Is this a buffer system? NaF + Ca5 (PO4)3OH<---->Ca5(PO4)3F + Na+ + OH- Also, how does Le Chatelier’s principle impact the above?

Q: antiseptic and disinfectant in topical pharmaceutical products in the treatment of skin disorders…

A: We know that the maximum amount of solute that can be dissolved in a solvent at a particular…

Q: 5. The pK,'s for phosphoric acid represent the following ionizations: H;PO4 2 H2PO4 + H* pK = 2.14…

A: Chemical reaction between H3PO4 and NaOH is:   H3PO4+3NaOH→Na3PO4+H2O

Q: A 1.00 L Tris buffer solution is made by mixing 121.14 g of Tris base (MW = 121.14 g/mol), 84 mL of…

A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: How many moles of HA would need to be added to 481 mL of 0.816 M NaA to produce a solution with a pH…

A:

Q: What is the pH of a solution that has a 1:4 ratio of acetate ion to acetic acid? pKa acetic acid =…

A: Given  pKa = 4.75 acetate ion to acetic acid = 1/4 It is Acidic buffer,  pH = pKa + log([acetate…

Q: How many moles of NaA would need to be added to 544 mL of 1.07 M HA to produce a solution with a pH…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: Caffeine (C8H10N4O2) is a neutral weak base and has a Kb= 4.1 x 10^-4. If you dissolve 85 mg in 5.00…

A: Given: Kb of Caffeine (Assuming B) is 4.1 × 10-4. Mass of B used = 85 mg = 0.085 g…

Q: The 3-step ionization of phosphoric acid: H3PO4 = H + H2PO4 H2PO4 = H + HPO4² HPO4? = H* + PO4 Kal =…

A: We need to an acid whose pKa is close to 7.0. then we make a solution of the acid and its conjugate…

Q: The experimental pH of a 0.25 M solution of potassium hydrogen phosphate, K2HPO4, is 10.25. a. Is…

A: The acidic or basic nature of the compound is decided on the basis of the pH value of the compound.…

Q: We dissolve 1.00g of a weak acid HA in 1L of water. Find the concentration, in ppm, of the acid HA…

A: Given: Mass of HA = 1.00 g. Volume of solution = 1 L pKa of HA = 3.27  Molar mass of HA = 140.113…

Q: that is 0.192 M in lactic acid and 0.155 M in sodium lactate? The Kaof lactic acid is 1.4 × 10-4.…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: Given the following table of K, values, what would be the best conjugate acid to choose to make a…

A: The solution is given below -

Q: C6H4NH2COOH, para-aminobenzoic acid (PABA), is used in some sunscreen agents. Calculate the…

A: Para-aminobenzoic acid (PABA), C6H4NH2COOH dissociates as,                              C6H4NH2COOH…

Q: A 1 liter solution is made by adding 0.5844 moles NaH2PO4 and 0.5116 moles Na2HPO4. What will be the…

A: A 1 liter solution is made by adding 0.5844 moles NaH2PO4 and 0.5116 moles Na2HPO4. What will be the…

Q: If [HA]pKa pH<pKa

A: Buffer solution : It is a solution that has the ability to resist in the change in pH when a small…

Q: Solve the following problem, taking turns in your group to explain how to do the next step: What is…

A:

Q: In pure water, what are the concentrations of H+ and OH- ions?

A: Given; ions

Q: Write the Henderson-Hasselbalch equation for a propanoic acid solution (CH;CH,CO,H, pKa=4.874) using…

A: In general equation, pH=pKa+log10([A-])/[HA] The equation for propanoic acid…

Q: Will 260.0 milligrams of calcium carbonate raise the pH of 75.0 milliliters of stomach fluid from a…

A:

Q: 8) What will be the pH (aq., 25 oC) of 250.0 mL of a solution of 0.821 M HCOOH and 0.909 M HCOOK,…

A:

Q: (a) Please write the conjugate bases of the following acids. (1) CH3COOH - CH3CO0 (Ka = 1.76 x 10-5)…

A: Required information from previous parts: From part-(c), the desired ration of conjugate base to…

Q: Benzoic acid, HC7H502, and its salts are used as food preservatives. Ka for benzoic acid is…

A:

Q: you mix together 50.0 mL of 0.25 M (NH4)2S and 50.0 mL of 0.20 M NH4Cl. What will the resulting…

A:

Q: C6H4NH2COOH, para-aminobenzoic acid (PABA), is used in some sunscreen agents. Calculate the…

A: Consider the given information is as follows; Concentration of C6H4NH2COOH = 8.0×10-2 MKa =…

Q: en can you conclude that a buffer solution has achieved its m When pH is less than the pka. When the…

A: Buffer solution is the mixture of weak Acid/base with its conjugate base/acid. pH range for acidic…

Q: 3) into a 1.000 liter volumetric flask, and suddenly realize that you don’t have all the reagents…

A:

Q: If NH4OH at 30.0 °C is 1.20 % ionized is 0.250 M solution, what is its ionization constant and the %…

A: Ionisation constant is also known as equilibrium constant  Which is equal to the ration of…

Q: dict the pH range of aqueous solutions of the following salts: KNO3, KHCO3, NH,F, and NH¼Br,…

A: The question is based on the concept of salt hydrolysis. We have to identify the nature of the salts…

Q: Calculate the final pH when 2.6 mmol NaOH is added to 1 mmole phosphoric acid, given pka1 = 2.1,…

A: Given, mol of NaOH = 2.6 mmol pKa1=2.1pKa2=7.2pKa3=12.4

Q: 1. Which of the following is/are true when NH4Br is dissolved in water? 1. Both NH4+ and Brare…

A: Ammonium bromide NH4Br is a salt. When it is dissolved in water NH4+ ion and Br- ion are formed.…

Q: (Q25) A buffer solution is prepared by adding 0.797 moles of formic acid and 0.866 moles of sodium…

A: ★ Answer : pH of the solution will be 4.027  ★ Solution :

Q: Which of the following will not produce a buffered solution? 100 mL of 0.1 M NaHCO3 and 25 mL of 0.2…

A: We know that, about Buffer solution this solution have tendency to resist the pH change when small…

Q: Using the table of the weak base below, you have chosen Aniline as your weak base in the buffer…

A: Given: Buffer solution of weak base aniline (assuming B) and its conjugate acid HB+. pH of solution…

Q: Based on this information, what mass of solid conjugate base should the student weigh out to make…

A:

Q: What is the pH of 0.075 M methylammonium bromide, CH3NH3Br?  (Kb of CH3NH2 = 4.4 × 10−4.)

A: The value of Kb for the given weak base methylammonium bromide is = 4.4x10-4 The concentration of…

Q: What combination of substances will give a buffered solution that has a pH of 5.05? (Assume each…

A: The Henderson Hasselbalch equation for basic buffer is given as : Given, Volume of solution =…

Q: Suppose you have just added 50.0 ml of a solution containing 0.0400 moles of weak acid HA to 500.0…

A: When weak acid is titrated with strong base, the resultant solutionwill have unionized acid and salt…

Q: Calculate the pH of each of the following buffered solutions.            Ka of acetic acid = 1.8 x…

A: Since you are asked for multiple sub parts, we are entitled to solve first three only.

Q: A chemist titrates 250.0 mL of a 0.0555 M methylamine (CH3NH₂) solution with 0.1413 M HNO3 solution…

A:

Q: Calculate how much of each solution you need to take to prepare 1 L of buffer solution with a pH of…

A: The question deals with the concept of Buffer preparation. by adding suitable amount of sodium…

Q: A chemist titrates 190.0mL of a 0.5533M ammonia NH3 solution with 0.8320M HCl solution at 25°C…

A:

Q: If NH4OH at 30.0 °C is 1.20 % ionized is 0.250 M solution, what is its ionization constant and the %…

A:

Q: Quinine (C20 H24 N2O2) is the most important alkaloid derived from cinchona bark. It is used as an…

A: Given :  pKb1 = 5.1  pKb2 = 9.7  Mass of quinine  = 1 gm  Volume of solution = 1930 ml

Q: You have been observing an insect that defends itself from enemies by secreting a caustic liquid.…

A: The relation given by Henderson Hasselbalch for calculating the pH of the weak acid solution is…

Q: Calculate the [H*] and [OH] in a solution prepared by diluting 0.10 mole of HCN and 0.10 mole of…

A: Given data is as follows: The moles of HCN = 0.10 mole The moles of NaCN = 0.10 mole The total…

Q: D,e,f

A: Given: Kb for NH2OH = 1.10×10-8

Q: 2.Aspirin (acetylsalicylic acid) is absorbed from the stomach in the free (non-ionized) acid form.…

A: The given data contains, pH = 2.59. pKa = 3.5

Q: bund in the human body? e Choose one or more: O HCOO /COO-;Ka = 1.77×10-4 O H3PO4/H2PO42-; Ka =…

A: Buffer solutions that can resist pH change upon addition of acid and base

Q: Caffeine is a weak base with a ?bKb of 4.1×10−44.1×10−4. Calculate the initial molar concentration…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Calculate the pH of the following mixture 500 ml 0.35 M CH3CH2NH2 + 500 ml 0.25 M HNO3

A: Given : The volume of CH3CH2NH2= 500 ml Molarity of CH3CH2NH2 =0.35 M The volume of HNO3=500 ml…

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.