If the Kp of a weak base is 2.4 x 10-6, what is the pH of a 0.47 M solution of this base? pH 0.00511 Incorrect

Q: what is the pH of a solution that is 0.40 M in sodium acetate and 0.60 M on acetic acid? (Ka for…

A: Determine the pH using Henderson-Hasselbalch equation.

Q: Calculate the Kb for the weak acid of Ka = 3.1 x 10-8. Calculate Ka for the weak base of Kb = 6.5 x…

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Q: • Calculate the pH of water sample with hydrogen ion concentration of 3.16 * 10-8 mols/L • Calculate…

A: pH = - log [H+]

Q: Calculate the hydroxide ion concentration, [OH ], for a solution with a pH of 3.72. (OH ] = 10 x1010…

A: From given data  pH = 3.72  Formula used  pH = -logH+...............................equation 1 H+OH-…

Q: The % ionization of a 0.015 M aqueous solution of an acid is 0.14 at 25 °C. What is Ka of this acid…

A: Let the acid be HA. So it will disociate as H+ + A- . Let the concentration of acid be denoted as C…

Q: Q3// Calculate the sodium acetate concentration that used in preparing a buffer solution with…

A: “Since there are multiple questions  and it is not mentioned that which one has to be solved , and…

Q: (Q11) lodic acid (HIO3) is a relatively strong weak acid (Ka = 0.17). What will be the equilibrium…

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Q: What is the pH of the solution?

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Q: If the K of a monoprotic weak acid is 4.0 x 10-6, what is the pH of a 0.10 M solution of this acid?…

A: In this question we have to tell the PH of the solution.

Q: For the diprotic weak acid H2A, Kal = 3.8 × 10-6 and K2 = 7.8 x 10-9. What is the pH of a 0.0750 M…

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Q: The pH of a 0.244 M solution of sodium methanoate, HCOO-Na+, is 8.57. Calculate Kb for the…

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Q: -3 The pH value of a (0.062 + 0.002) mol dm HCI solution is: Select one: 1.21 0.11 1.21 1 1.21 0.01…

A: There are two types of bases/acids. One is strong base/acid which is completely dissociable in into…

Q: The pH of a solution prepared by mixing 45.0 mL of 0.183 M KOH and 25.0 mL of 0.145 M HCI is O…

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Q: 6) What is the pH of an aqueous solution that is 0.1M NHẠC1? The Kb value for NH3 is 1.8 x 10-5…

A: Given Kb for NH3 = 1.8 * 10-5. The two ionization reactions are as follows: NH4Cl -------> NH4+ +…

Q: Q3/ Calculate the pH of a solution containing (0.1 M) of (Fe+] [Mg+]. knowing that Ksp is for…

A: Dissociation of Fe(OH)3 : Fe(OH)3 → Fe3+ + 3 OH- Ksp = 1 x 10-13 = [Fe3+] [OH-]3   Dissociation of…

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

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Q: What is the pH of a 0.370 M weak base solution? The Kp of the weak base is 0.000091. Your Answer:

A: Calculate PH [ OH-] = √KbC PH + POH = 14

Q: Calculate the pH and the pOH of an aqueous solution that is 0.030 M in HCl(aq) and 0.075 M in…

A: Given-> Concentration of HCl = 0.030 M Concentration of HBr = 0.075 M

Q: (Q17) What is the pH of a solution that is 0.404 M in sodium formate (NaCHO2)? The Ką of formic acid…

A: Given, Concentration of the sodium formate, NaCHO2 (C) = 0.404 M Ka of formic acid = 1.8 × 10-4…

Q: For the diprotic weak acid H2A, Kal = 3.5 x 10-6 and Ka2 = 7.7 x 10-9. What is the pH of a 0.0400 M…

A: Ka1>> Ka2  it means second dissociation is very small

Q: ind the α0 and α1 values of hypochlorous acid in a solution with a pH of 7.0. (Ka = 3x10-8 for HOCl)

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Q: A. Find the pH of a 0.325 M acetic acid solution. Ka = 1.8 x 10-5. B. Determine the % ionization for…

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Q: PH value 9.45 using 0.3 M Na2CO3 and 0.2 M HCl How much of each solution to prepare the 1 L buffer…

A: Solution:

Q: What is the pH of a 0.256 M C6H5CO₂H M solution if the K₂ of C6H5CO₂H is 6.5 x 10-5? Your Answer:

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Q: What is the pH of a 80.0 mL solution which is 0.27 M in IO¯ and 0.41 M in HIO? The Ka for HIO is 2.3…

A: 1- First calculate the pKa value of acid HIO :  We know that, pKa = -log(Ka)  pKa = -log( 2.3 ×…

Q: Calculate the pH of a solution formed by mixing 15.0 mL of 0.250 M HClO with 15.0 mL of 0.315 M…

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

A: Given that, HA ----> H+ + A-  [HA] = 0.11M , pH=4.80  Then,

Q: What is the pH of an aqueous solution that is 0.1M NH4Cl? The Kb value for NH3 is

A:

Q: What is the pH of an aqueous solution that is 0.1M NHẠC1? The Kb value for NH3 is 1.8 x 10-5 (Hint:…

A: Since NH4Cl is completely soluble in water, it is dissociated into NH4+(aq) and Cl-(aq). NH4+(aq) is…

Q: For the diprotic weak acid H2A, Kaj = 3.1 x 10-6 and Ka2 = 8.9 x 10-9. What is the pH of a 0.0550 M…

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Q: If the K, of a weak base is 7.2 x 10-6, what is the pH of a 0.33 M solution of this base? pH = 4.675…

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Q: What is the pH of a solution which is 0.021 M in weak base and 0.035 M in the conjugate weak acid…

A: The pH of buffer solution can be determined by using Handerson-Hasselbalch equation-

Q: Find the ph and the percent hydrolysis of a 0.0335 M solution of pyridine hydrochloride (the salt of…

A: Given : Concentration = 0.0335M

Q: constant 1.8×IO-5. Calculate the pH of the solution (1) addition 10 ml ,0.1 M NaOH. * (2) addition…

A: Given [CH3COOH] =[CH3COONa] =1M total volume = 1L therefore, no of moles of CH3COOH and CH3COONa= 1M…

Q: Question 1 Determine the molarity of a solution of the weak acid HCIO2 (Ka = 1.10 x 10-2) if it has…

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Q: 10. What is [H+] in M for a solution with PH=1 ]None of the others ]1 x 10–6 |1 x 10-10 |1 × 10-1 |1…

A: pH = -log[H+]

Q: 1) Find the α0 and α1 values of the hypochlorous acid in a solution with a pH of 7.0. (Ka = 3x10-8…

A: The α0 and α1 represents the relative concentration and can be determined by the concentration of…

Q: (8) Answer each of the following questions: (a) Ka for HNO₂ is 4.6 x 10-4. What is the Kb for its…

A: The pH of a solution is used to determine the acidity or alkalinity of a solution. The pH of a…

Q: A certain weak base has a Kp of 8.00 x 1'. What concentration of this base will produce a pH of…

A: The given pH is 10.31 Kb = 8.00 x 10-7 pOH = 14-10.31 = 3.69 [OH-] = 10-3.69 = 0.000204173

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.26. What is the Kb of this base?…

A: Weak base dissociated less in solution

Q: 0.350 M KCI 6.

A: pH of 0.350M KCl is

Q: 17. The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base? A. 4.4 x 10-8…

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Q: A 1.50 g sample of lithium nitrite, LiNO2, is added to 100.0 mL of water. Acid dissociation constant…

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Q: A solution of a weak acid, HA, has [HA] = [A-] = 0.301 M.  If the acid dissociation constant for the…

A: Given: [HA] = [A-] = 0.301 M Acid dissociation constant, Ka = 2.2 x 10-4

Q: What is the pH of a 0.31 M solution of NH4CIO4? Kp of NH3 is 1.8 x 105. Round tenth (X.X).

A: given data from question- conc. = 0.31 M Kb = 1.8×10−5 pH = ?

Q: PH? a. 10-3 M Acetate Acid b. 10-2 M Benzoic Acid

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

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Q: e proton concentrations of three solutions at 25 °C are given Basic Acidic Neutral Answer Bank [H]=…

A: If the pH of a solution is 7, then it is called a neutral solution.  If the pH of a solution is more…

Q: Lab Report #6-2-4: 0.1 M NagPO4 solution, using the given pH data, calculate value of (Ka or Kb) O…

A: The question is based on the concept of salt hydrolysis . we have to calculate the dissociation…

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.