What is the pOH of a .17 M solution of pyridime (Kb= 1.4 x 10-9) at 25•C?

Q: 3. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution.…

A: (a) Initial Concentration of CH3COOH Given mass of acetic acid = 0.056 gms,           Volume of…

Q: 8. Classify as spontaneous or no reaction. If spontaneous, write out the complete reaction. a) Ni²+…

A: Here we have to predict whether the following given redox reactions are spontaneous or not.

Q: Calculate the pH at 25 °C of a 0.44 M solution of lidocaine HCI (C14H2NONH,CI). Note that lidocaine…

A: Since C14H21NONH is a weak base with pKb = 7.94 Hence the pKa of its conjugate base i.e C14H21NONH2+…

Q: What is the [H30*] in a 175 mL sample of 0.0629 M KOH(aq)? 9.08 x 10-13 mol L-1 O 2.78 x 10-14 mol…

A:

Q: Consider a solution of Na₂A for which F = 0.050 mol L-¹, K₂,1 = 4.70 x 10-³ and K₁,2 = 1.80 x 10-¹0,…

A: Given the formality of Na2A = 0.050 M  Each Na2A(aq) given 1 A2-(aq). Hence molarity of A2-(aq) =…

Q: Calculate the pH of a solution that is 0.0330 M in a. NaH,PO4 (Kal = 7.11 x 10-3, K,2 = 6.32 ×…

A:

Q: - 4. Determine the pH of a 0.095 mol/L HIO4 solution if the K₂ = 1.29 x 10-² + HIO4 (aq) H3O+ (aq)…

A: 4)

Q: alculate the concentration of free Ca²⁺ in a solution of 0.10 M CaY²⁻ at pH 8.00. (K= 5.0 × 10¹⁰)

A:

Q: What is the pOH of a 0.0085 M Sr(OH)2 aqueous solution at 298 K?

A: Hydroxide ion concentration  determine the basicity if the solution.

Q: The OH concentration in an aqueous solution at 25 °C is 7.1 x 10-5. What is [H*]?

A:

Q: Calculate the pH at 25 °C of a 0.47M solution of anilinium chloride (C6H5NH₂CI). Note that aniline…

A:

Q: What is the hydronium ion concentration of a 0.200 M solution of methylamine? The Kb value for…

A:

Q: O Classify the following reactions in solutions as acidic or basic. a) H2SO4 (29) + H2O1) → 2H*(29)…

A: If a substance when dissolved in water releases H+ ions , it is said to be an acid and the solution…

Q: What is the pOH of a 0.521 M weak base solution that has a Kb = 2.5 x 10-7

A:

Q: What was the original 1. concentration (M) of an aqueous acetic acid (CH3COOH) solution whose pH is…

A:

Q: etermine [H3O+] and [OH] concentrations (in M to two decimal places) for each: (a) Pure water at 10…

A: pH of a solution is defined as negative logarithmic of concentration of hydrogen ions

Q: Calculate the pH of a 0.25 M ammonium chloride solution with a Kb value of 1.8 x 10-5. A pH = 5.5 B)…

A:

Q: Calculate the pH of a 0.0241 M KOH solution at T (°C) Kw each temperature. 1.15 x 10-15 5 1.88 ×…

A: Given  [OH-]   =  0.0241 M pH at 20℃  = ? PH at 35℃  = ?

Q: Calculate the pH of 0.30 M NaOH solution ?   Kw = 1.0 x 10-14

A: pH is defined as the concentration of hydronium ion in the solution

Q: What is the pOH of an aqueous solution prepared by dissolving 4.3 g piperidine, C5H10NH, 286.0…

A: we have to calculate the pOH of piperidine solution

Q: Four solutions of an acid dissolved in water are sketched below, as if under a microscope so…

A: The strength of different acids can be compared on the basis of the degree of dissociation of these…

Q: What is the pH of a solution of 0.300 M HNO containing 0.110 M NaNO? (Ka of HNO is 4.5 \times 10)

A:

Q: What is the OH– concentration of an aqueous solution with a pH of 9.83? (Kw = 1.01 ´ 10–14)

A: Acid-base equilibrium.

Q: H2Se is a diprotic acid. What is the pH of a 0.10 M H2Se solution ? Kal = 1.3 x 10-4 and Ka2 = 1.0 x…

A:

Q: The pH scale depends on the value of Kw. What would the pH of neutral water be if the Kw was 5.54…

A: Given: The Kw of neutral water = 5.54 × 10-15 We have to calculate the pH of neutral water.

Q: What is the pH of a solution of 0.300 M HNO₂ containing 0.210 M NaNO₂? (Ka of HNO₂ is 4.5 × 10⁻⁴)

A: BUFFER SOLUTION It is a solution of weak acid or base with their corresponding conjugate base or…

Q: What is the pH of a 0.15 M solution of the weak base, ammonia, NH3 (Kb = 1.8 x 10-5) in water? (SHOW…

A: Ammonia is a weak base, when it reacts with water it forms hydroxide ion. aAt equilibrium 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.