A solution is made by dissolving 0.0860 moles of Ba(OH)2 in enough water to make 755 mL of solution. What is the pH of the resulting solution?

Q: If the K, of a weak base is 3.8 x 10–6, what is the pH of a 0.21 M solution of this base? pH =

A: In this question we have to calculate the pH of Solution of base of given concentration, the Kb of…

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

A:

Q: The pH of a solution that contains 0.010 M H3O+ is

A: The concentration of [H3O+] = [H+] = 0.01 M.

Q: A solution is made by dissolving 0.02500 moles of Ba(OH)2 in enough water to make 750. ml of…

A:

Q: What is the pH of a solution prepared by adding 25.0 mL of 0.10 M HNO3 to 40.0 mL of 0.10 M NH3(aq)?

A: The reaction takes place in the solution prepared by mixing HNO3 and NH3 solutions is written…

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: What is the pH of a barium hydroxide solution obtained by dissolving 0.27 grams of barium hydroxide…

A:

Q: The pH of a 0.0057 M solution of Ca(OH)₂ is

A: Given- Concentration of Ca(OH)2= 0.0057 M

Q: A solution is made by dissolving 0.06100 moles of Ba(OH)2 in enough water to make 250.0 mL of…

A: Given, moles of Ba(OH)2 = 0.06100 moles Volume of the solution = 250.0 mL = 0.250 L pH of the…

Q: Suppose 0.100 mol of NaCH3COO is dissolved in enough water to make 1.00 L of solution. What is the…

A: pH is referred to the potential of hydronium ion and is calculated by taking the negative log value…

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

A:

Q: (a) When 6.3 g of nitric acid are dissolved in water to produce 500.0 mL of solution, what is the…

A: pH of solution is defined as the concentration of hydronium ion H3O+ present in the solution.

Q: The pH of a basic solution is 9.93. What is [OH ]?

A:

Q: The pH of an aqueous solution of 0.393 M nitrous acid is

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Q: What is the pH of a 0.105 M solution of acetic acid? What is the percent ionization of the acid?

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Q: The pH of a solution of household ammonia, a 0.950-M solution of NH3, is 11.612. What is Kb for NH3.

A:

Q: What is the pH of a 0.00065 M solution of HI?

A: The pH of the solution has to be calculated,

Q: Calculate the pH of a solution prepared from 0.200 mol of NH4CN and enough water to make 1.00 L of…

A: NH4CN is a salt of weak acid HCN and weak base NH4OH. pH of a salt of weak acid (WA)and weak base…

Q: The pH of a basic solution is 10.59. What is pOH?

A: The sum of pH and pOH for a solution is equal to 14. pH + pOH = 14 Given that,pH = 10.59

Q: A solution is prepared by dissolving 0.00050 mol KOH in enough water to prepare 500.0 mL of…

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: What is the pH of 0.32M solution of barium hydroxide?

A: The pH of a solution indicates the acidity or basicity of a solution, which is measured using…

Q: If the K, of a weak base is 2.7 x 10, what is the pH of a 0.30 M solution of this base?

A: Solution Ph may be a live of however acidic or basic is AN solution.It is measured in terms of…

Q: If the hydroxide concentration of a solution is [OH-] = 4.67 X 10-8 what would the pH of that…

A: Given:The concentration of OH, [OH-] = 4.67 X 10-8To find:pH = ?

Q: If enough HCl was added so that the concentrations of NH3 and NH4+ were 0.082 M and 0.017 M,…

A: An aqueous solution containing a mixture of weak base NH3 and its conjugate acid NH4+ leads to the…

Q: If a sample of a certain solution is determined to have a [H3O+] concentration of 5.6×10^−12…

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: 5 mg of HNO3, which is a strong acid, is added to 750 ml of water. What is the final pH of the…

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Q: Calculate the pH of a solution made by adding 2.50 g of lithium oxide 1Li2O2 to enough water to make…

A: The pH of a solution is a measure of hydrogen ion concentration, which in turn is a measure of its…

Q: Question attached

A: Phenol also known as carbonic acid having formula of HC6H5O is a weak acid . Given, Ka (Acid…

Q: If 100 ml of an aqueous solution of HNO3 contains 0.0056 moles, what is the pH?

A: Given Volume of HNO3 solution = 100 mL = 0.1 L Moles of HNO3 = 0.0056 moles pH of the solution = ?…

Q: Provided that a chemist prepared a 1.00 M acetic acid solution (HC2H3O2) wherein he found out that…

A: The weak acids are those that partially dissociate in aqueous solution to give protons. The pH is…

Q: What is the pH of a solution in which 43 mL of 0.33 M NaOH is added to 13 mL of 0.170 M HCl?

A: Moles of NaOH and HCl are determined as follows,

Q: What is the pH of a solution made by diluting 27 mL of 0.57 M HClO4(aq) to a total volume of 250 mL?

A: Since HClO4 is a strong acid and hence on diluting it will dissociate completely producing H+ ions…

Q: What is the pH of a 4.7 × 10⁻⁶ M KOH solution?

A: The concentration of KOH solution = 4.7 × 10−6 M pH of KOH solution = ?

Q: What mass in grams of nitric acid is present in 700 mL of a solution with a pH of 1.866?

A:

Q: A solution is made by dissolving 0.05700 moles of Ba(OH)2 in enough water to make 330.0 mL of…

A:

Q: Calculate the pH of a solution (aq., 25 oC) when 50.00 mL of 0.150 M HClO4 is added to 30.00 mL of…

A: Normality = n factor * Molarity  for HClO4 , n factor =1  for Ba(OH)2 , n factor =2

Q: Calculate the pH of a solution made by adding 2.70 g of lithium oxide (Li2O) to enough water to make…

A: Mass of lithium oxide = 2.70 g Volume of solution = 1.300 L

Q: What is the pH of a 0.00165 M solution of NaOH?

A:

Q: A solution is made by dissolving 27.5 g of HONH₃ClO₃ in 500.0 mL of water. Determine the pH of the…

A: Given: Mass of HONH₃ClO₃ = 27.5 g Volume of Water = 500.0 mL To Calculate: The pH of the solution

Q: 1.00 L of hydrochloric acid is prepared and has a final pH of 1.045. What mass of HCl) is dissolved?…

A:

Q: an aqueous solution has a pOH = 6.8. The pH of this solution is ____

A: • The values provided in the question are:-      i) pOH of an aqueous solution = 6.8    • We need to…

Q: A barium hydroxide aqueous solution has pH of 10.87. Calculate its molar concentration

A:

Q: What is the pH of a 2.5 × 10⁻⁶ M KOH solution?

A: The formula for a aqueous solution under the standard conditions - Now calculate the pOH of the…

Q: The concentration of a strong monoprotic acid is 0.0010 M.  What is the [OH-]? What is the pH?

A: We calculate the pH of an acid or base using the Sorenson pH scale.…

Q: Calculate the the pH of a solution composed of 0.20 M ammonia and 0.15 M ammonium chloride?

A:

Q: a 0.365g sample of HCl is dissolved in enough water to give 2.00 x 10 ^2 mL of solution. what is the…

A: pH = -log[H+] [H+] = [HCl] = Number of moles of HCl/Volume of solution (L) Number of moles of HCl =…

Q: Calculate the pH of each of the following strong acid solution 0.225 g of HClO3 in 2.00 L of…

A: Given data contains, Mass of HClO3 is 0.225 g. Volume of the solution is 2.00L. The moles of HClO3…

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.