Which of the following are likely to act as Lewis acids and which as Lewis bases? Explain. (a) AlBrs (b) CH3CH2NH2 (c) BH3 (d) HF (e) CH3SCH3 () TÍCl,

Q: A chemist takes 8.579 mL of liquid acetic acid, CH,COOH (molar mass: 60.052 g/mol) with 1.05 g/mL…

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Q: Which of the following is a feature of a Lewis acid?

A: Acid-base concept can be explained by various theories :-  Arrhenius theory  Bronsted-Lowry theory…

Q: What is the pH of a 0.660 M solution of NaCN (Ka of HCN is 4.9 × 10⁻¹⁰)?

A: The pH will be 11.56.

Q: Addition of phenolphthalein to an unknown colorlesssolution does not cause a color change. The…

A: a) Given :Addition of phenolphthalein: No color change               addition of bromthymol blue:…

Q: A solution is prepared by mixing 585 mL of 0.600 M NH3 and 320 mL of 0.600 M HCI. Assuming that the…

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Q: Ciprofloxacin is a member of the fluoroquinolone class of antibiotics.  Which nitrogen atoms are…

A: The structure of Ciprofloxacin is given below -

Q: Calculate the percent ionization of propionic acid 1C2H5COOH2 in solutions of each of the following…

A: The percent ionization of propionic acid is to be calculated

Q: A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05 g/mL…

A: Given, A chemist takes 8.579 mL of liquid acetic acid, CH₃COOH (molar mass: 60.052 g/mol) with 1.05…

Q: A 20-year-old student with coffee addiction had an episode of extreme hyperventilation due to…

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Q: A chemist takes 8.579 mL of liquid acetic acid, CH;COOH (molar mass: 60.052 g/mol) with 1.05 g/ml…

A:

Q: When titrating 15 mL of hydrazoic acid (HN3) 0.000489 mol/L, with KOH 0.000517 mol/L: What is the…

A: Here we are required to find the pH of the solution

Q: Based on their compositions and structures and on conjugate acid–base relationships, select the…

A: Given: BrO- or ClO-

Q: which of the following weak acids would be the best to use to make buffer solution of pH=7.2?

A: A buffer solution is a solution whose pH does not change by adding small amount of acid and base.…

Q: Which of the following are Lewis acids?

A: Lewis acid are the acids which an accepts electron pair. These chemical species contains empty…

Q: To increase the pH of 1.50 L of 0.25 M HCIO3 (aq), which of the following would you add to the…

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Q: Calculate the pH after0015 mole of gaseous HCI is added to2730 mL of each of the following buffered…

A: Given  Volume = 273.0 mL = 0.273 L a) 0.093 C6H5NH2 and 0.16 M C6H5NH3Cl First find initial moles of…

Q: A 20-year-old student with a coffee addiction had an episode of extreme hyperventilation due to…

A: The given information is: pH = 7.53 Conc. of bicarbonate ion = 22mmol/L The formula to calculate…

Q: Four unlabeled beakers in laboratory are filled with solutions of the following compounds: Na,S,…

A: In the given problem we are provide with four unlabeled beakers consisting of any of the following…

Q: A solution is prepared by mixing 25 mL of 0.06 M NaOH with 65 mL of 0.125 KOH. What is the pH of…

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Q: The value of K, for benzoic acid is 6.30×10-5. What is the value ofKg, for its conjugate base,…

A: Given: For Benzoic acid  The value of Ka = 6.30 x 10-5  For Conjugate base, C6H5COO- The value of Kb…

Q: Given a mixture of 100cm3 of 1.01M HCl and 400cm3 of 0.04 NaOH, calculate the pH of the solution.

A: We have given that Volume of HCl = V1 = 100ml Molarity of HCl = M1 = 1.01M Volume of NaOH = V2…

Q: A solution is prepared by mixing 400 mL of 0.500 M NH3 and 195 mL of 0.500 M HCI. Assuming that the…

A: Given-> Volume of NH3 = 400 ml Molarity of NH3 = 0.500 M Volume of HCl = 195 ml Molarity of HCl =…

Q: A 0.15 M solution of a certain weak acid has a pH of 4.00. The K, of the weak acid is

A: Given :-  Concentration of weak acid = 0.15 M  pH of solution = 4.00  To calculate :-  Ka

Q: The K, of a monoprotic weak acid is 0.00560. What is the percent ionization of a 0.127 M solution of…

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Q: expline buffer systems and acid-base titration curves    defthe Arrhenius, Bronsted-Lowry, and…

A: Note: As per guidelines can answer the first question. I was given an explanation for buffer systems…

Q: In the laboratory, a general chemistry student measured the pH of a 0.319 M aqueous solution of…

A: using the given PH using the PH calculate the H+ concentration . PH=-logH+ put the value pH  then…

Q: Suppose 0.0013 mol HA and 0.0013 mol A¯ are present in 170. mL solution and the pH is 4.00. What is…

A: Given: Moles of HA = 0.0013 mol. Moles of A- = 0.0013 mol. And the pH of the solution = 4.00

Q: An aqueous salution at 25C is 13-97. HNO3 by mass and has a density of +-048 g/m² what is the PH of…

A: Given data: Mass of HNO3 13.9% Density of solution is 1.048 g/ml To find: pH of solution

Q: How many grams of NaOH must be added to 250 mL of 0.10 M HC2H302 in order to bring the pH to 4.50?

A: To calculate the mass of NaOH, it is required to calculate the number of moles, which can be…

Q: Addition of phenolphthalein to an unknown colorless solution does not cause a color change. The…

A: Phenolphthalein and bromothymol blue are pH indicator. They ae widely used in titrations and testing…

Q: The value of K, for acetic acid is 1.80x10-5. What is the value of K, for its conjugate base,…

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Q: The pH of an aqueous solution of NaCN is 10.38. What is [CN-] in this solution?

A: NaCN is a salt of strong base (NaOH) and a weak acid (HCN). The solution is thus basic in nature.

Q: If a buffer solution is 0.280 M in a weak acid (?a=1.6×10−5) and 0.510 M in its conjugate base, what…

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Q: In the laboratory, a general chemistry student measured the pH of a 0.386 M aqueous solution of…

A: Note: As per our guidelines we are suppose to do only first question. To get the solution of other…

Q: To what volume should 160ml of any weak acid, HA, with a concentration 0.25 M be diluted to double…

A: The dissociation reaction of weak acid HA is  HA -----> H+ + A-

Q: If the ?a of a monoprotic weak acid is 7.5×10−6, what is the pH of a 0.30 M solution of this acid?

A: Given: The Ka of a monoprotic weak acid = 7.5×10−6 We have to calculate the pH of a 0.30 M solution…

Q: Ammonia, NH3, acts as an Arrhenius base, a Brønsted-Lowrybase, and a Lewis base, in aqueous…

A: First of all we must know about the Arrhenius base, Bronsted - Lowry base and Lewis base, Arrhenius…

Q: An aqueous solution at 25 C is 110% HNO, by mass and has a density of 1.046 g/mlL. What is the pH of…

A: Molarity of a solution is the number of moles of solute present in 1 liter of solution. The pH scale…

Q: Why do successive Kₐ’s decrease for all polyprotic acids

A: A polyprotic acid is an acid having the ability to donate multiple protons that dissociates in…

Q: In the laboratory, a general chemistry student measured the pH of a 0.558 M aqueous solution of…

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Q: The product of [H3O*] and [OH-] in water A. is greater than 1 B. decreases with pH C. increases with…

A: The pH is a method that determines the acidity and basicity of a solution. The pH of a solution is…

Q: Calculate the percent ionization of propionic acid 1C2H5COOH2 in solutions of each of the following…

A: The percent ionization or dissociation is termed as the percent dissociation of an acid varies with…

Q: At a certain temperature, a solution of ammonia at equilibrium is found to have concentrations of…

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Q: Which one of the following 1.0 M solutions would have the highest pH?

A: A large Kb value indicates the high level of dissociation of a strong base. A lower pKb value…

Q: Polymers are not very soluble in water, but their solubility increases if they have charged groups.…

A: Casein is the type of protein that is found in skim milk and coagulated at a certain pH. It is one…

Q: In the laboratory, a general chemistry student measured the pH of a 0.591 M aqueous solution of…

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Q: A solution is prepared that is initially 0.069M in ethylamine (C,H,NH,), a weak base, and 0.15M in…

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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.