A certain acid, HA, has a Ka given by: HA + H2O H3O* +A- Ka = 6.80 × 10-6 What is the pH of a 0.247 M aqueous solution of the acid's potassium salt, KA, which undergoes the hydrolysis reaction? A+ H2O # OH- + HA A) 4.72 B) 9.28 C) 4.11 D) 9.89 E) 9.44 O A O B O E

Q: 3) Aniline (B), shown below, is an organic base used in the manufacture of certain plastics. NH2 a)…

A: Given,   aniline is represented by B it is given that it is a base.

Q: -8 What would be the pH of a solution 5. The K, for hydroxylamine, HONH2, is 1.1 x 10 prepared by…

A:

Q: 13.3) The solubility of Ca(OH)2 at 20°C is 0.165 g/100 g H2O. The density of a saturated solution is…

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Q: Calculate Ka value for a .200 M solution of hypobromous acid (HBrO) with a hydronium ion…

A: Answer: On adding HBrO in water, its ionization will take place and hydronium ions will be produced…

Q: pH of the 0.025 M C65NH3Cl solution? (Ka=3.8*10^-10

A: C6H5NH3Cl is a salt of weak baseC6H5NH3Cl and strong acid HCl.pH for this type of salt is calculated…

Q: A 0.0200 M solution of a certain monoprotic weak acid is 18.0% ionized. What is the value of Ka for…

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Q: Calculate the pH when 29.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: Which of the following solutions will have the lowest pH value? A.) 0.10 M HNO3 B.) 0.03 M H2SO4…

A: Given acids: A.) 0.10 M HNO3 B.) 0.03 M H2SO4 C.) 1.0 M HCN (Ka = 4 X 10-10) D.) 2.0 M…

Q: Given Ka for HNO2 = 5.0 * 10 ^ - 4 1. What is the pH after the reaction of 30.0 mL of 0.25 M HBr…

A: Q1) According to the law of equivalence, an acid exactly neutralizes the same number of equivalents…

Q: b) A 0.0380 M solution of acetic acid (CH3COOH), a weak acid, with Ka = 1.8 x 10-5

A:

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 36.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Buffer Mixture is defined as an Aqueous solution which contains weak acid or weak base with its…

Q: What is the pH of 0.15 M solution of acetic acid (CH3COOH) Ka=1.75 x 10^-5 A) 2.6 x 10^-6 B) 0.0016…

A: Calculating pH of the acetic acid. CH3COOH + H2O <----------> CH3COO- + H3O+

Q: Calculate the pH when 20.0 mL of 0.150 M KOH is mixed with 42.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

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Q: A solution (total volume = 1L) of 0.4 M NH3 contains 12.78 g of NHẠCI (MW = 53.491 g/mol). Kb = 1.8…

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Q: What is the pH of a 0.25M NaCH3COO solution? (the Ka value for acetic acid is 1.76 x 10^-5)

A: Sodium acetate is a salt of a weak acid (CH3COOH) and a strong base (NaOH). Therefore, the pH…

Q: Consider that 20.0 mL of 0.10 M HA (an arbitrary weak acid, Ka= 1.5 × 10−6) is titrated with 0.10 M…

A: we have to calculate the pH of solution   after the addition of 5.0 mL of 0.10 M NaOH  after the…

Q: Calculate the pH when 32.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBRO (Ka = 2.5 x 10 9)…

A: Given data is as follows: The concentration of KOH =  0.150 M The volume of KOH = 32.0 mL The…

Q: You have a 0.189 M solution of propanoic acid.  You add enough sodium propanoateto make the solution…

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Q: Calculate the pH when 40.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

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Q: What is the pH of a solution of 0.85M HC2H3O2 and 0. 65M NaC2H3O2? The Ka for HC2H3O2 is 1.8 x 10^-5

A: Buffer Solution :- Buffer solution is prepared using weak acid and it's conjugate base of the weak…

Q: What is the pH for a solution with 0.10 MCH 3 COOH solution and 0.30 M CH 3 COONa? (K a for acetic…

A:

Q: Calculate the pH when 31.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: KOH + HOBr = KOBr + H2O Moles of HBrO = Molarity x volume in…

Q: 6) Which of the following has the highest hydroxide ion concentration? 0.1 M HCI 0.1 M H₂SO4 a…

A:

Q: Calculate the Ka of a weak monoprotic acid if a 0.10 M aqueous solution of the acid has a [H+] of…

A: An acid dissociation constant can be defined as the quantitative measure that is used to describe…

Q: Calculate the pH when 22.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A:

Q: a solution is made from 0.23 M CH3NH2 (a weak base) and 0.24 M CH3NH3Cl. what is the pH of the…

A: The pH of this buffer solution can be calculated by using Handersson-Hesselbalch equation-

Q: Consider that 20.0 mL of 0.10 M HA (an arbitrary weak acid, Ka= 1.5 × 10−6) is titrated with 0.10 M…

A:

Q: Q4: 30 ml with 0.2 M HOAC is diluted to 100 ml and titrated with 0.1 M NaOH. Calculate the pH when…

A: When half of acid is neutralized, it will form an acidic buffer solution in which [Acid ] =…

Q: A buffer solution is 0.308 M in H2 C204 and 0.252 M in NaHC204. If Kal for H2C2O4 is 5.9 x 10¬ª,…

A: The pH of a buffer solution prepared by mixing a weak acid with the salt of its conjugate base can…

Q: 1 out of Calculate the pH of a 0.40M solution of sodium acetate (NaCH,COO) given that the K, of…

A: NaCH3COO solution means salt hydrolysis. NaCH3COO is made up of weak acid acetic acid and strong…

Q: A buffer solution is 0.341 M in CH3COOH and 0.270 M in CH3COONa. If Ka for CH3COOH  is 1.8x 10^-5  ,…

A: The objective of this question is to calculate the pH of a buffer solution. The buffer solution is a…

Q: During the titration of 50.00 mL of a 0.289 M solution of propanoic acid ( HC3H5O2 ) with 0.155 M…

A: The balanced equation is HC3H5O2 (aq) + NaOH (aq) ----------> NaC3H5O2 (aq) + H2O (l)

Q: %3D What is the pH of a 0.1000 M NACH3COO solution? (Ka CH3COOH = 1.8x10^-5) 4.75 5.13 8.87 7.45…

A: We have find out pH of 0.1000 MNaCH3COO Solution.

Q: Can someone answer this question? My friends have three different answers 3.6, 3.47, and 1.6. Who is…

A:

Q: Calculate the pH when 6.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given : concentration of HBrO = 0.3 M and volume of HBrO solution = 20 mL = 0.020 L…

Q: )A solution made by dissolving 7.40 g of potassium hypochlorite (KClO) into 1.50 L of solution.…

A:

Q: Calculate the pH when 10.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given Molarity of KOH = 0.150 M Volume of KOH = 10 ml Molarity of HBrO = 0.300 M Volume of HBrO = 20…

Q: If a fifth solution (solution E) is made by mixing 10mL of soln C and 10mL of soln D, how will…

A: It is given that there are 4 solution which are sodium propanoate, propanoic acid, HCl and NaOH with…

Q: A solution contains 0.131 M sodium cyanide and 0.302 M hydrocyanic acid (Ka = 4.00 × 10-¹0). The pH…

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Q: 2. A solution contains 250 mL of 0.25M benzoic acid (HBen) and 0.20M sodium benzoate (NaBen). What…

A: Step 1:Ka= 6.5×10-5pka= -(log Ka)      =-(6.5×10-5)      = 4.18 Step 2:HCl is strong acid when added…

Q: Calculate the pH when 50.0 mL of 0.150 M KOH is mixed with 20.0 mL of 0.300 M HBrO (Ka = 2.5 × 10⁻⁹)

A: Given:Concentrations KOH  = 0.150 M    Volume = 50 mLHBrO = 0.300 M   Volume = 20 mLNow number of…

Q: What is the pH of a 0.0520 M solution of hydrocyanic acid, HCN (Ka = 4.9 × 10-10)? %3D

A: The dissociation constant(Ka) for a given reaction is defined as the ratio of concentration of…

Q: 4. A solution was prepared by dissolving 0.541 g of benzoic acid (HC,HSCOO) in 100 mL of water. The…

A:

Q: 2. Consider the weak acid phenol (C6H5OH), for which Ka = 1.05 x10-10 in aqueous solutions at 5°C.…

A: Given:  Concentration of phenol (C) = 0.850 M  Ka = 1.05 x 10-10

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.