An unknown weak acid with a concentration of 0.091 M has a pH of 1.80. What is the Ka of the weak acid?

Q: HC3H5O2 is a weak acid. A 0.25 M solution of HC3H5O2 has a pH of 2.74. The Ka of HC3H5O2 is?…

A: Please find your solution below :

Q: A 0.110 M solution of an unknown weak acid has a pH of 4.35 at 25 degrees celsius. What is the…

A: The concentration of hydronium ion in solution can be calculated by using PH equation Ka for weak…

Q: An unknown weak acid with a concentration of 0.530 M has a pH of 5.600. What is the Ka of the weak…

A: Given, Concentration of the unknown weak acid (C) = 0.530 M pH of the solution = 5.60  Ka for weak…

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 0.00959 M solution of a weak base has a pH of 9.33. What is the Ka for its conjugate acid?

A: Concentration of OH- is calculated as follows,

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0143 M solution. The pH of the…

A: Given :-  Concentration of weak acid solution = 0.0143 M  pH of solution = 2.59  To calculate :  Ka…

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

A: The solution is as shown below:

Q: An unknown weak acid with a concentration of 0.350 M has a pH of 5.600. What is the Ka of the weak…

A: given, the concentration of weak acid (c) = 0.350M pH = 5.600

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.

A:

Q: An unknown weak acid with a concentration of 0.310 M has a pH of 5.600. What is the Ka of the weak…

A: Give data, Molarity of HA = 0.310M pH = 5.600 Equilibrium constant is defined as the ratio of…

Q: Enough of a monoprotic weak acid is dissolved in water to produce a 0.0137 M solution. The pH of the…

A: Since the acid is weak monoprotic acid. Hence we can assume it to be HA

Q: The Ka of a monoprotic weak acid is 0.00638. What is the percent ionization of a 0.127 M solution of…

A:

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

A:

Q: Determine the Ka of a weak acid HA that has a concentration of 0.025 M and a pH of 4.09 at 25°C.

A:

Q: An unknown weak acid with a concentration of 0.320 M has a pH of 5.600. What is the Ka of the weak…

A: HA  ↔ H+ + A-Writing equilibrium expression for the above weak acid,Ka = [H+] [A-][HA]  But at…

Q: B. If the pH of a weak acid solution is 2.500 and the solution has a concentration of 0.100M, what…

A: Given: pH = 2.5 Concentration = 0.100M

Q: concentration

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

Q: An unknown weak acid with a concentration of 0.290 M has a pH of 5.600. What is the Ka of the weak…

A: For weak acid,pH=12(pKa-logC)Where, C is concentration in M unit

Q: An unknown weak acid with a concentration of 0.140 M has a pH of 5.600. What is the Ka of the weak…

A:

Q: A weak base, B, has a concentration of 0.155 M. If the pH of the solution is 11.24, what is the K of…

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Q: solution that shows a pH of 11.70 has a  [H+] of what?

A:

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: HZ is a weak acid. An aqueous solution of HZ is prepared by dissolving 0.020 mol of HZ in sufficient…

A:

Q: An unknown weak acid with a concentration of 0.067 M has a pH of 1.80. What is the Ka of the weak…

A:

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: The Ka of a monoprotic weak acid is 0.00836. What is the percent ionization of a 0.145 M solution of…

A: Assuming the monoprotic acid is HA. Hence the ionization reaction of HA can be written as HA…

Q: An unknown weak acid with a concentration of 0.190 M has a pH of 5.600. What is the Ka of the weak…

A: Assuming the unknown weak acid is HA Hence the dissociation reaction of acid is  HA ------> H+ +…

Q: An unknown weak acid with a concentration of 0.400 M has a pH of 5.600. What is the Ka of the weak…

A: If HA is the weak acid, then the reaction taking place is, HA+H2O→A-+H3O+ Concentration of H3O+ can…

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

A:

Q: An unknown weak acid with a concentration of 0.510 M has a pH of 5.600. What is the Ka of the weak…

A:

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: An unknown weak acid with a concentration of 0.066 M has a pH of 1.80. What is the Ka of the weak…

A:

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…

A:

Q: An unknown weak acid with a concentration of 0.420 M has a pH of 5.600. What is the Ka of the weak…

A: Solution The acid equilibrium constant is that the constant of the dissociation reaction of AN acid…

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: An unknown weak acid with a concentration of 0.090 M has a pH of 1.80. What is the Ka of the weak…

A: The question is based on the concept of equilibrium. we have been given concentration and pH of the…

Q: An unknown weak acid with a concentration of 0.450 M has a pH of 5.600. What is the Ka of the weak…

A: Calculate the hydrogen ion concentration as follows: [H+] = 10^(-pH) = 10^(-5.6) Let HX be the weak…

Q: An unknown weak acid with a concentration of 0.088 M has a pH of 1.80. What is the Ka of the weak…

A: Since it is not given whether the weak acid is monoprotic or polyprotic. Hence I'm assuming the acid…

Q: A solution of benzoic acid (C6H5COOH) that is 0.20 M has a pH of 2.45. What is Ka for benzoic acid?

A: Benzoic acid is a weak acid. With the help of pH firstly calculate hydronium ion concentration.

Q: Kb

A:

Q: An unknown weak acid with a concentration of 0.058 M has a pH of 1.80. What is the Ka of the weak…

A: Assuming the weak acid is monoprotic acid HA. Hence the ionisation reaction of acid can be written…

Q: An unknown weak acid with a concentration of 0.062 M has a pH of 1.80. What is the Ka of the weak…

A: weak acids like acetic partial dissociate into individual ions . PH= -log[H+]

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: What is the Ka of the acid in a solution that is 0.34M in the acid, and 0.247M in the conjugate base…

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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…

A:

Q: An unknown weak acid with a concentration of 0.220 M has a pH of 5.600. What is the Ka of the weak…

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.