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: The pH of a 0.50 M solution of an acid, HA, is 4.67. Calculate Ka of HA.

A:

Q: The pH of a 0.10 M weak acid solution is determined to be 5.15 at room temperature. Calculate the Ka…

A:

Q: A 0.17 M solution of a weak acid has a pH of 2.85. What is the ka of the weak acid?

A: Given: concentration of weak acid=0.17M              pH of weak acid=2.85 To calculate: Ka of weak…

Q: The pH of a 0.0081 M solution of HNO₃ is

A: Given values-> [HNO3] = 0.0081M HNO3 ---> H^+ + NO3^- [H^+] = 0.0081M pH =-log [H^+] =…

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: A chemist dissolves 641. mg of pure nitric acid in enough water to make up 60. mL of solution.…

A: Molecular mass of nitric acid = 63 gm / mol => moles of nitric acid = mass in gm / molecular mass…

Q: The pH of a 0.0068 M solution of Ca(OH)₂ is

A: pOH = - log[OH-] pH + pOH = 14

Q: Calculate the pH of each acid solution. Explain how the resulting pH values demonstrate that the pH…

A: pH of the solution is equal to the negative logarithm of the concentration of hydronium ions H3O+.…

Q: A chemist dissolves 770. mg of pure nitric acid in enough water to make up 380. mL of solution.…

A:

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: The pH of an aqueous solution of 0.534 M methylamine (a weak base with the formula CH3NH2) is

A:

Q: A chemist dissolves 744. mg of pure hydrobromic acid in enough water to make up 110. mL of solution.…

A: Mass of HBr given is 744 mg = 0.744 g Molar mass of HBr is 80.91 g/mol. Therefore, number of moles…

Q: A chemist dissolves 602.mg of pure hydrobromic acid in enough water to make up 240.mL of solution.…

A:

Q: Determine the pH of a 0.650 M solution of magnesium nitrite, Mg(NO2)2 at 25 °C. A solution…

A: Answer: Hydrolysis of the salt of weak acid and strong base or strong acid and weak base takes place…

Q: A chemist dissolves 715. mg of pure potassium hydroxide in enough water to make up 80. mL of…

A:

Q: If the molarity of an unknown substance is expressed as 3.7 x 10-5, what is the pH of the substance?

A:

Q: The pH of a 0.050 M solution of boric acid is 5.28. What is the value of the boric acid ionization…

A: Given : We have to calculate the ionization constant.

Q: Consider the following ions: Cl-, HS-, NO2-, F-, and HS04-. (a) Which of these ions in water gives…

A: Given ions  Cl- HS- NO2- F- HSO4-

Q: The compound dimethylamine is a weak base like ammonia. A solution contains 0.263 M (CH3)2NH₂*…

A: answer :pH is the measurement of the acidity of the solution.As per the given solution contains,…

Q: The probe of the pH meter shown here is sitting in a beakerthat contains a clear liquid. (a) You are…

A: The probe of the pH meter shown here is sitting in a beakerthat contains a clear liquid.  (a) You…

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: Acetominophen, HC8H8NO2 (MM=151.17 g/mol), is the active ingredient in Tylenol, a common pain…

A: The  question involves concept of equilibrium. we have been given pH of the solution. We have to…

Q: A 0.037 M solution of a weak acid (HA) has a pH of 4.34. What is the Ka 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: concentration

A: pOH = 14 - pH  pOH = 14 - 10.41  pOH = 3.59

Q: A certain solution was found to have a pH of 5.50. Which of following statements is true about this…

A:

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 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: What is pH of a 0.1 Molar solution of oxalic acid in water

A: Given : Concentration of oxalic acid i.e H2C2O4 = 0.1 M The Ka1 and Ka2 of oxalic acid are 5.0 X…

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

A:

Q: The pH of a 2.642M solution of a weak acid, HB is 2.34, What is the Ka for the acid?

A: Given: The conc. of the weak acid solution = 2.642 M HB is a weak acid with a pH = 2.34 A weak acid…

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 pH of each of the following solutions of strong acids.

A:

Q: Hydrogen selenide (H2Se) reacts with water according to the following equation. H2Se + H2O → SeH– +…

A:

Q: . 60.0 mg of codeine sulfate (C18H21NO3H)2SO4 is dissolved in 10.0 mL of water. Calculate the…

A: The given solution contains 60mg of codeine sulphate in 10m1 of water. Also given the molecular…

Q: What is the pH of a calcium hydroxide solution obtained by dissolving 0.17 grams of calcium…

A: Given that : The mass of calcium hydroxide solution = 0.17 g The volume of the solution = 510 mL We…

Q: Normally, the pH of the human body is fixed in a very narrow range between 7.35 and 7.45. A patient…

A: Bicarbonate buffering system is the main buffer system controls pH of blood.

Q: The pH of saliva is normally in the range of 6.4 to 7.0. However, when a person is ill, the person's…

A: pH is defined as negative logarithm of hydrogen ion concentration   pH= -log[H+] If pH<7 then the…

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.