An unknown weak base with a concentration of 0.0910 M has a pH of 11.90. What is the Kb of this base?

Q: Handwritten work for the pH of a solution that 0.82 M

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Q: Determine the Kb of a weak base if a 0.31 M solution of the base has a pH of 11.79 at 25°C.

A: The pOH is calculated from pH as shown below.

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: An unknown weak base with a concentration of 0.0910 M has a pH of 10.60. What is the Kb of this…

A: Kb is the dissociation constant of a weak base. Higher is its value, stronger is the base.

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 0.135 M solution of a weak base has a pH of 11.23. Determine Kb for the base.

A: Weak base are those which do not dissociate completely in water. For base concentration depend on…

Q: Which of the following solutions would have the highest pH? Assume that they are all 0.10 M in acid…

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

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: An unknown weak base with a concentration of 0.0910 M has a pH of 10.70. What is the Kb of this…

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Q: MOH base solution is 0.02 M with an ionization degree of 0.02. The pH of the base solution is

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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: Determine the Kb of a weak base if a 0.19-M aqueous solution of the base at 25⁰C has a pH of 10.88

A: The question is based on the concept of equilibrium. we have been given a weak base  whose PH and…

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.63. What is the Kb of this base?

A: The weak base dissociates feebly in an aqueous solution to furnish the hydroxide ions. For example,…

Q: Assume that a generic weak base has an 0.83 M concentration. It also has a pH value of 10.5. Solve…

A: Given, Concentration of a weak base = (C) = 0.83 M pH of the solution = 10.5 Ka of the given base =…

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: An unknown weak base with a concentration of 0.170 M has a pH of 10.26. What is the Kb of this base?

A: We have pH as 10.26, concentration as 0.17 M, we have to calculate the Kb of the base .

Q: Find the pH if the concentration of OH- is 0.52 M?

A: [OH-] = 0.52 M

Q: A 0.135 M solution of a weak base has a pH of 11.22.  a) Determine Kb for the base.

A: Concentration of OH- is determined as follows,

Q: What is the pH of 2.9x10 M

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Q: Please help me, double check your answers as previous tutors got it wrong.

A: pH is the potential of the hydrogen or the power of the hydrogen. It basically explains how acidic…

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…

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Q: An unknown weak base with a concentration of 0.0910 M has a pH of 10.90. What is the Kb of this…

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Q: A certain weak base has a Kb of 7.80 × 10-7. What concentration of this base will produce a pH of…

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Q: An unknown weak base with a concentration of 0.0910 M has a pH of 10.80. What is the Kb of this…

A: Welcome to bartleby!  Introduction :  We have to calculate Kb of the base .

Q: A certain weak base has a Kb of 8.40×10−7. What concentration of this base will produce a pH of…

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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…

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Q: If the Ka for a weak acid, HA, is 4.5 × 10−6, what is the Kb for its conjugate base, A−?

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Q: If the ph of 0.10 M HA (weak acid) is 4.10, calculate Ka for this weak acid.

A: From given pH value the hydronium ion concentration is determined first.

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

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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…

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Q: Find the pH of 0.10 M ammonia.

A: pH: pH of any solution is defined as it is the power of hydrogen atoms into the solution. Here , we…

Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.42. What is the Kb of this base?

A: Given is Concentration (c) = 0.170 M pH = 9.42 Kb = 0.170

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: 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: A certain weak base has a ?b of 8.40×10−7. What concentration of this base will produce a pH of…

A: Weak base dissociated less in solution

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: Kb

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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: A certain weak base has a Kb of 7.20×10-7. What concentration of this base will produce a pH of…

A: Since it is not given whether the base is monoprotic or not. Hence I'm assuming it to be monoprotic…

Q: A certain weak base has a K, of 8.20 x 107. What concentration of this basc will produce a pH of…

A: Given, pH= 10.29 Kb = 8.20*10-7

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…

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Q: Pure water have a pH of 7 at 25°C. Prove this statement.

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Q: A certain weak base has a Kb of 8.60×10−7M. What concentration of this base will produce a pH of…

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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: An unknown weak base with a concentration of 0.170 M has a pH of 9.37. What is the Kb of this base?

A: The pH of any compound can be calculated on the basis of the concentration of hydronium ions present…

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…

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Q: An unknown weak base with a concentration of 0.170 M has a pH of 9.53. What is the Kb of this base?

A: The K b represents an equilibrium constant.  If the value of K b is small, then the base will be…

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.