A solution with a pH of 2.17 is

Q: The pH of a basic solution is 9.77. What is [H+]?

A:

Q: Determine the pH for the following: a single solution prepared to final concentrations of 0.03417 M…

A: Given : Concentration of HCl = 0.03417 M And concentration of H2SO4 = 0.03417 M Since both acids are…

Q: A solution contains 0.119 M ammonium chloride and 0.126 M ammonia. The pH of this solution is

A: The given data contains, Molarity of ammonium chloride = 0.119 M. Molarity of ammonia = 0.126 M pKb…

Q: A solution is prepared by diluting 0.55 mol HNO3 with water to a volume of 1.75L. What is the pH of…

A: Molarity = Number of moles of solute/Volume of solution in L pH = -log[H+]

Q: The pH of a solution of 0.200 M NaOH is __________.

A: • The values provided in the question are:-     i) Concentration of sodium hydroxide solution,…

Q: A 0.135 M solution of a weak base has a pH of 11.23. Determine Kb for the base.

A: Weak base are those which do not dissociate completely in water. For base concentration depend on…

Q: Calculate the pH of a solution t

A:

Q: What is [H⁺]?

A: Given :- pH = 11.65  To calculate :- [H+]

Q: Calculate the pH of a solution that is 0.0330 M in

A: In all cases formula for weak acid to calculate pH is to be used. a. pH = 0.5pKa-0.5logC =…

Q: The pH of a solution is is 12.5. What are the hydronium ion and hydroxide ion concentrations in the…

A: At 25 degree Celsius.                                          PH + POH = 14.…

Q: A solution contains 0.392 M NH¸I and 0.134 M ammonia. The pH of this solution is

A:

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: MOH base solution is 0.02 M with an ionization degree of 0.02. The pH of the base solution is

A:

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

A:

Q: The pH of a basic solution is 10.33. What is [H]?

A: Given details, The pH of the base solution [OH-] = 10.33 To calculate the [H+].

Q: Given, pH of a solution Á is 3 and is mixed with another solution Bhaving pH 2. If both are mixed,…

A: Introduction: The given data : The pH of the solution A = 3 The pH of the solution B = 2 To…

Q: What is the pH of a 0.627 M weak base solution? The Kb of the weak base is 0.000066.

A: Given :- concentration of weak base solution = 0.627 M  Kb for weak base = 0.000066  To calculate :-…

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

A:

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: The pH of a basic solution is 8.11. What is [H⁺]?

A: An acidic substance is the substance that can give H+ ions. They are corrosive and sour in nature.…

Q: What is the concentration of a solution of (a) KOH for which the pH is 11.89,

A: We know that, the pH of the solution is equal to the negative log10 of the hydrogen ion…

Q: The pH of a basic solution is 10.41. What is [OH⁻]?

A: pH of a solution is the parameter which is used to define the acidity or basicity of a solution.…

Q: If a solution has a proton concentration of 0.00156 M, what is the pH?

A: pH is a scale to measure the concentration of hydrogen ions. The negative logarithm of hydrogen ion…

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

A: pH + pOH = 14

Q: If the ?b of a weak base is 5.9×10−6,5.9×10−6, what is the pH of a 0.28 M 0.28 M solution of this…

A:

Q: What is the pH of a uffer solution

A: The pH is as calculated below:

Q: Determine the pH of a solution that is 3.85% KOH by mass. Assume that the solution has density of…

A:

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: A solution contains 0.281 M ammonium bromide and 0.480 M ammonia. The pH of this solution is

A: Given data contains, Concentration of ammonium bromide is 0.281 M. Concentration of ammonia is 0.480…

Q: Also, is the solution acidic, basic, or neutral?

A: HClO4 is an strong acid, dissociate as - HClO4 --------> H+ + ClO4-   The concentration of the…

Q: An aqueous solution contains 0.411 M Na,HPO4 and 0.436 M H,PO4. The pH of this solution is

A:

Q: Calculate the concentration of an aqueous solution ofNaOH that has a pH of 11.50.

A: Given: pH of NaOH solution is 11.50

Q: Determine the pH of the following: 1.00 × 10–6 M KOCl solution

A: We have to determine the pH of the following: 1.00 × 10–6 M KOCl solution

Q: a solution with a pH of 12.0 is

A: Answer to the following question is given as:

Q: A solution contains 0.145 M ammonium chloride and 0.108 M ammonia. The pH of this solution is

A:

Q: A solution contains 8.64x102 M potassium nitrite and 0.370 M nitrous acid. The pH of this solution…

A:

Q: Calculate the pH of the following solutions.  - 0.020 M HCl

A: Hydrogen ion concentration is an important parameter of an aqueous solution. The concentration of…

Q: The pH of a basic solution is 13.11. What is the (H+)

A:

Q: The pH of an acidic solution is 4.17. What is pOH?

A: pH and POH is defined for acid and base. We have relation between them so we will use the same

Q: A solution contains 0.354 M potassium cyanide and 0.401 M hydrocyanic acid. The pH of this solution…

A: The given problem can be solved by using Henderson-Hasselbalch equation as; pH = pKa + log SaltAcid…

Q: 2. A solution with a pH of would be considered an acid. Оз 8 10

A: Answer - The correct option is (a)  = 3 Explanation - The scale has values ranging from zero (the…

Q: The pH of a basic solution is 12.51. What is pOH?

A:

Q: If pH of solution is 13, it means that if is:(a) Weakly acidic(b) Weakly basic(c) Strongly acidic(d)…

A: 1. To determine the acidity and basicity of the solution, the concept of pH was introduced. 2. pH…

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: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0194 M solution. The pH of the…

A: Given, a weak monoprotic acid is dissolved in enough amount of water to make the aqueous solution.…

Q: Calculate the pH of a solution with a hydrogen ion concentration of 0.0003 M

A: Given  concentration of hydrogen ion = 0.0003 M We have to calculate the pH of solution.

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

A:

Q: The pH of a basic solution is 12.39. What is [H*]?

A: The question is based on pH determination of a solution pH is defined as negative logarithmic of…

Q: A solution contais 0.0111 grams of strong base calcium hydroxide completely dissolved in 635 ml of…

A: Given,Calcium hydroxide = 0.0111 grams,Volume = 635 ml.Molar mass of 74.093 g/mol.Equivalent Weight…

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.