Calculate the pH of a 0.155 M  solution of KOH.   Calculate the pOH of a 0.155 M  solution of KOH.   Write both answers to at least two decimal places

Q: Calculate the pH value for a 1:1 mixture of O.003 M Ca(OH)2 (aq) and 0.001 M HCI (aq). Provide your…

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Q: If you know the [OH], how can you determine the pH of a solution? Match the words in the left column…

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Q: What is the pH of a solution with hydronium ion concentration equal to 0.0046 M.

A: Given :- concentration of hydronium ion in solution = 0.0046 M  To be calculated :- pH of solution

Q: Calculate the value of pOH for a solution of strong acid with an H3O+ concentration of 3.8 x 10-9 M.…

A: Given that : H3O+ = 3.8 x 10-9 M We have to calculate the pOH and identify whether the solution is…

Q: Calculate the [H3O+] ,[OH-], pH & pOH of a 0.10 M HCl.

A: pH = -log [H3O+]  [H3O+].[OH-] = kw  pOH = -log [OH-]

Q: The pH of a solution is 2.45. What is the molar concentration of hydronium ions in the solution?…

A: We have given that  pH = 2.45  [H3O+] = ?

Q: calculate ph of 0.15 M solution HCL at 25 degrees

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Q: A chemist dissolves 164. mg of pure nitric acid in enough water to make up 120. mL of solution.…

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Q: A solution has a hydrogen ion concentration of 5.1 × 10⁻⁵. Calculate the pOH of the solution. Please…

A: pH :-  The negative logarithm to the base 10 of hydrogen ion concentration expressed in mol/L of a…

Q: pH, [OH-], and pOH

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Q: A chemist dissolves 262. mg of pure hydrobromic acid in enough water to make up 390. mL of solution.…

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Q: Sid What is the pH of ammonium bromide solution with a concentration of 0.563 M. The base ionization…

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Q: What is the pH of a 0.0350 M NaOH solution? Use correct number of significant figures. Explain why…

A: The required relationships are given below. pH + pOH = 14 pOH = -log [OH-]

Q: Calculate the concentration of all species present and the pH of a 0.020-M HF Solution.

A: Concentration of HF = 0.020 MKa(HF) = 3.5 * 10-4Chemical reaction of HF in water Chemical Equation…

Q: The pH of an aqueous solution of 9.39×10-2 M ammonium nitrate, NH4NO3 (aq), is . This solution is…

A: 9.39×10-2 M is the concentration of ammonium nitrate, NH4NO3 (aq)

Q: Determine the [OH-], pH, and pOH of a 0.15 M ammonia solution

A: Construct ICE table and calculate the required values,

Q: List the factors that affect acid strength?

A: Acid is the one which accepts the electrons according to Lewis theory. According to Bronsted theory…

Q: Calculate the OH− concentration and pH of a 0.0025 M aqueous solution of sodium cyanide, NaCN.…

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Q: The pH of an aqueous solution at 25°C was found to be 6.70. The pOH of this solution is| The…

A: Provided pH=6.70 Concentration of H3O+=10-pH pOH = 14 - pH Concentration of  OH-= 10-pOH

Q: Determine the pH of an HF solution of each of the following concentrations. In which cases can you…

A: We need to calculate pH of HF. 1) 0.240 M 2) 0.0530 M 3) 0.0300 M

Q: For each of the following strong base solutions, determine [OH−],[H3O+][OH−],[H3O+], pH, andOH.…

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Q: The pH of an aqueous solution at 25°C was found to be 8.50. The pOH of this solution is The…

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

Q: For each of the following substances, identify whether the substance is classified as an Arrhenius…

A: According to Arhenius , acid are the substance  which release H+ ion and base are the substance…

Q: find the pH of the solution obtained by dissolving 2.24 liters of HCl gas under normal conditions in…

A: The question is based on concept of ideal gas equation and concentration. first we will calculate…

Q: Calculate the pH of a solution that is 0.142 M HCL?

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Q: Given a 0.25M solution of hydrochloric acid, determine the hydromium ion concentration of the pH.

A: The pH of the given solution can be defined as the measure of its basicity or the acidity. It is…

Q: 0.05 moles of Sr(OH)2 is dissolved in enough water to from 0.25L of solution. What is the pH of the…

A: Given that,  moles of Sr(OH)2 = 0.05 mol Volume of Sr(OH)2 solution = 0.25 L Molarity of Sr(OH)2…

Q: What are the major species present in 0.320 M solutions of each of the following acids? Calculate…

A: The major species in the solutions are those which coule be identified in large concentration. For a…

Q: Calculate the pH of solutions with the following hydronium ion concentrations: Remember to use the…

A: pH = - log [H+] This also can be written as,pH = -log[H3O+] Just substitute the hydronium ion…

Q: Which solution is most acidic (that is, which one has the lowest pH)? 0.80 M HCN 0.40 M HCN…

A: HCN is a weak acid but HNO3 is a strong acid. So, the most acidic will be HNO3 solution. We can…

Q: For each of the following compounds, indicate whether a 0.100 M aqueous solution is acidic (pH 7),…

A: 1) 0.100 M HCl Calculation of pH: pH=-log[H+]=-log0.1=1 Since pH < 7, thus the solution is…

Q: What is the pH, pOH, [OH-], and [H+] of a 0.006M solution of HNO3

A: pH of any solution tells about the acidity of that solution. Less is the pH more acidic is the…

Q: For an aqueous solution of 0.045 M HNO3, calculate the values of the following parameters:  [H+ ],…

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Q: The pH of an aqueous solution at 25°C was found to be 12.00. The pOH of this solution is . The…

A: Given: The pH of an aqueous solution at 25°C was found to be 12.00. To find : The pOH of this…

Q: For each of the following strong base solutions, determine [OH−] and [H3O+] and pH and pOH. 1.…

A: 1.Given, 1.15*10-2M Ba(OH)2

Q: Consider 0.010M solutions of HI, Nal, HSCN, and NaSCN. Which of the following lists shows these…

A: Acid is the substance having a pH value less than 7 while the base has a pH value greater than 7.…

Q: The pH of an aqueous solution at 25°C was found to be 5.50. The pOH of this solution is The…

A: A pH is a unit to the acidity of the solution. The expression to calculate pH are as follows:…

Q: The pOH of an aqueous solution at 25°C was found to be 13.00. The pH of this solution is The…

A: The solution is as follows :

Q: Determine the pH of an HF solution of each of the following concentrations. In which cases can you…

A: (a)ICE table for the reaction is given below.

Q: Which solution is most acidic (that is, which one has the lowest pH)? 0.30 M HF 0.60 M HF 0.30 M HBr

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Q: A chemist dissolves 237. mg of pure perchloric acid in enough water to make up 240. mL of solution.…

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Q: Calculate the pH of each solution given the following. [H3O+]=4.5×10−2M Express your answer…

A: The pH of a solution is determined by taking the negative logarithm of hydrogen or hydronium ion…

Q: Calculate the pH of a solution when 20 mL of a .1 M HCl are mixed with 40mL of a 0.05 M NaOH answer…

A: HCl mixed with sodium hydroxide

Q: Calculate the concentration of OH ions in a HCl solution whose hydrogen ion concentration is 1.40 M.

A: · We have HCl solution.· Hydrogen ion concentration = 1.40 M∘ We need to calculate the concentration…

Q: Calculate the concentration of H+ ions if the pOH of the solution is 3.56

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Q: What is the pH and pOH of each solution given the following [OH ]? Classify each solution as acidic,…

A: Given  pOH = -log [OH-] , pH = -log [H+] and pH + pOH = 14 1) [OH-] = 10-3 M using pOH = - log [OH-]…

Q: The pH of a solution is a measure of the molar concentration of hydrogen ions, H* in moles per…

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

Q: Calculate the pH of a solution when3.78grams of HCl was placed in 150.25 mL of water. HCl is a…

A: Solution -

Q: What is the [OH-] , [H+] and pH of a solution containing 0.00086M KOH

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

Q: A chemist dissolves 307. mg of pure perchloric acid in enough water to make up 200. mL of solution.…

A: Perchloric acid is HClO4  Given : Mass of HClO4 added = 307 mg = 0.307 g…

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.