.45 M solution of a newly discovered weak acid HZ has a pH of 2.60. What is the value of Ka for HZ?

Q: In a 0.735 M solution, a weak acid is 12.5% dissociated.(a) Calculate the [H3O+], pH, [OH-], and pOH…

A: Given data Concentration : C = 0.735 M % dissociation = 12.5  Suppose that weak acid (HA)…

Q: A 0.0722 M solution of a weak acid has a pH of 3.11. Calculate the Ka of this acid.

A: A weak acid is an acid that dissociates partially to give H3O+ in water. The dissociation of a weak…

Q: 5.3 The pH of a 0.1051 M of a monoprotic acid solution is 3.98. Calculate the Ka of the solution.

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Q: Calculate the Ka of a 0.35M weak acid HA if the pH of the solution is 2.97. Ka *** assume the…

A:

Q: In a 0.35 M solution, a weak acid is 2.8% dissociated.     (a) Calculate the [H3O+], pH, [OH−]and…

A: To calculate, we would use the given information .

Q: A 0.14 M weak acid solution has pH = 3.90. Determine Ka.

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Q: What is the ph of a 0.214 M weak base solution? The Kb of the weak base is 0.000033.

A: Given :-  Concentration of weak base = 0.214 M  Kb = 0.000033  To calculate :-  pH of solution

Q: Calculate the pH of a solution prepared by mixing 5.0 mL of a strong acid solution of pH 4.00 and…

A:

Q: What is the pH of a 0.627 M weak base solution? The Kb of the weak base is 0.000066.

A: Given :- concentration of weak base solution = 0.627 M  Kb for weak base = 0.000066  To calculate :-…

Q: A chemist dissolves 262. mg of pure hydrobromic acid in enough water to make up 390. mL of solution.…

A:

Q: Sid What is the pH of ammonium bromide solution with a concentration of 0.563 M. The base ionization…

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Q: The pH of an aqueous acid solution is 6.15 at 25 ° C. Calculate the Ka for the acid. The initial…

A: The equilibrium constant for acid dissociation is denoted as Ka. It represents the ratio of the…

Q: In a solution with a pH of 7.0, the hypochlorous acid is Find the values of α1. (Ka = 3x10-8 for…

A:

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0182 M solution. The pH of the…

A: Given : Concentration of monoprotic acid, HA (assuming it HA) = 0.0182 M And pH of solution = 2.68…

Q: How many moles of H₃O⁺ or OH⁻ must you add per liter of HA solution to adjust its pH from 3.15…

A: pH = -log [H+] pOH = -log [OH-]

Q: Calculate [H3O+] for a solution with a pH of 4.80.

A: We know that pH of solution = -log[H+] or…

Q: The pH of a 0.2 M solution of a weak acid HA is found to be 3.6. Calculate the Kb for A-

A: Wr will ionize HA , then calculate concentrations at equilibrium to find Kb .

Q: a) A 0.01M solution of ammonium chloride has a pH = 5.62 Calculate the basic ionization constant for…

A: (a) NH4Cl is a salt of a strong acid hydrochloric acid(HCl) and a weak base ammonium…

Q: concentration

A: [H+] = 10^-pH  [H+] = 10^-1.80  [H+] = 0.0158 M

Q: A 0.27M Solution of this week acid has a pH of 2.59 determine the Ka Of the weak acid

A:

Q: base has % ionization of 0.5%. What is the pH of 0.03 M solution of the base? a. 10.18 b. 1.50 c.…

A: GIVEN   % ionization is 0.5% Let         The base is NaOH and ionization of NaOH                NaOH…

Q: Find the pH of 0.010 moles of HCI in 10 liters of water.

A: Step : 1           Find the pH of 0.010 moles of HCI in 10 liters of water.

Q: In a 0.20 M solution, a weak acid is 3.0% dissociated.(a) Calculate the [H₃O⁺], pH, [OH⁻], and pOH…

A: Given, Molarity of solution = 0.20 M % of acid dissociated = 3.0% To find [H₃O⁺]? pH?  [OH⁻]?…

Q: What is the relationship between the acid ionization constant for a weak acid ( Ka ) and the base…

A: Acid is a compound that donates proton and base is a compound that accepts proton. The strength of…

Q: How is the equilibrium constant for a weak acid? A. Small B.Large C. neutral

A: The equilibrium constant may be explained as the mathematical expression which will be equivalent to…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0104 M solution. The pH of the…

A: Given, pH of the solution is 2.63 and the concentration is 0.0104M We can determine the Ka using the…

Q: Determine the pH of an HF solution of each of the following concentrations. In which cases can you…

A: HF undergoes dissociation as: HF+H2O→F-+H3O+

Q: A solution contains equal concentrations of an Acid and it's conjugate base. If the ka of the acid…

A: A mixture of a weak acid and its conjugate base (or a mixture of a weak base and its conjugate acid)…

Q: What is the ratio of acid to base in a solution having a pH=9?

A: Assume pKa of acid = 8.5

Q: A 0.350M solution of acetic acid has a pH of 2.60 @ 25°C. Determine the Ka of acetic acid.

A: Given, Concentration of acetic acid = 0.350M. pH of acetic acid = 2.60. The concentration of H+ can…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0147 M solution. The pH of the…

A: Since the acid is a weak acid so it dissociates partially so the degree of dissociation is not high.

Q: What is the Ka of a weak acid whose 0.10 M solution produces a pH of 2.38?

A:

Q: A 0.068 M solution of an unknown weak acid has a pH = 1.86. What is the Ka of the acid?

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Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0138 M solution. The pH of the…

A: Assuming the monoprotic acid is HA Hence the dissolution reaction of HA will be  HA ----> A- + H+…

Q: Iodic acid (HIO3) is fairly strong for a weak acid, having a K, equal to 0.16 at 25°C. Compute the…

A: odic acid, HIO3. It is a white water-soluble solid. Its robustness contrasts with the instability of…

Q: Enough of a monoprotic acid is dissolved in water to produce a 1.77 M solution. The pH of the…

A: Given: Concentration of monoprotic acid = 1.77 M pH of solution = 2.72

Q: The pH of a weak base (B) is 8.73 when the concentration of the weak base is 0.012 M. What is the…

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Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0154 M solution. The pH of the…

A: Let the monoprotic acid be HA. HA →H+ + A- Ka=[H+][A-][HA] where ka is the equilibrium constant for…

Q: What is the percent ionization of a 0.15 M solution of weak acid that has a pH of 1.86?

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Q: How many moles of H₃O⁺ or OH⁻ must you add per liter of HA solution to adjust its pH from 9.33 to…

A:

Q: 1. Calculate the percentage of ionisation of 0.1 M and 1.0 M acetic acid with pH 2.87 and 2.37…

A: For weak acid we have the following expression           H+=cαWhere concentration of acid is Cand…

Q: If a weak acid  (HA) has a Ka of 1.35 x 10-8, what is Kb for A-, the conjugate base.

A: If a weak acid (HA) has a Ka of 1.35 x 10-8, the Kb for A-, the conjugate base is to be calculated.

Q: Equal molar amounts of benzoic acid and sodium acetate are mixed together in water, is the resulting…

A: Kb for acetate ion = Kw/Ka = 10-14/1.7 x 10-5 = 5.88 x 10-10

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0120 M solution. The pH of the…

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Q: The pH of a 0.30 M solution of an acid, HA, has a pH = 5.20. Calculate Ka of HA

A: To calculate Ka of HA: The dissociation constant for the acid:

Q: An unknown weak acid with a concentration of 0.080 M has a pH of 1.80. What is the Ka of the weak…

A:

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0187 M solution. The pH of the…

A: concentration of solution = 0.0187 M pH of solution = 2.42 ka = ?

Q: The pH of a weak base (B) is 9.99 when the concentration of the weak base is 0.18 M. What is the…

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Q: If the pH of a 0.800 M solution of an acid is 3.45, calculate the % ionization of this acid and…

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Q: Calculate the the pH of a solution composed of 0.20 M ammonia and 0.15 M ammonium chloride?

A:

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.