pH=7.30

Q: What is the pH of a solution of 0.12 M of benzoic acid for which PK₁ = 4.20?

A:

Q: Calculate the pH of a 0.150M solution of aniline, C₆H₅NH₂ ka=4.0E-10

A: Answer:Negative of logarithm of OH- ion concentration is equal to pOH, so,Also,

Q: Find the pH of 0.2 M ammonia solution (pka=9.74). 2) a) b) Find the initial concentration of the…

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Q: Write out the products when the following acids dissociate and release a proton (don't forget…

A: According to Arrhenius theory acids which gives an H+ ions on dissociation in aqueous medium and…

Q: What is the pH of a 0.34 M solution of LiNO2? Use the Ka of its parent acid, HNO2. Ka of HNO2 =…

A:

Q: (10 pts) What is the Kg of an acid HA if the pH of a 0.150 M solution NaA has a measured pH 8.52? 9.

A: Molarity of NaA solution = 0.150 M Measured pH = 8.52 From the relation, pOH is calculated as,

Q: Lactic Acid, HC3H5O3, is found in our sour milk. What is the pH of 0.30 M lactic acid? This acid is…

A: Given :            Concentration of lactic acid = 0.30 M            Ka for lactic acid = 1.4 X 10-4…

Q: If in a solution [H,01-10 [OH ], what is the pH of the solution?

A: Given that :  [H3O+] = 10 [OH-]  We need to determine pH of this solution.

Q: What concentration of oxalic acid, HOOCCOOH(H2A), will have a pH of 50 (pKa1 = 1.25; pKa2 = 4.14)?

A: Given:pH = 50pKa1 = 1.25pka2 = 4.14The pH of a solution is determined using the negative logarithm…

Q: 3. Which of the following reactions shows acetic acid, a common weak acid, reacting with water…

A: The reaction with water follows      Weak electrolytes are substances that cannot completely…

Q: (Q7) If the initial concentration of the weak base ammonia in a solution is 0.401 M and the solution…

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Q: Ihave some acetic acid that dissociates in water. [CH3COOH] = 0.405 M and [CH3COO]=0.505 M.…

A: The acid ionization constant for acetic acid is 1.8×10 -5.

Q: The base protonation constånt K, of morpholine (C,H,ONH) is 2.14 x 10 . Calculate the pH of a 0.86 M…

A: Equilibrium constant is the ratio of  product of concentration of products raised to their…

Q: 3. Determine the pH of the following solutions: a. 1.9 M HClO2 solution (Ka = 1.1x10-2) b. 2.8 M…

A: In this question, we will determine the pH of the following two solution one is acidic solution and…

Q: 7. Using Ka to Calculate pH (7.1) Calculate the pH of a 0.20 M solution of HCN. (Ka=4.9×1010.)

A: Please find your solution below :

Q: find the pH of a KOH solution that is aqueous and 1x10-7M.

A: pH is defined as negative logarithm of hydrogen ions.

Q: a solution that is 0.20 M in HCHO2 and 0.12 M in NaCHO2 (Ka (HCHO₂) = 1.8 × 10-4) Express your…

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Q: 2. Calculate Ka for Aspirin solution (350 ml containing 1.26 g) with pH 2.6. The molecular formula…

A: Given data, Mass of aspirin=1.26gVolume=350mL=0.350LpH=2.6Molecular mass of aspirin=180g/mol

Q: 2 Calculate the pH of 0.15 M of C6H5COONa. K₁= 6.3*105 Show your work!

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

Q: (8) [Text - Problem 2.43] 2-43 What is the pH of a water that contains 120.00 mg L-¹ of bicarbonate…

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Q: (Q7) If the initial concentration of the weak base ammonia in a solution is 0.247 M and the solution…

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Q: Q9) The base ionization constant for (Kp) for acetate ion CH3COO') is equal to: O 4.75 Ɔ 9.25 Ɔ 1.8…

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Q: Calculate the [H3O+][H3O+] of oranges with pH=3.50pH=3.50 .

A: We are having oranges with pH=3.50 pH = - log [H3O+]

Q: What is the pH of a 0.26 M solution of NaNO₂? For nitrous acid, HNO₂, K₂ = 4.6 x 10-4. pH = 1 1.97

A: We have to calculate the pH of the solution

Q: 8. i) Identify the letter choice that shows the correct Bronsted-Lowry acid-base pairs for: H3PO…

A: Bronsted-Lowry acid-base theory: The Bronsted-Lowry acid-base theory states that the acid is a…

Q: For a 6.60x10-2 M solution of H₂Se, calculate both the pH and the Se2- ion concentration. H₂Se + H₂0…

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Q: (Q6) If the equilibrium pH of an aqueous solution is 1.72 and the solution is 0.433 M in formic…

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Q: What are the [H,O*| and [OH] of Diet Coke that has a pH of 3.17? ()

A:

Q: (Q6) If the equilibrium pH of an aqueous solution is 1.72 and the solution is 0.382 M in formic…

A: Given ; pH = 1.72

Q: Calculate the pH of a 0.0015 M solution of C6H5NH2 (Kb for C6H5NH2 = 3.80 ⨉ 10-10).

A:

Q: (Q20) In the hydrosulfuric acid solution described in Q19, what is the equilibrium concentration of…

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Q: What is the pH of a grapefruit that contains 0.007 M citric acid solution (C6H8O7)? CoH8O7(aq) +…

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Q: Calculate the pH of the following solutions. (a) [H3O+] = 1.0x10-6 M pH = (b) [H3O+] = 1.0x10-3 M pH…

A: The formula to calculate the pH value of the solution is  pH = - log [H3O+]  or pH = - log [H+]

Q: The pH of 0.125 M Na2X is 11.15 and the pH of 0.125 M H₂X is 2.55. Calculate pKai and pKaz for H₂X.

A: The pH of a solution is used to determine the acidity or alkalinity of a solution. The pH is simply…

Q: (Q13) The poison strychnine is a weak base with Kp = 1.8 x 106. What will be the equilibrium pH of a…

A: Given-> Kb = 1.8 × 10-6 Molarity = 0.710 M

Q: What is the pH of a solution containing 3xx10^(-4)mg//L of OH^(-)(25^(@)C) ?

A: Given that the concentration of the HO- ion in the solution is 3×10-4 mg/L at 25 °C.Formula:pOH =…

Q: Determine the pH of a 0.095M hypochlorous acid solution given that the K₂=3.0 x 10 (EQ3.7)…

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.