Calculate the [OH-], [H3O+], pOH and pH of a 0.075 M NH3 Ka NH4+ = 5.70 x 10-10

Q: Calculate the [H3O+] of a 0.390 M acid solution; Ka=4.52 x10-5

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Q: Why is the ph of NH4C2H3O2 nearly 7

A: The question is based on the concept of salt hydrolysis . we need to calculate pH of ammonium…

Q: iven the following: [H3O+] = 6.330 x 10-5,  calculate the pH:  (note: for pH always please use 3 sig…

A: pH = - log[H3O+] = - log(6.330×10-5) =5-log(6.330) = 4.20

Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in base…

A: pH is the measure of concentration of H+ ions. Here pH can be calculated with the help of kB values,…

Q: Calculate the pH of 9.3×10−2  M propionic acid (C2H5COOH). Ka= 1.3x10-5

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Q: Calculate the pH, pOH, and [H+1] of a solution in which the [OH- ]=2.34x10-5

A: Given [OH-] = 2.34*10-5

Q: Calculate the [H +], [OH -], pH , pOH of 005 M NH3     Kb=   1.8 x 10 -5

A: pH is a measure of how acidic/basic water is. The range goes from 0 to 14, with 7 being neutral. pHs…

Q: Benzoic acid, HC6H5CO₂, is a monoprotic acid (only one H* ionizes) with a K₂ = 6.5 x 10-5. Calculate…

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Q: Consider 0.50 M HC₂H3O₂ (K₂ = 1.8 × 10-5). What are the major species in the solution? HC₂H302 H₂O

A: Where given compound HC2H3O2 is a weak acid and it's name is acetic acid It is an organic acid ,…

Q: Cyanic acid (HOCN) is an extremely acrid, unstable substance. What are the[H3O+] and the pH of 0.10…

A: Given  Concentration of HOCN (c) = 0.10 M Ka = 3.5×10-4 [H3O+] = ?  pH=?

Q: The [H3O+] of lemon juice is 2.5 x 10-2 M.  Calculate the pH.

A: Given  [ H3O+ ]  = 2.5 × 10-2 M  PH = ?

Q: What is the pH of a solution with [OH1-] = 1 x 10-8 ?

A: Since, pH represent the acidity of the solution. If pH less than 7 then solution is acidic. If pH =7…

Q: Calculate the [H3O+], [OH-], pH and pOH of  a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

A: pH of a solution is given by the negative logarithm of hydrogen ion  concentration in the solution…

Q: Calculate the pH of 4.0 X10 -4 M KOH

A: Please find your solution below : pH is a measure of acidity or basicity of a substance. It is…

Q: Calculate the pH of 0.15M CH3COOH. Ka=1.8×10-5

A: In this question, we have to find out the correct answer of given problem by the help of the…

Q: Calculate the pH, pOH, and [OH-1] of solution in which the [H3O+]=1.2x10-3

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Q: Calculate the [H+] of a solution prepared by combining 1 L of a HC1O4 solution with pH = 2.00 and 1…

A: Given data, pH of HClO4 solution = 2.00 Volume of HClO4 = 1.0L Volume of H2SO4 = 1.0L pH of H2SO4 =…

Q: Calculate [H+] for a 9.00×10-4 M aqueous solution of cinnamic acid (HC9H7O2; Ka = 3.70×10-5). 1b)…

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Q: Calculate the [H3O+], [OH-], pH and pOH of  a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

A: Nitrous acid is an weak acid, so in an aqueous solution it is in equilibrium with its ions.  Initial…

Q: Calculate the [H3O+], [OH-], pH and pOH of a 0.12 M HNO2

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Q: Determine the [H*],[OH-], and pOH of a solution with a pH of 11.63 at 25 °C. [H*] = M [OH-] = M %3D…

A: Since at 25 oC [H+] * [OH-] = 10-14 pH = -log[H+] pOH = -log[OH-] pH + pOH = 14

Q: Calculate the pH of pure water if [H3O+] = 1.0 x 10-7.

A: PH is the power of Hydrogen. PH is used to determine nature of solution like as acidic,basic or…

Q: Calculate the [H3O+], [OH-], pH and pOH of  a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

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Q: A solution has a pH of 3.76. What is the molarity concentration of H3O+ and OH¹ in this solution? A)…

A: The objective of this question is to determine the molarity concentration of H3O+ and OH- in a…

Q: 1) Write a chemical reaction to show the neutralization of hydriodic acid (HI) by sodium hydroxide…

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Q: propanoic acid, a weak monoprotic acid (HC3H5O2, Ka = 1.3 x 10-5), calculate [H+] and pH of a 0.10 M

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Q: Calculate the [H +], [OH -], pH , pOH of 0.005 M NH3 Kb= 1.8 x 10 -5

A: Ammonia is a weak base hence it dissociated less

Q: Calculate the [H3O+], [OH-], pH and pOH of  a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

A: The acid, HNO2 is dissociated as:                        HNO2→H++NO2-Initial:              C…

Q: Calculate the [H3O+], [OH-], pH and pOH of  a 0.120 M HNO2  (nitrous acid).  Ka = 7.10 x 10-4

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Q: What will be the pH if 0.00150 moles of HCI is added to 1.00 L of water ? The reaction gives the…

A: Given :-  No.of moles of HCl in 1.00L of water = 0.00150 mol  To calculate :-  pH of solution

Q: 5. Make the following conversions. Report answers to 2 decimal places.In each case, tell whether the…

A: pH = -log[H3O+]  [H3O+].[OH-] = kw  Kw at 25°C = 1.00 × 10-14

Q: K, for hypochlorous acid, HC1O, is 3.50 × 10–8. K, for benzoic acid, C, H5 COOH, is 6.30 x 10-5. K,…

A: Acids are chemical compounds which release H+ ions in solution. Higher the amount of H+ released,…

Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid…

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Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10M in acid…

A: HC6H5O (Benzoic Acid) has the lowest Ka value (1.3 × 10^-10).Therefore, HC6H5O would have the…

Q: Calculate the pH of a 0.41 M CH3COONa solution. (Ka for acetic acid = 1.8 ×10−5.)

A: The reaction is written below. CH3COO - + H2O ⇌ CH3COOH - + OH- The ICE table is shown below.

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.