The pH of a 0.22 M aqueous solution of a weak acid at 25.0 °C is 4.50. What is the value of Ka for the weak acid? O 1.4 x 10-4 O 2.2 x 10-6 none of the above O 1.0 x 10-9 O 4.5 x 10-9

Q: Calculate the [H3O+] of a 0.390 M acid solution; Ka=4.52 x10-5

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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: Z is a weak base. An aqueous solution of Naz is prepared by dissolving 0.350 mol of Naz in…

A: Dear student I have given answer to your question in the image format.

Q: What is the Ka of cyanuric acid if a 0.030 M cyanuric acid aqueous solution has a pH of 4.15? O…

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Q: Find the percent ionization of a 0.337 M HX solution. The Ka for HX is 3.5 x 104. Select one: O 3.2…

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Q: What is the [H] of an aqueous solution with a pH of 6.2? 3.2 x 10-5 M 6.2 x 10-6 M 6.3 x 10-7 M 1.6x…

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Q: What is the pH of a 0.24 M solution of sodium propionate, NaC3H5O2, (base) at 25°C? (For propionic…

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Q: Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 8.32. O 5.7 O 8.3 x…

A: pOH of an aqueous solution is 8.32 .We have to calculate the molarity of hydroxide ion in the…

Q: What is the equilibrium concentration of H2C204 in a 0.170 M oxalic acid, H2C2O4, solution? For…

A: Let α  be the degree of dissociation of H2C2O4:                          H2C2O4    ↔       HC2O4-  +…

Q: A 1.0 M solution is made with the imaginary polyprotic a For this acid, Ka1 = 1x 10-6 and K2 = 1 x…

A: Here we have to determine pH of 1.0M aqueous solution of polyprotic acid H2A. Ka1=1×10^-6 and Ka2=…

Q: What is the k a of a monoprotic weak acid if a 0.825 M solution has a pH of 2.046?…

A: Given: The reaction is as follows: HA(aq)------------>H+(aq)+A-(aq). The concentration of…

Q: HF is a weak acid. Which reaction do you predict has an equilibrium constant less than 1? O None of…

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Q: What is the k a of a monoprotic weak acid if a 0.206 M solution has a pH of 3.403?     1.32x10-7…

A: Given Concentration of weak acid = 0.206 M pH of weak acid = 3.403

Q: D Question 2 For the following solution, calculate the pH. K = 1.8 x 10-5 0.15 M CH3COOH Question 3…

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Q: What is the k a of a monoprotic weak acid if a 0.250 M solution has a pH of 1.858?

A: Given :- pH of weak acid solution = 1.858  initial concentration of acid = 0.250 M  To calculate :-…

Q: What is the hydroxide ion (OH)concentration of a 0.0325-M solution of ammonia, a weak base with a Kp…

A: We have 0.0325 M solution of ammonia with Kb as 1.76*10-5 . We have to calculate the hydroxide ion…

Q: Which of the following bases would have the highest pH value? 0.1 mol/L NaOH 0.1 mol/L Ca(OH) 2 55.5…

A: pH is defined as the negative logarithm of hydrogen ion concentration. pH = -log [H+] According to…

Q: What is Ka for a weak monoprotic acid if a 0.020 M solution of the acid has a pH of 3.28 at 25°C? O…

A: To find Ka value of a weak acid, first find out hydronium ion concentration and from that find out…

Q: 0.1 M solution of the acid has pH = 4.70. What is K₁ of the acid?

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Q: The [OH] in a 0.20M solution of NH4OH is: (Kb for NH4OH = 1.8 x 10-5) 3.6 x 10-6 M O 1.8 x 10-5 M…

A: Given: Initial concentration of NH4OH=0.20 M Kb of NH4OH = 1.8×10-5 Let x be the dissociated amount…

Q: A solution of CSH5N (pyridine, Kp = 1.7 x 10 °) has a pH of 9.40. What is the [C5H5N]? O 9.3 x 1011…

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Q: What is the k a of a monoprotic weak acid if a 0.932 M solution has a pH of 4.456?   a 3.50x10-5…

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Q: Which of the following statements is/are TRUE regarding a 0.20 M solution of the strong acid, HX? 1.…

A: Here we are required to find the statement true about strong acid.

Q: The pH of a 0.55 M aqueous solution of hypobromous acid, HB1O, at 25.0 °C is 4.48. What is the…

A: The percentage of ionization of HBrO can be calculated as follows

Q: A solution of a weak acid contains 5 mM conjugate acid (HA), 2.5 mM conjugate base (A-), and 2.5 mM…

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Q: NH3 is a weak base (Kp = 1.8 x 10³) and so the salt NHĄCI acts as a weak acid. What is the pH of a…

A: At Temperature 25°C Kb (NH3) = 1.8 × 10-5 [NH4Cl] = 0.028 M

Q: Which aqueous solution has the lowest pH at 25 °C? 0.45 M H2S O 0.35 M HF O 0.34 M HOCIO O 0.33 M…

A: Answer :-  0.33 M HBr has lowest PH at 25 °C

Q: 6. A 0.495M solution of nitrous acid, HNO2, has a pH of 1.83. Find the percent ionization of nitrous…

A: Given: pH of the acid =1.83, Concentration of acid is = 0.495 M To find: Percent ionization of acid.…

Q: What is the pH of a 0.250 M weak acid solution, if the K₂ of the acid is 3.22 x 10-5? 1.86 2.55 3.29…

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Q: What is the k a of a monoprotic weak acid if a 0.619 M solution has a pH of 4.242?

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Q: Calculate the molarity of hydroxide ion in an aqueous solution that has a pOH of 3.00. O O 11.00 3.0…

A: pH = -log[H+] pOH = -log[OH-]-> pH < 7 , it is acidic and [H+] > [OH-]-> pH > 7 ,it…

Q: Determine the Ka of an acid whose 0.294 M solution has a pH of 2.80. ○ 5.4 x 10-2 ○ 4.9 x 10-7 8.6 x…

A: The problem is asking us to find the Ka, or acid dissociation constant, of an acid. The Ka is a…

Q: What is the pOH of 0.003M acetic acid solution (Ka = 1.8 * 10 ^ - 5) O 11.4 O 10.4 O 3.3 O 4.6…

A: pH is defined as negative logarithm of hydrogen ion concentration.

Q: The base protonation constant K of ammonia (NH3) is 1.8 × 10 Calculate the pH of a 1.2 M solution of…

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Q: What is the pH of the following solution? 30.0 mL of 0.41 M HOCI (Ka = 2.8 x 10-8) is added to 30.00…

A: We have to calculate the pH of solution

Q: Calculate the pH of a 0.025 M solution of propanoic acid (K, = 1.3 x 10-5). 7.48 0.025 O 5.6 x 104…

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Q: CH3NH, is a weak base with K, = 4.0 x 104. What is the pH of a 1.0 M solution of CH3NH;CI? O 5.3 O…

A: Here salt is a combination of weak base and strong acid so we can determine pH by applying…

Q: The acid-dissociation constant at 25.0 °C for hypochlorous acid (HC10) is 3.0 - 10-8. At…

A: Dear student this question is related to equilibrium concept.

Q: A solution is made with 3.825 g NH,CI, dissolved in enough water to make 625 mL of solution. If the…

A: First, we calculate the concentration of the solution. After that, we calculate the [OH-] with the…

Q: A solution of CgH5N (pyridine, Kp = 1.7 x 10) has a pH of 9.40. What is the [C;H5N]? O 0.37 9.3 x 10…

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Q: What is the pH of a solution that is 0.063 M in HA and also 0.023 Min NaA? (Ka = 4.1 × 10- O. 5.46…

A: Given: The concentration of HA is 0.063 M The concentration of NaA is 0.023 M The Ka value is 4.1 x…

Q: Find the pH of the 0.04 M Na3PO4 solution. (Ka1= 7x10-3, Ka2= 2.2x10-7 , Ka3= 4.5x10-13) P.s:…

A: The dissociation of Na3PO4 is: Na3PO4⇌3Na++PO43- The hydrolysis reaction of PO43- OR equilibrium…

Q: What is the pH value for a 5.5 x 10-3 M aqueous solution of hydrogen sulfate? O-1.96 O 1.96 O 0.51…

A: pH of a solution is defined as the negative logarithm of hydronium ion concentration.Mathematically,…

Q: Water (H,O) acts as a Brønsted-Lowry base in which of the fallowing equilibrium reactions? HCO, +…

A: According to Bronsted-Lowry theory,  acids are the species which donate protons and bases are the…

Q: 1.0 x 10 11 moles of HCl are added to 1.0 L of H2O. What is the pH? O 10.0 O 11.0 3.0 o 7.0

A: Moles of HCl = 1.0 × 10^-11 mole Volume of H2O = 1.0 L

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.