Calculate the pH of 0.40 M NH3 solution, Kb = 1.8 x 10° M.

Q: What is the pH of a 0.0560 M solution of HONH3CI (Kb of HONH₂ is 1.1 x 10-8)?

A: Given,Concentration of  of Objective : Determine the pH of solution

Q: Determine the pH of the molecules given in a 1L beaker containing 0.035M solution of the given…

A: Given,  The molarity of each solution in 1 L beaker is 0.035 M.  The pH of the solution is:

Q: The CO2 we breathe reacts with water in our blood to form the weak acid H2CO3. What mole ratio of…

A: Given:Ka of H2CO3 is 4.4 ✕ 10−8

Q: What is the pH of a 0.1777 M NH(aq) solution at room temperature?  The base ionization constant of…

A: Interpretation -  To determine the pH of 0.1777 M NH3(aq) solution at room temperature when base…

Q: = 1 acid HI H₂S = 2 HIO, HCIO, strong or weak? strong The chemical formulae of some acids are listed…

A:

Q: Given the Ka-250 x 10 for HA, determine the pH (to three significant figures) of a solution that is…

A: Given the Ka = 2.5 * 10 ^ - 9 for HA, we need to determine the pH (to three significant figures) of…

Q: Use the acidity model pH = − log[H+], where acidity (pH) is a measure of the hydrogen ion…

A: Given data: The pH of the solution = 5.8. To find: [H+] for a solution.

Q: The pH of a 3.65 M ammonia NH3 solution (Kb = 1.8 x 10-5) is? If hypochlorous acid HClO (Ka = 3.0 x…

A:

Q: Calculate the pH of a 5.3 x 10-3-M solution of H2S04 (Ka, = 1.2 x 10-2). pH =

A: Given-> Concentration of H2SO4 = 5.3 × 10-3 M

Q: You begin with 100 mL of 0,250 M HCN and add to it 0,75 M NaOH at 25°C (HCN Ka = 6,2 * 10-10)…

A: Given: The volume of 0.250 M HCN added to 0.75 M NaOH is 100 mL. The acid dissociation constant of…

Q: Determine the pH of a solution that is 0.45 M CH₂COOH and 0.40 M CH3COONa. Be sure your answer has…

A:

Q: 3. Classify the following as acidic, basic, or neutral. pH = 9.0 Он - 1X 10-7 м РОН %3 4.0 H* = 1.5…

A: pH = -log[H+]  pOH = -log[OH-]  pH + pOH = 14.0  So, pH = 14.0 - pOH

Q: Strong Bases; Calculate pH [base] [H3O"] pH Step 1 The strong base dissociates completely in aqueous…

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Q: . Calculate the pH of a 0.0368 M aqueous solution of nitrous acid (HNO2, Ka = 4.5×10-4).

A: HNO2 is a weak acid and does not undergo complete dissociation in solution.

Q: Sulfurous acid (H₂SO3) is a diprotic acid with Kal = 1.39 x 10-2 and K₁2 = 6.73 x 10-8. Determine…

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Q: The K for benzoic acid is 6.5 × 10 a . Calculate the pH of a 0.36 M benzoic acid solution.

A: The answer to the following question is-

Q: Calculate the pH of a 0.0159 M aqueous solution of formic acid (HCOOH, Ka 4). = 1.8×10

A:

Q: Determine the pH

A: The scale which is used to analyze the acidity and basicity of an aqueous solution is called as pH…

Q: Calculate the pH of the solution that contains 0.145 M NH3 and 0.192 M NH4Cl.  The Ka of NH4+ is…

A: The solution will be the buffer solution if the weak acid and its corresponding conjugate base are…

Q: The base protonation constant K₁ of lidocaine (C14H21 NONH) is 1.15 × 10 Calculate the pH of a 0.88…

A: Step 1: The base lidocaine (C14H21NONH) is a weak base, which is obvious from its small value of the…

Q: What is the pH of a 0.481 M solution of NH4Br? For NH3, Kb = 1.8 × 10–5

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Q: Calculate the pH of an 0.025 M solution of NH3. NH3 is a weak base. Kb = 1.80 x 10-5

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

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Q: What is the hydronium M ion concentration for an unknown solution with a pH of 9.65? Please write…

A: Given     PH = 9.65   [ H3O+ ]  = ?

Q: 2. What is the pH, the pOH and the [OH] of a solution in which the [H*] = 2.43 x 10-6 M? %3!

A: pH is defined as  the negative log of hydrogen ion concentration  pOH is defined as the negative log…

Q: Determine the pH of each of the following solutions. (a) 0.684 M hypochlorous acid (weak acid…

A:

Q: Calculate the pH, pOH, concentration H30*, and concentration OH in 500.0 mL of 0.09933 M HNO3…

A: Given: Concentration of HNO3 = 0.09933 M And volume of solution = 500.0 mL = 0.500 L…

Q: A solution is made by dissolving 15.1 g of CH₃NH₃NO₃ in 500.0 mL of water. Using Ka(CH₃NH₃⁺) = 2.3 ×…

A:

Q: Metal compound ‘A’ reacts with dilute hydrochloric acid to produceefferenvescence. The gas evolved…

A: Metal compound ‘A’ reacts with dilute hydrochloric acid to produce efferenvescence. The Evolved gas…

Q: aq 6. (1) Define pH in words. The strong acid HCI has a pH value of 1, use the following equation…

A: 6)  HCl(aq)  ➝ H+(aq) + Cl-(aq) i) Define pH = ? HCl is a strong acid. pH of the solution = 1…

Q: pH of a 0.223 M solution of sodium hydrogen chromate (K, 3.0 X 107)

A: Given data are as follows

Q: Find the pH of 0.54 M C5H5N(aq) given that its Kb = 1.7×10-9.

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Q: The Kb value for ammonia is 1.8 × 10–5 . Determine the pH  and the concentration of [OH– ] in a 0.40…

A: Given:  Kb value for ammonia = 1.8 × 10–5 Initial concentration of NH3 = 0.40 M

Q: Calculate the pH of a 0.22 M codeine solution (Kb = 1.6ã10−6).

A: The value of Kb for the given weak base is = 1.6x10-6 The concentration of the base solution is =…

Q: Calculate the pH of a 0.591 M aqueous solution of benzoic acid (CH₂COOH, K₂ = 6.3x10-5). pH =

A: Here,concentration of benzoic acid = 0.591 MKa = 6.3×10-5We have to find out pH.. Herw first we need…

Q: Phthalic acid (H₂CH₂O₂) is a diprotic acid with Kal = 1.12 x 10-3 and K₁2 = 3.90 x 10-6. Determine…

A: Given : acid is diprotic

Q: For a certain acid pK₂ = 6.59. Calculate the pH at which an aqueous solution of this acid would be…

A: Given that, for a certain acid pKa = 6.59. The degree of dissociation of the acid in an aqueous…

Q: What is the pH of a 0.250 M solution of H2SO4? K22 = 1.20×10-2

A:

Q: Q3. This question is about the pH of several solutions. Give all values of pH to 2 decimal places.…

A: PH  of solution determines the nature of solution whether it is acid or basic solution. The acidic…

Q: The Ka value for acetic acid, CH,COOH(aq), is 1.8 × 10-5. Calculate the pH of a 1.20 M acetic acid…

A: Acetic acid dissociates as: CH3COOH→CH3COO-+H+

Q: 3+ Calculate the pH of a 0.064-M Al (NO3); solution. The K, value for Al (H20)," is 1.4 x 10.

A: Concentration of Al ion = 0.064 M

Q: What is the pH of a 0.00105 M  solution of nicotine (C10H14N2)? (Kb1 = 1.0 × 10–6)

A: The explanation is given below-

Q: Kb(NH3) 1.8 x 10-5. What is the pH of 0.40 M NH4CI? pH = = (type your answer; do not use scientific…

A: The objective of the question is to determine the pH of the given solution.It is given that,The…

Q: The acid dissociation constant K of boric acid (HBO3) is 5.8 × 10¯¹0. Calculate the pH of a 2.5 M…

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Q: Determine the pH of a 0.450M solution of aniline hydrochloride. C6H;NH, (ag) + H,O(1) = H;O* (ag) +…

A:

Q: Determine the pH of a 0.10 M solution of sodium acetate (CH3COONa) at 25°C. (Ka of acetic acid = 1.8…

A:

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.