Determine the pOH of a .10M aqueous solution of KF. For hydroflouric acid, Ka = 7.0x10^-4 A. 1 B. 5.92 C. 8.08 D. 5.01 E. 1.58

Q: A. What is the pOH of the solution at the half equivalence point? B. What is the ionization…

A: Given data :  Unknown base  solution  = 10 ml .  Titrated with known concentrated HCl of molar…

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Q: 1 Determine the pH of the resulting solutions when the following reagents are mixed. a. 25.00mL of…

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Q: u make 50.00mL of a 0.045M solution of NaOH from a 2.5M stock solution. 9. How many milliliters of…

A: Answer: As, for the dilution, we add water in the solution, therefore moles of NaOH taken from stock…

Q: 38. Fluorinating water is traditionally done to protect the enamel on teeth. One method used to…

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Q: 6. Consider the reaction of 50.0 mL of 2.0 M nitric acid with 90.0 mL 1.0 M potassium hydroxide.…

A: The equation of given reaction is,

Q: LIOH+HNO3 → H₂O + Li NO3 200.0 mL of a 0.100 M solution of LiOH is mixed with 250.0 mL of a 0.100 M…

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Q: 8. A 1.000 L buffer solution contains 0.250 mol/L. NH, and 0.250 mol/L. NH, CL K=1.8x10 Determine…

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Q: Please don't provide handwriting solution

A: Ka = C2Here  Ka = Disociation constant = ?          C = concentration = 1.43 M           = Digree of…

Q: 4. Calculate the pH of each of the following solutions of strong acids and bases: a. 0.0010 M HCI b.…

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Q: A solution that contains a weak acid and its conjugate base in roughly equal concentrations is A.…

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Q: The Ka of an acid is known to be 1.51 X 10^-5. A solution is made by adding 0.279 mol of the acid to…

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Q: The pOH of an acidic solution is 11.37. What is [OH 1?

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Q: Rank the compounds below in order of increasing acidity  HF, H2O, NH3

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Q: An acid (HA) dissociates as follows: HA - H* + A minus Arrow should be interpreted as an equilibrium…

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Q: You have measured the mass of samples A,B,C,D, and E on the analytical balances in our chemistry…

A: ∵ Standard deviation S=ΣXi-X2n-1Where ,         X=sample average         Xi=Individual values in…

Q: 2. For each of the following salts, determine the pH of a 2.50M solution of the salt. You will need…

A: Molar concentration of solution of salt = 2.50 M

Q: 1. Convert 8.62  pH value to OH- concentration (in mM).

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Q: Calculate the pH of a solution formed by mixing 300.0 mL of 0.15 M NH4CI with 400.0 mL of 0.20 M…

A: Given: Concentration of NH4Cl = 0.15 M Volume of NH4Cl solution added = 300.0 mL = 0.300 L…

Q: a. 0.155 M HONH, ( Къ 3 1.1 х 10 $) pH = b. 0.155 M HONH3C1 pH = c. pure H20 pH = TIONU and 0 155 M…

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Q: A 17.8 mL solution of 0.100 mol L-1 NaOH is titrated using 0.150 mol L-1 HCl. What is the pH of the…

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Q: 16. You take 50.0 mL of a 1.0 M solution of citric acid. Citric acid is a weak acid which has a Ka =…

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Q: 300 ml of 0.05 M ammonia solution, where the density of the solution is 0.88 g/ml. The pka of…

A: The negative logarithm to the base 10, of the ionization constant of an acid Ka is denoted as p Ka .…

Q: A solution is made from 0.39 M HF and 0.31 M NaF. What is the pH of the K, for HF is 6.8x10 4?…

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Q: An aqueous solution of NH4CI would be either acidic or basic depending on the amount of salt…

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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.