What is the pH of the solution containing 2.5 X 104 of OH- at 25°C?

Q: The pH of a solution of C₂H₅NH₂ is 9.47 at 25 °C. What is the H⁺ concentration in this solution?.

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Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Answer: NH4Cl is the salt of weak base and strong acid, therefore its hydrolysis will take place in…

Q: The pH of a basic solution is 10.61. What is [H⁺]?

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Q: NH3 is a weak base (?b=1.8×10^−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Given: Kb = 1.8 × 10-5              Concentration of solution = 0.056 M             Temperature = 25…

Q: The pH of a basic solution is 10.19. What is [OH⁻]?

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Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid.   What is the pH of a…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: In a solution, [H+] = 1.54 x 10-2 M. What is its pH and is it considered an acid or a base?

A: Given is,  [H+] = 1.54 x 10-2 M

Q: What is the pH of a solution which is 0.023 M in weak base and 0.035 M in the conjugate weak acid…

A: The solution is as follows:

Q: (a) What is the pH of 0.0111 M NaOH? Is the solution neu-tral, acidic, or basic? (b) What is the pOH…

A: To determine a)The pH of 0.0111 M NaOH b)The pOH of 1.35 x 10⁻³ M HCl

Q: A solution has a pH of 3.10. What is the OH- concentration of the solutionat 25 degrees Celcius?

A: pH of a solution is equal to the negative logarithm of the concentration of H+ions.

Q: What is the pH of a solution that has [OH-] = 5.0 x 10-7 M?

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Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: To calctulate the pH, we would use Ka or Kb expression.  “Since you have posted multiple questions,…

Q: What is the pH of an aqueous solution in which [H+] is 0.0025 M?

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Q: The pH of a basic solution is 10.57. What is [OH⁻]?

A: The question is based on the concept of pH of the solution.  it is defined as a negative logarithm…

Q: The pH of a solution with pOH = 8.5 Is this an acid, base, or neutral?

A: Given :- pOH of solution = 8.5  To be calculated :- pH and nature of the solution

Q: The pH of a basic solution is 10.41. What is [OH⁻]?

A: pH of a solution is the parameter which is used to define the acidity or basicity of a solution.…

Q: NH3 is a weak base ( ?b=1.8×10−5 ) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A:

Q: NH3 is a weak base (?b=1.8×10−5�b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the…

A:

Q: NH3 is a weak base (?b=1.8×10^5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A:

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A:

Q: pH

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Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Calculating for pH given the value Kb :- In solving this problem we need the right dissociation…

Q: If the hydroxide concentration of a solution is [OH-] = 4.67 X 10-8 what would the pH of that…

A: Given:The concentration of OH, [OH-] = 4.67 X 10-8To find:pH = ?

Q: Morphine has the formula C17H19NO3. It is a base and accepts one proton per molecule. It is isolated…

A: Given information is as follows: Volume of sulfuric acid = 8.92 mL = 0.00892 L Concentration of…

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

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Q: Calculate [H+] for each of the following solutions, andindicate whether the solution is acidic,…

A: pH = -log[H+] pOH = -log [OH-] pH + pOH = 14

Q: What is the pH of a solution that has [OH-] = 2.2 x 10-5 M?

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Q: What is the pH (in two decimal places) of a 0.047 M solution of Sr(OH)2?

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Q: NH3 is a weak base ( ?b=1.8×10−5 ) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Ammonium chloride (NH4Cl) is a salt of a weak base (NH3) and a strong acid (HCl).When NH4Cl…

Q: What is the pH of a solution that is 0.041 M in NH4Cl?

A: NH4Cl salt can be formed from weak base NH4OH and strong acid HCl. So it is a salt of strong acid…

Q: What is the pH of a solution that has [OH-] = 6.5 x 10-3 M?

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Q: The pH of a basic solution is 10.65. What is [OH⁻]?

A: Given the pH of the basic solution, pH = 10.65  We can find the pOH of the solution using the…

Q: The pH of 0.55 M aqueous solution ammonia HN3 at 25.0 degree C is 11.50. What is the value of Kb for…

A: NOTE : You have given HN3 instead of NH3. Since the pH is in basic zone, hence the specie will be…

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

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Q: In a solution, [H+ ] = 3.25 x 10-10 M. What is its pH and is it considered an acid or a base?

A: A solution can be classified as acidic or basic or neutral depending on the pH value. For a solution…

Q: The pH of a basic solution is 11.43. What is [OH⁻]?

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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.