Q1- SOLVE mathematically, then choose the correct answers: (42 marks) 1- Calculate the pH of solution made by combining 100 ml of 0.28 M HC;H;0; and 50 ml of 0.36 M NaOH, Ka for HC,H;0, =1.8 x 10~ a-3 b-3.68 c- 474 d-5 e- 6

Q: NH3: 1x10 tre 5. After you have calculated the pH of the solution with a mass percent of 3.00% NaOH…

A: Total mass of solution is 100gram Mass of NaOH = 3gram Density =1.0242gm/ml. Molarity of NaOH =…

Q: A 40.25 litre aqueous solution of a weak base, B-, has a concentration of 0.097 M.  The Kb -value…

A: Kb = 5.00 x 10-12 [BOH] = 0.097 M

Q: What is the pH of a solution prepared by dissolving 8.50 g C6H5NH3^+Cl^-in 750 mL of 0.258 M…

A: Given data is as follows: The mass of C6H5NH3+Cl- = 8.50 g The volume of C6H5NH2 = 750 mL The…

Q: What is the pH of a solution made by mixing 30.00 mL of 0.10 M HI with 40.00 mL of 0.10 M NaOH?…

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Q: 7-18. What is the pH of an aqueous solution that is 14.0% HCI by weight and has a density of 1.054…

A: Given information,      An aqueous solution that is 14.0% HCl by weight and has a density of 1.054…

Q: The pH of 225 mL of a 0.227 M solution of unknown weak base is 12.97. What is the Kb of this base?…

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Q: and 1. What is the autoionization of water? Give the reaction. Determine the pH, pOH, [H'], and [OH]…

A: As per the guidelines I am allowed to answer first one question at a time. I have solved all for…

Q: Write the equations that represent the first and third ionization steps for phosphoric acid (H3PO4)…

A: We will explain all the asked questions

Q: NH3 is a weak base (K, = 1.8 × 10-5) and so the salt NHCI acts as a weak acid. What is the pH of a…

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Q: Write the equilibrium expression for water’s self-ionization. What are the [H+], pH and pOH for pure…

A: The equilibrium expression for self ionization of water is : or Equilibrium constant: pH…

Q: The benzoate ion, C6H5COO-, is a weak base with Kb = 1.6 * 10-10. How many moles of sodium benzoate…

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Q: 5) if 125.0 ml water is added to 175.0 ml a strong acid solution of PH = 3. What should be the PH of…

A: Molarity : It is one of unit of the measurement of the concentration of a solution. It is defined as…

Q: The kb for a certain amine BNH2 is 8.6 × 10-6. Calculate the pH when 79.6 mL of 0.110 M BNH2 have…

A: Given, kb for BNH2 = 8.6 x 10-6 We have 79.6 ml (or 0.0796 L) of 0.110 M (or 0.110 mol/L)BNH2  no.…

Q: Determine the (H*]. [OH-], and pH of a solution with a pOH of 7.25 at 25 °C. [H*) = 1.8 x10-7 =…

A: Given that  POH= 7.25  We have to determine [H+] , [OH-]  and PH of a solution  Complete solution is…

Q: Like all equilibrium constants, the value of Kw depends on temperature. At body temperature (37 °C),…

A: The answer to the following question is given as:

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

A: An acid is a particular substance which upon dissociation in an aqueous medium gives H+ ions…

Q: The pHpH of a 1.00 MM solution of caffeine, a weak organic base, is 12.300. Calculate the KaKa of…

A: In this question,  we have to find the pH of solution by the use of Henderson hessalbalch equation,…

Q: How many grams of benzoic acid (CH:CO2H, 122.12 g mol", K = 63×10-7) is rquired t prepare an aqueous…

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Q: Calculate the pH of a 0.594 M aqueous solution of pyridinium chloride, C5H5NHCl. The Kb of pyridine…

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Q: What is the pH of a soluti on prepared by dissolving 3.00 g of the weak acid HA (molar mass = 138.12…

A: The question is based on the concept of chemical equilibrium. we have to calculate pH of the…

Q: Aspirin has the structural formula   At body temperature (37 °C), Ka for aspirin equals3 x10-5. If…

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Q: Sona Peycholegy Research P x app. 101edu.co Question 8 of 9 Calculate the pH when 40.0 mL of 0.150 M…

A: Given:  Concentration of HNO3 = 0.150 M  Volume of HNO3 solution= 40.0 ml = 0.04L  Concentration of…

Q: How much 0.500 M NaOH should be added to 12.0 g of tris hydrochloride to reach pH 7.77 in a final…

A: Given, Molarity of NaOH = 0.5 MAmount of tris-hydrochloride (T-HCl) = 12 gFinal pH = 7.77Final…

Q: A Moving to the next question prevents changes to this answer. estion 2 What is the pH of the…

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Q: (from the in class activity) - Suppose you dissolve three tablets of Sudafed (R), each containing…

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Q: The ionization constant for water (kw) is 2.9 × 10^-14 at 40 °C. Calculate [H3O], [OH], pH, and pOH…

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Q: Calculate the pH if 68mL of 0.150M ethylamine (pKb=3.252) is added to 68 mL of 0.128 M KOH. Assume…

A: Ethylamine is a weak base with pKb of 3.252. KOH is strong base. There is no reaction between strong…

Q: The following boxes represent aqueous solutions containinga weak acid, HA and its conjugate base,…

A: pH=It is defined by saying that a measurement of the level of acid or alkali  in a substance.…

Q: Calculate the pH of 0.606 M anilinium hydrochloride (C6H5NH3Cl) solution in water, given that Kb for…

A: pH of C6H5NH3Cl = to be calculated  Concentration of aniliniun hydrochloride = 0.606M Kb for aniline…

Q: In a 0.12 M solution of a weak monoprotic acid, HY, the acid is 5.0% ionized. Prepare the accurate…

A: Ionisation constant for weak acid is given as follows Ka = [H+][Y-] / [HY] [H+]= Concentration of H+…

Q: Which of the following is the pH of the solution containing 0.01 mol CH3COOH and 0.820 grams of…

A: Use the Henderson-Hasselbalch equation, which I have shown below: pH = pKa + log [[CH3COO-]…

Q: C6H₂O₂ + H₂O = HC6H₂O₂ + OH- K₂ = 1.7 x 10-5 for sorbic acid, HC6H7O₂ a The potassium sorbate…

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Q: What mass of aluminum hydroxide can be dissolved in a solution whose pH is held at 11.20? (Ksp of…

A: pOH = 14 - pH = 14 - 11.20 = 2.80  -log [OH-]  = pOH                    = 2.80    log [OH-] = -2.80…

Q: Acetic acid (CH3COOH) is a product of many microbial metabolisms. It forms acetate ion and a…

A: Weak acids are not completely dissociated into ions in an aqueous solution. So, when it is dissolved…

Q: 16.46. (D)

A: Given information: Volume of Ba(OH)2 solution = 20.0 mL Concentration of Ba(OH)2 solution = 0.015 M…

Q: What is the pH of a solution prepared by adding 2.37mL of 1.78 M HCL to 0.664L of .399 M weak base,…

A:

Q: I'm not sure what this question wants me to solve for

A: Note: Assuming that question is to calculate the diluted HCl concentration.

Q: What is the pH of a solution made by mixing 30.00 mL of 0.10 M HCl with 40.00 mL of 0.10 M KOH?…

A:

Q: Calculate the pH of a solution containing 0.70 M HC2H302 and 0.25 M NaczH302. The K, for HC,H;0, is…

A: Given :-  Ka for HC2H3O2 = 1.8 × 10-5 concentration of HC2H3O2 = 0.70 M  concentration of NaC2H3O2 =…

Q: What is the pH of a 75.0mL of a 0.1M pyridine (C5H5N) solution (kb = 1.7 x 10 -9) when 100mL of a…

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Q: The pH of blood plasma is 7.40. Assuming that the principal buffer system in blood is HCO, /H2CO3,…

A: Given,  pH of blood plasma = 7.40

Q: NH3 is a weak base (K, = 1.8 × 10-') and so the salt NH4CI acts as a weak acid. What is the pH of a…

A: Given, Concentration of NH4Cl solution = 0.075 M Kb for NH3 = 1.8 × 10-5 pH of the solution = ?…

Q: How many milliliters of 0.500 M NaOH should be added to 10.0 g of tris hydrochloride to give a pH of…

A: Given data contains, Molarity of sodium hydroxide is 0.500 M. Amount of tris hydrochloride is 10.0…

Q: Referencen) What volume of 0.0830 M NaOH must be added to 100. mL of 0.100 M NAHC0, to reach a pH of…

A: Volume of NaOH needed can be calculated from the Henderson hasselbalch equation the concentration of…

Q: NH3 is a weak base (K, = 1.8 × 10-5) and so the salt NH¼C1 acts as a weak acid. What is the pH of a…

A: Given : concentration of NH4Cl = 0.088 M Since the salt given is a soluble ionic salt. Hence it will…

Q: 7

A: The salt given is NH4C3H5O2.

Q: 5. Calculate the pH of a solution that is 0.050 M NH, and 0.150 M NH,CI. The Ka=5.62 x 10-10 for…

A:

Q: Consider a 1.O-L solution that is initially 0.640 M NH3 and 0.610 M NHẠCI at 25 °C. What is the pH…

A: Given, concentration of NH3=0.640 Mconcentration of NH4Cl = 0.610Mmoles of NaOH = 0.104 molKb of…

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.