Consider a 0.155 M LiCNO solution where Ka of HCNO = 2.0 × 10** Blocks a) Write the dissociation reaction of the salt, LICNO. b) Write the hydrolysis (ionization) reaction that occurs in the aqueous solution. c) Calculate the pH of a 0.155 M LİCNO solution.

Q: Hydrochloric acid, HCI, is a strong acid that completely dissociates in water and sodium hydroxide…

A:

Q: Determine the pH of a solution that is prepared by dissolving 8 g of Ba(OH)2 in 3.8 L water at 25°C.…

A: pH is given by: pH = 14 - pOH       = 14 - (-log[OH-])       = 14 + log [OH-]…

Q: Calculate the pH value of 0.01M Ba(OH), solution.

A: Given concentration of Ba(OH)₂ solution = 0.01 MTo find :pH Value of the above solution

Q: What is the pH of a 0.116 M solution of KOH?, and a 0.116 M solution of Ca(OH)2 ?

A: Step 1: Step 2:

Q: Calculate the pH of a solution formed by the reaction of 0.355 grams of sodium with water (see…

A: Given,

Q: Calculate the pH of a mixture that contains 0.23 M of HCNO and 0.16 M of HBrO. The ?a of HCNO is…

A: Given: Concentration of HCNO=0.23 MConcentration of HBrO=0.16 MKa of HCNO=3.5×10-4  Ka of…

Q: In a titration experiment, it takes 31.45 mL of 0.018 M NaOH to neutralize a 15.00 mL sample of HCI.…

A: Acid reacts with base to form salt and water. In the given reaction acid is HCl. It reacts with NaOH…

Q: In a solution of equal concentrations of barbituric acid (C4 H 4 N 2 O 3 ) and sodium barbiturate (C…

A: A mixture of weak acid and its conjugate ion with strong base forms an acidic buffer solution. A…

Q: Calculate the pH of 0.238 M Ca(OH)2, assuming the solution ionizes completely.

A:

Q: Find the pH of a solution (adding 0.0100 mol of Ba(OH)2 to 155mL of solution containing 0.0240 mol…

A: Answer:- This question is answered by using the simple concept of calculation pH of solution made by…

Q: 4.25g of Na2HPO4 is added to a 250.00-ml volumetric flask, which is then filled to the mark with…

A: Given that, The mass of the Na2HPO4 in the solution is 4.25 g. The volume of the solution is 250 mL.…

Q: Calculate the pH when 29.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: An analytical chemist is titrating 215.6 mL of a 1.000M solution of hydrazoic acid (HN) with a…

A: Step 1: Step 2: Step 3: Step 4:

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 36.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Buffer Mixture is defined as an Aqueous solution which contains weak acid or weak base with its…

Q: solution contains a mixture of hydrogen cyanide (HCN, Ka = 4.9 X 10–10) and sodium cyanide (NaCN).…

A: pH of buffer solution is calculated by using Henderson Hesselbalch equation

Q: Consider 0.10 M NaCN solution. (a) Show an equation of dissociation (ionization) of NaCN in water.…

A: The dissociation of NaCN in water is as follows :NaCNs ⇌                 Na+aq + CN-aq

Q: You are preparing a solution with Boris. Boris placed 60.5 g of K,C,H_O along with 0.320 moles of…

A:

Q: Calculate the pH of a 2.1 M Ca(OH)2 aqueous solution.

A: Consider the given information is as follows; Molarity of Ca(OH)2 = 2.1 M pH = ?

Q: The sample of 30.00 mL of 0.015 M HClO is titrated with a 20.00 mL of a 0.015 M NaOH solution. (a)…

A: In quantitative analysis,acid-base titrations are carried out to find the concentration of unknown…

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 42.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

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: What is the pH of a solution obtained by mixing 0.75 L of 0.147 M  Ba(OH)2 and 0.28 L of 0.0660 M…

A:

Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

A:

Q: Calculate the pH of a solution formed by mixing 550.0 mL of 0.30 M HClO with 275.0 mL of 0.20 M…

A:

Q: Calculate the pH of the solution that results when 10.0 mL of 0.15 M NaOH is added to 50.0 mL of…

A:

Q: A titration of 0.100 M NaOH is titrated into 25.0 ml of a 0.100 M HCHO2 solution (Ka= 1.80 x 10^-4)…

A: Acid-base titration: It is an analytical method used for determining the concentration of unknown…

Q: Calculate the pH of each of the following strong acid solutions. (a) 0.000726 M HClO4 pH =…

A:

Q: Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: A 9.802-g portion of NaCN was dissolved in enough water to prepare 1.00-L of solution. Calculate (a)…

A: The pH of a solution is used to determine the acidity or alkalinity of a solution. The pH is…

Q: determine the pH of a 0.24 M Ca(OH)2 solution

A: Given;

Q: Can you please answer question 5

A: The question is based on the concept of the pH of the solution.It is defined as a negative logarithm…

Q: Calculate the pH when 31.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: KOH + HOBr = KOBr + H2O Moles of HBrO = Molarity x volume in…

Q: You are asked to find the pH of each solution described below. A 0.50 M solution of HBrO3 A 0.030…

A: The compound completely dissociate to form H+, then is called strong acid .Where the compound…

Q: Calculate the pOH and pH of a 0.0045 M solution of NaOH.

A: concentration of NaOH solution is 0.0045 M  we have to find pH and pOH of solution  pH = -log[H+]…

Q: hydrofluoric acid is 6.6*

A: Molarity of KOH = 0.13 M Volume of KOH = 250 mL  mmol of KOH = M × V     = 0.13 × 250 = 32.5 mmol…

Q: A solution of the strong base Mg(OH)2 has pH = 9.57. a)         Calculate the molarity of the…

A:

Q: Calculate the pH when 6.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given : concentration of HBrO = 0.3 M and volume of HBrO solution = 20 mL = 0.020 L…

Q: when 100 ml of a .01 M Mg(OH)2 solution is mixed with 100 mL of a .01 M HCl solution, what is the pH…

A: Since both acids and base are strong  hence they will react to form water as shown below Mg(OH)2 + 2…

Q: )A solution made by dissolving 7.40 g of potassium hypochlorite (KClO) into 1.50 L of solution.…

A:

Q: Calculate the pH when 10.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given Molarity of KOH = 0.150 M Volume of KOH = 10 ml Molarity of HBrO = 0.300 M Volume of HBrO = 20…

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: To a solution consisting of 8 mL of water, 2.065 mL of EtOH, 60% of nitric acid, and 10 mL of TEOS,…

A: The objective of this question is to calculate the pH of the solution after the addition of the…

Q: Determine the pH of   (a) a 0.25 M NH3 solution.    (b) a solution that is 0.25 M NH3 and 0.40 M…

A: Ammonia is a weak base, it is a Lewis base.

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.