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?

Q: weak monoprotic acid (HA) has an acid ionization constant Ka = 1.8x10° at 298 K. If 100 mL of a 0.10…

A: First write equilibrium equation for reaction of weak acid and strong base and fine limiting…

Q: Hydrocyanic acid, HCN, is a weak acid (Ka = 4.02*10-10). If I dissolve 0.882 g of HCN in enough…

A: Given information is as follows: The amount of HCN = 0.882 g The volume of water = 600 mL The value…

Q: A 0.17 M solution of a weak acid has a pH of 2.85. What is the ka of the weak acid?

A: Given: concentration of weak acid=0.17M              pH of weak acid=2.85 To calculate: Ka of weak…

Q: If the Ka of a monoprotic weak acid is 3.1x10-6, what is the pH of a 0.15 M solution of this acid?

A: Ka of monoprotic acid (HA) = 3.1×10-6[HA] = 0.15 M

Q: A weak acid, HA, is a monoprotic acid. A solution that is 0.220 Min HA has a pH of 2.440 at 25°C.…

A: The objective of the question is to find the acid-ionization constant, Ka, for the weak acid HA and…

Q: For the diprotic weak acid H2A, ?a1=3.7×10−6 and ?a2=6.2×10−9. What is the pH of a 0.0450 M…

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Q: Aspirin, a drug that is used to relieve minor aches and pain, is a weak monoprotic acid. What is the…

A: we know that pH = -log [H+] so -log [H+] = 3.12 [H+] = 0.000758

Q: Calculate pH of the following solutions: a) 0.25 M HNO3 in 0.065 M CH3COOH (K,=1.75x10). b) 0.33 M…

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Q: None

A: Step 1:Since H2A is a weak diprotic acid, it can donate two H+ ions. We will find the concentration…

Q: A beaker holds a mixture of 0.40 M HIO3 and 1.0 M HCOOH. Ka(HIO3) = 1.6 x 10-¹ Ka(HCOOH) = 1.77 ×…

A: We know weak acids having lower value of dissociation constant Ka ionise weakly so can ignore their…

Q: A diprotic acid (H2A) has ?a1=4.84×10−7 and ?a2=5.65×10−11. What is the pH of a 0.424 M H2A…

A: Answer:-This question is answered by using the simple concept of calculation of pH of a weak acid…

Q: You are studying a clear solution and you added the pH indicator methyl violet. The colour range of…

A: The color of a solution of pH 0.2 is needed to be determined on the addition of an acid-base…

Q: hydroxide

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Q: what is the ph of a solution that is 0.100 m in hydrofluoric acid? The Ka of hydrofluoric acid is…

A: Recall the following expression to find pH of the given solution of hydrofluoric acid. Given that…

Q: The pH of a 1.86 M solution of a weak monoprotic acid, is 2.31.  What is the Ka of the acid?

A: Given  pH = 2.31 Concentration of acid = 1.86 M Ka =?

Q: Calculate the pH of a 0.350 M solution of benzoic acid. Benzoic acid is a weak monoprotic acid with…

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Q: What is the pH of a solution of 0.79 M acid and 0.55 M of its conjugate base if the ionization…

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Q: A 0.0720 M solution of a monoprotic acid is known to be 1.52% ionized. What is the pH of the…

A: Concentration of solution of monoprotic acid = 0.0720 M Percent ionization = 1.52%

Q: Chloroacetic acid, HC2H2ClO2, has a greater acid strength than acetic acid, because the…

A: Since you have asked multiple question, we will solve the first question for you. If you want any…

Q: 6a) Write the hydrolysis reaction of hypochlorous acid Clearly identify the acid, base, conjugate…

A: Given data:Concentration of solution of acid =0.050 MDetermine the hydrolysis reaction of…

Q: The pH of a 0.45 M solution of a weak acid, HA, is 2.13. What is the value of Ka for the weak acid?

A: Given data,pH=2.13Molarity of HA=0.45

Q: A 0.037 M solution of a weak acid (HA) has a pH of 4.34. What is the Ka of the acid?

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Q: The pH of a 0.154 M solution of a weak acid, HB, is 2.72. What is K, for the weak acid?

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Q: "Acid rain" forms when rain falls through air polluted by oxides of sulfur and nitrogen, which…

A: 1) Here given---- pH of the acid rain = 3.41 We know---- pH = - log [H+] Or, [H+] = 10-pH  Now…

Q: The pH of a 0.0040 M solution of Ca(OH)₂ is

A: Given, Concentration of Ca(OH)2 solution = 0.0040 M So, [OH-]= 2×0.0040 M= 0.0080 M

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: To calctulate the pH, we would use Ka or Kb expression.  “Since you have posted multiple questions,…

Q: Phenol is a weak acid with a Ka = 1.28 x 10-10.  As a pure compound, it is rather corrosive but in…

A: Phenol (PhOH) will give the below reaction in water. PhOH ----> PhO- + H+ assuming a…

Q: If a buffer solution is 0.170 M in a weak base (?b=3.7×10−5) and 0.540 M in its conjugate acid, what…

A: In question it is not mentioned whether the base is monoprotic or polyprotic. Hence assuming it to…

Q: A weak acid, HA, is a monoprotic acid. A solution that is 0.220 Min HA has a pH of 2.440 at 25°C.…

A: The objective of this question is to calculate the acid-ionization constant, Ka, for the weak acid…

Q: Calculate the pH of the following aqueous solution:           0.40 M NH 4Cl (p K b for NH 3 = 4.74)

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Q: If a buffer solution is 0.200M in a weak acid (?a=9.0×10−5)and 0.550M in its conjugate base, what is…

A: Ka = 9.0 x 10-5  pKa = -log Ka = - log ( 9.0 x 10-5)  pKa = 4.046 [Acid] = 0.200 M  [Conjugate base]…

Q: what is the pH?

A: Given :-  Concentration of weak base = 0.120 M  Concentration of conjugate acid = 0.590 M  Kb = 5.9…

Q: Calculate the pH of a 0.30 M solution of HCN (weak acid). Ka for HCN is 4.9 x 10-10

A: Given: Concentration of the HCN solution = 0.30 M Ka for HCN = 4.9 × 10-10 We have to calculate the…

Q: For the diprotic weak acid H2A, ?a1=2.9×10−6 and ?a2=8.2×10−9. What is the pH of a 0.0650 M solution…

A: Diprotic acid is dibasic acid which has two acidic H+. This will dissociate two times.

Q: Calculate the magnitude of the equilibrium constant for benzoic acid, HC7H5O2, if a 0.100 M solution…

A: The benzoic acid represented as C6H5COOH. It is a weak acid and dissociate into hydrogen and…

Q: A new potential cure for the common cold, code-named Z-123, is being tested by a pharmaceutical…

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Q: The pH of a 0.0492 M solution of a weak acid is 2.641. What is the Ka of the acid?

A: pH= 2.641

Q: The pyridinium ion (C5H4NH*) is a weak acid (Ka = 5.60 x 10-6). Calculate the pH of a solution that…

A: Given that, the pyridinium ion is a weak acid. The Ka of it is Ka = 5.60×10-6. 3.7 mL of 0.167 M of…

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.