A solution is made by dissolving 18.7 g of CH3NH3NO3 in 500.0 mL of water. What is the value of Ka for CH3NH3+? The Kb of CH3NH₂ is 4.4 × 10-4.

Q: The value of Ka for phenol (a weak acid) , C6H5OH , is 1.00×10-10 . Write the equation for the…

A: Given:-           The week acid is reacts with water to produce the conjugate base and hydronium…

Q: NH3 is a weak base (Kb = 1.8 x 10-5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

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Q: The Ka for four acids are H₂CO3: 4.5 x 10-7, HCO₂H: 1.8 × 10-4, H3C,H,O,: 7.1 x 10-4, HCN: 6.2 x…

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Q: CH3CH2CO2H , Ka = 1.3 x 105 CH3CH2CO2, Kb = 7.7 x 10-10 F, Kb = 1.4 x 10-11 HF , Ką = 7.2 x 10-4 For…

A: Conjugate acid formed when an acid donates a proton to a base  Conjugate base is formed when a…

Q: what is the Ka or Kb value of the solution NaC2H3O2 when the pH is 7.24?

A: The relation between the acid-dissociation constant (Ka) of an acid and the base-dissociation…

Q: Propanoic acid HC3H5O2, has a Ka of 1.3 x 10-5. What is the [H3O+] in a (1.51 x 10-1) M solution of…

A: The ionization of Propanoic acid HC3H5O2 takes place as,                             HC3H5O2 (aq)  +…

Q: Calculate [H+] for a 3.00×10-4 M aqueous solution of cinnamic acid (HC9H7O2; Ka = 3.70×10-5)

A: The acid (say HA) dissociates in water to produce corresponding  ion and hydronium ions.          HA…

Q: what is the concentration of CH3COOH in NaCH3COO 0,4 M solution (ka = 10^-5)

A: To determine the concentration of CH3COOH in a solution of NaCH3COO, you need to consider the…

Q: What is the pH of the solution of 35 mL 0.20 M formic acid and 55 mL 0.10 M sodium formate in 110 mL…

A: Molarity of formic acid = 0.20M Volume of formic acid = 35mL Molarity of sodium formate = 0.10M…

Q: What is the pH of a 2.4 M solution of H2CO3? (Ka of H2CO3 = 4.3 x 10-7, Ka of HCO3- = 7x 10-11)

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Q: What is the pH of a solution that is 0.15 M NH4Cl and 0.35 M NH3?   The Ka of NH4Cl is 5.01 x…

A: In this question , we have to calculate the correct pH of given problem by the help of…

Q: The value of Ka for phenol (a weak acid) , C6H5OH , is 1.00×10-10 . Write the equation for the…

A: Phenol is weak acid as the given in question so it will deprotonated by the release of H+ and we get…

Q: What is the pH of 2*10-3 M Na2HPO4?

A: we need to consider the dissociation of the compound and the equilibrium constants involved. In the…

Q: ph of a 30.0 ml sample of 0.1 M HOAc is 3.22, what's the equilibrium [H+] and the Ka value?

A: Given :- pH is 3.22 of a 30.0 mL sample of 0.1 M HOAc. To calculate [H+] & Ka value.  Now, HOAc…

Q: If the ph of  24.0 ml of 1.0 M NaOAc is added to 1.0 M of HOAc is 4.97, what's the equilibrium [H+]…

A: The value of pH is given by the following equation pH= -log [H+] Or,  [H+] = 10-pH pH of a buffer…

Q: What would be the pH of a/solution made by adding 100.00 mL of 0.100 M NaOH to 100.0 mL of 0.100 M…

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A: We wil calculate value of kb

Q: Carbonic acid (H2CO3) and bicarbonate ion (HCO3-) are used as a buffer system to regulate the blood…

A: Given:

Q: 85. Formic acid (HCO₂H) was first isolated by the destruc- tive distillation of ants. In fact, the…

A: Answer:HCOOH is a weak organic acid and when added in water, its partial ionization takes place and…

Q: 2. A 0.0560 g quantity of acetic acid is dissolved in enough water to make 50.0 mL of solution.…

A: Welcome to bartleby !

Q: 7, Calculate the [H3O+] of a 0.110 M acid solution; Ka=5.45 x 10-7 Group of answer choices 4.55 x…

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Q: What is the pH of the solution that is prepared by dissolving 0.844 g of lactic acid (90.08 g/mol,…

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Q: Acetic acid,  CH3COOH , has a  Ka of  1.8×10−5. Calculate  Kb  for the acetate ion.

A: Given, Ka for Acetic acid = 1.8 × 10-5 Kb for acetate ion = ? Note:  Kw = 1.0 × 10-14

Q: What is the concentration of every major component in a 0,10 M acetic acid (CH3COOH)? Ka of acetic…

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Q: What is the pH of the solution that is prepared by dissolving 0.8 g of lactic acid (90.08 g/mol, Ka…

A: We have given that  What is the pH of the solution that is prepared by dissolving 0.8 g of lactic…

Q: What is the pH of a solution when 33.4 g of methylammonium chloride. CH3NH,CI, is dissolved in…

A: Provided dataVolume of solution is 514.2 mL or 0.5142 L.Mass of the sample(CH3NH3Cl) is 33.4…

Q: What is the hydroxide ion concentration of 2.0 x 10-6 M NaOCl solution (Ka=3.0x10-8)?

A: molarity = 2.0 × 10-6 M Ka = 3.0 × 10-8  OH- = ?

Q: Propanoic acid (CH3CH2COOH) has a Ka of 1.3×10–5. FW(propanoic acid) = 74.08 g/mol; FW(calcium…

A: Buffers are generally good over the range pH = pKa ± 1. For example, the acetate buffer would be…

Q: If 10.0 ml of 1.0 M NaOC and 1.0 M HOAc has a ph of 4.98, what is the equilibrium [H+] and ka value?

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Q: If vinegar contains 4% (w/v) of acetic acid (Ka= 1.8x10-5), calculate the pH of solution made by…

A: Q.1:  Before dilution:  concentration, C1 = 4%(w/v)  Volume, V1 = 50 mL  After dilution:…

Q: Periodic acid, HIO4, is an important oxidizing agent and a moderately strong acid. In a 0.10 M…

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Q: If you mix 125.0  mL of 0.50 M CH3CO2H with 75.0 mL of 0.83 M NaOH, what is the pH of the resulting…

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Q: What is the weight of pyridine, CSH§N that must be dissolved in 250 mL of solutic to produce a…

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Q: What is the pH of a solution made from adding 15.00 mL of 0.11 M Na₂HASO to 28.00 mL of 0.21 M Na…

A: Answer:Buffer solution is a type of solution that resists the change in its pH on adding small…

Q: ASA (also known as AspirinTM) contains acetylsalicylic acid, C16H12O6. Acetylsalicylic acid is a…

A: Given, ASA (also known as AspirinTM) contains acetylsalicylic acid, C16H12O6. Acetylsalicylic acid…

Q: What is the concentration needed of hypochlorous acid (a weak organic acid) needed to reach a pH of…

A: Given, PH= 4.75  Ka = 2.9 x 10-8

Q: If the ph of a 30.0 mL sample of 1.0 M NaOAc is 9.33, what's the equilibrium [H+] and the Ka value?

A: PH = -log[H+] NaOAc is the salt of strong base and weak acid.

Q: Benzoic acid has a Ka - 6.3 × 10-5. What is the percent ionized in a 0.13 M solution of benzoic…

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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.