8) A 0.185 M solution of a weak acid has a pH of 2.95. Calculate the acid ionization constant (Ka) for the acid.

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0143 M solution. The pH of the…

A: Given :-  Concentration of weak acid solution = 0.0143 M  pH of solution = 2.59  To calculate :  Ka…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.181.18 M solution. The pH of the…

A: Given: The molarity of the monoprotic acid = 1.18 M The pH of the solution = 2.78 We have to…

Q: The pH of an aqueous solution of 0.354 M hydrofluoric acid is

A: Hydrogen fluoride is a weak acid and its pKa value is = 3.17 The concentration of HF solution is =…

Q: A chemist dissolves 130. mg of pure sodium hydroxide in enough water to make up 70. mL of solution.…

A:

Q: The pH of 0.259 M solution of an unknown acid is measured to be 2.353. What is the Ka of the acid?

A:

Q: "Acid rain" forms when rain falls through air polluted by oxides of sulfur and nitrogen, which…

A:

Q: The pH of an aqueous solution at 25°C was found to be 2.40. The pOH of this solution is The…

A: Given that   Ph of aqueous solution is 2.40

Q: A typical aspirin tablet contains 328 mg acetylsalicylic acid (HC,H;O,). Calculate the pH of a…

A: Given, Mass of one aspirin tablet = 328 mg So, mass of two tablet = 2×328 = 656 mg=0.656 g Final…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0200 M solution. The pH of the…

A: Assuming the monoprotic acid is HA Hence the dissolution reaction is  HA ---> H+ + A-  since pH =…

Q: A chemist dissolves 134. mg of pure sodium hydroxide in enough water to make up 170. mL of solution.…

A: Answer: pH tells us about the power of hydrogen ion concentration and its value is equal to the…

Q: The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31.  What is the Ka of the acid?

A: Given  pH = 2.31 Concentration of acid = 1.86 M Ka =?

Q: A chemist dissolves 696. mg of pure perchloric acid in enough water to make up 350. mL of solution.…

A: and,

Q: the Ph of a 0.050 M weak acid solution is 5.25. Calculate the Ka of the acid.

A: Given, pH of weak acid= 5.25 [weak acid ] =0.050 M Ka = ?

Q: A chemist dissolves 724.mg of pure potassium hydroxide in enough water to make up 170.mL of…

A: potassium hydroxide will release hydroxide ions in the solution.

Q: 6a) Write the hydrolysis reaction of hypochlorous acid Clearly identify the acid, base, conjugate…

A: Given data:Concentration of solution of acid =0.050 MDetermine the hydrolysis reaction of…

Q: The pH of an aqueous acid solution is 6.15 at 25 ° C. Calculate the Ka for the acid. The initial…

A: The equilibrium constant for acid dissociation is denoted as Ka. It represents the ratio of the…

Q: If the concentration of an acid is 0.0025 M, calculate the pH of the acid.

A:

Q: What is the pH of a 0.115 M solution of acid HA if the ionization constant (KA) of this acid is 0.31…

A: We will first find the expression for Ka using ICE table. After doing so, we will calculate…

Q: The pH of an aqueous solution of 0.512 M nitrous acid is

A: Given 0.512M Nitrous acid HNO2 Pka of Nitrous acid  [H+] = (7.2*10-4*0.512)1/2 [H+] = 0.0192

Q: (a) Do the calculations and show that the hydronium ion concentration for a 0.233-M solution of C6…

A: (a) C6H5NH3+ hydrolyze in water as follows:

Q: A chemist dissolves 532. mg of pure perchloric acid in enough water to make up 110. mL of solution.…

A: Number of moles of HClO4 can be calculated as shown below:

Q: A chemist dissolves 555.mg of pure perchloric acid in enough water to make up 60.mL of solution.…

A: We have to calculate the pH of perchloric acid.

Q: A chemist dissolves 656. mg of pure barium hydroxide in enough water to make up 90. mL of solution.…

A:

Q: Calculate the ph of  3)A 0.0250 molar solution of potassium carbonate.

A: Given: Concentration of potassium carbonate(K2CO3) = 0.0250 M 1 mole of K2CO3 gives 2 moles of KOH…

Q: A 0.150 M solution of a weak acid has a pH of 2.65. Calculate the acid ionization constant Ka for…

A: 3.34×10−5Explanation:

Q: calculate the hydroxide ion concentration of a solution with pH =9.9

A: Given : pH = 9.9  Since , pH + pOH = 14  => pOH = 14 - pH = 14 - 9.9 = 4.1  pOH = - log[OH-

Q: what is the ph of a solution whose hydrogen ion concentration is 0.015?

A: As we know, HCl is a stong acid. It dissociates completely into H+ and Cl—in a chemical equation –

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.251.25 M solution. The pH of the…

A: HA  + H2O  →H3O+ +  A- Expression for Ka will be,Ka = [H3O+] [A-][HA] Given that,initial…

Q: Calculate the acid ionization constant (Ka) if the pH of the 0.1 M acetic acid solution is 2.87?

A: We have given that  Concentration of acetic acid = 0.1M  pH = 2.87

Q: A chemist dissolves 102. mg of pure perchloric acid in enough water to make up 310. mL of solution.…

A: Using given mass and volume first the molarity of the solution is calculated. Calculate the moles of…

Q: Calculate The pH 0.09M solution of magnesium hydroxide

A:

Q: A chemist dissolves 446. mg of pure barium hydroxide in enough water to make up 170. mL of solution.…

A:

Q: . Calculate the pH of the solution.

A: Given :-  Mass of NaOH =121 mg  Volume of solution = 180 mL  To calculate :-  pH of the solution…

Q: A chemist dissolves 387. mg of pure sodium hydroxide in enough water to make up 140. mL of solution.…

A: Given: Mass of NaOH = 387.0 mg = 0.387 g Volume of the solution = 140.0 mL = 0.140 L Known: Molar…

Q: A chemist dissolves 465. mg of pure potassium hydroxide in enough water to make up 90. mL of…

A: Mass of KOH in g = 465 / 1000 = 0.465 g Volume of solution in L = 90/1000 = 0.090 L Moles of KOH =…

Q: Calculate the hydroxide ion concentration of a solution with pH= 2.8

A: Given: pH= 2.8 To find: The concentration of hydroxide ion

Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: A chemist dissolves 744. mg of pure hydrochloric acid in enough water to make up 250. mL of…

A: Given data :  Mass of HCl = 744. mg = 0.744 g (1 mg = 0.001 g) Volume of solution = 250 mL = 0.25 L…

Q: A 0.185 M solution of a weak acid (HA) has a pH of 2.91.

A: The concentration of weak acid (HA) = 0.185 MThe pH of the solution = 2.91 The Ka of the weak acid…

Q: A chemist dissolves 423. mg of pure potassium hydroxide in enough water to make up 130. mL of…

A: Given data,  Mass of pure potassium hydroxide (KOH) = 423 mg  Volume of solution = 130 mL…

Q: A chemist dissolves 170 , mg of pure nitric acid in enough water to make up 70. mL of solution .…

A: Ans.  Number of the moles of the nitric acid = mass/molar mass =0.170g/63.01g/mol = 0.0026979 moles…

Q: The pH for 0.0850 M solution of C₆H₅CH₂COOH is 2.68. Determine the value of Ka for C₆H₅CH₂COOH.…

A: The acid dissociates as: C6H5CH2COOH→C6H5CH2COO-+H+

Q: A chemist dissolves 378. mg of pure barium hydroxide in enough water to make up 170. mL of solution.…

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

Q: Determine the pH of a solution that is 0.00482 M HCl0.00482 M HCl and 0.0304 M HClO2. The Ka of…

A: Given -> Molarity of HCl = 0.00482 M Molarity of HClO2 = 0.0304 M Ka = 1.1 × 10-2

Q: A 0.115 M solution of a weak acid (HA) has a pH of 3.29. Calculate the acid ionization constant (Ka)…

A: The concentration of HA = 0.115 M pH = 3.29 pH = 3.29H3O+ =10-pH=10-3.29=0.000513 M

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.261.26 M solution. The pH of the…

A: Given: Concentration of monoprotic acid (Assuming HA) = 1.26 M And the pH of the solution = 2.70

Q: A chemist dissolves 595. mg of pure nitric acid in enough water to make up 360. mL of solution.…

A: Molar mass of HNO3,

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.