A: The formula that will be used : pH = -log(H3O+)  pOH = -log(OH-)  pH + pOH = 14 Given, H3O+ = 1.4 x…

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 9.3×10-2 M. The hydronium ion…

A: Given : Hydroxide ion concentration [OH-] = 9.3 × 10-2 M.  a)  Hydronium ion concentration [H3O+] =…

Q: The pH of a basic solution is 12.29. What is [OH]?

A: pH + pOH = 14

Q: The pH of an aqueous solution at 25°C was found to be 4.60. The pOH of this solution is The…

A: We will calculate all the required terms.

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 9.7×10-2 M. The hydronium ion…

A: Given, Hydroxide ion concentration [OH-] = 9.7 X 10-2 M T = 250 C So we've given the concentration…

Q: The pH of a basic solution is 10.89. What is [H*]?

A: The pH of any solution is given by  pH = -log[H+] where [H+] = concentration of H+ ions in the…

Q: The hydronium ion concentration in an aqueous solution at 25°C is 4.7×10-2 M. The hydroxide ion…

A: The pH is a method that measures the acidity or basicity of a given solution. Given data - The…

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 3.2×10-2 M. The hydronium ion…

A: Concentration of OH- in aqueous solution is 3.2*10-2M.

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 3.8×10-2 M. The hydronium ion…

A: Acid strength depends in concentration of hydronium ions. The following formula is used,  pH…

Q: The pH of a basic solution is 9.03. What is [H1?

A: formula used:-  pH = -log[H+]

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 7.4×103 M. The hydronium ion…

A: 1. We are having the hydroxide ion concentration as 7.4*10-3 M We have to calculate the hydronium…

Q: The pH of an aqueous solution of 0.124 M ammonium nitrate, NH4NO3 (aq), is ___________. This…

A:

Q: The pH of a basic solution is 11.39. What is [OH-]?

A:

Q: If 215 ml of a .01M HBr is reacted with 250 ml of a .007M solution of KOH, what is the resulting pH?

A: HBr    +      KOH            →           KBr  +  H2OINITAL         215×.01…

Q: If 990. mL of water is added to 10.0 mL of 0.10 M HCl, what is the pH of the resultant solution?

A: Given that,  Volume of water = 990 mL Volume of 0.10 M HCl = 10.0 mL When volume of water and HCl…

Q: The pH of a solution with a [OH–] concentration of 1.20 x10–6 M are___, respectively.

A:

Q: The hydronium ion concentration in an aqueous solution at 25°C is 3.4×10 M. The hydroxide ion…

A:

Q: The pH of a basic solution is 10.15. What is pOH?

A: We have, the pH of a basic solution = 10.15We need to calculate it's pOH value.

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 5.1×10-² M. The hydronium ion…

A: Given:  [OH-] = 5.1 x 10-2 M  At 25°C :Kw = 10-14  Also, Kw = [H3O+][OH-]

Q: The pH of an aqueous KOH solution is 12.38. What is the hydrogen ion concentration of this solution?

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 3.4×10-2 M. The hydronium ion…

A:

Q: The pH of a solution of 0.50 M  NH4Cl  is

A: NH4Cl dissociates as follows: Ka of NH3 is 5.6×10-10 Thus concentration of HCl is 1.67×10-5 M.

Q: The pH of a basic solution is 9.77. What is [OH⁻]?

A: we know, pH + pOH = 14 pOH =  -log[OH-]

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 4.6×10-² M. The hydronium ion…

A:

Q: The pH of a basic solution is 11.29. What is pOH?

A: The pH scale varies from 0 to 14 where if the pH value is less than 7 which means the solution is…

Q: The pOH of a basic solution is 2.81. What is pH?   The pOH of an acidic solution is 11.55. What is…

A:

Q: What will be the pH value of the solution if we have added aqueous NH4Cl to a neutral solution and…

A:

Q: The pH of a basic solution is 12.89. What is [H⁺]?

A:

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 2.1×10-3 M. The hydronium ion…

A: Given, The concentration of the hydroxide ion, [OH-] = 2.1×10-3 M Concentration of the hydronium…

Q: The concnetration of NaOH solution is 1.0 M. What will be the pH of solution?

A: NaOH is a strong base , so we would first calculate its pOH using the formula : pOH = - log [OH-]…

Q: The hydroxide ion concentration in an aqueous solution at 25°C is 3.9×10² M. The hydronium ion…

A: • The values provided in the question are:-    i) Hydroxide ion concentration of a solution, [OH-] =…

Q: The pH of an aqueous solution of 0.176 M ammonium bromide, NH Br (aq), is This solution is

A: 1. Solution - According to the question - pH = pH stand for potential of hydrogen, since pH is…

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.