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

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: The K, of a certain base is 4.4x107. What is the pH of a 0.30-M solution of this base?

A: Hello. Since your question has multiple questions, we will solve the first question for you. If you…

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: A 0.027 M solution of NaY is made and the pH measured at equilibrium. If Y is a weak base and if the…

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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: 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: Consider HA (a weak acid) and HB (a weak base). 11) A 0.10 M solution of the weak base D has a pH…

A: Given: pH = 11.45 concentration of weak base = 0.10 M

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: 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: An unknown weak base with a concentration of 0.170 M has a pH of 9.54. What is the Kb of this base?

A: pH = -log[H3O+] Where [H3O+] is the concentration of hydronium ion…

Q: Find the pH of a solution that is 9.0x10^-2 M in H2CO3

A: To calculate the pH we have to know the concentration of [H3O+]. As we know  pH= -log [H3O+] in the…

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

A: Given: Concentration of base = 0.0910 M And pH of solution = 11.90  Since pOH = 14 - pH => pOH =…

Q: If the Kb of a weak base is 6.8*10^-6 what is the pH of 0.18M solution of this base

A: We have to calculate the pH of weak base.

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: 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 10.80. 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…

A:

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

A:

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: 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: An unknown weak base with a concentration of 0.170 M has a pH of 10.04. What is the Kb of this base

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Q: A 0.100 M weak base has a pH of 8.77. What is the Kb value of this base?

A: Given:Let the acid be : MOHpH=8.77also, concentration of weak base= 0.100Mi.e [MOH] =0.100M

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…

A:

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

A:

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: A 0.25-M weak base solution has a pH of 11.50. Calculate its Kb.

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Q: An unknown weak base with a concentration of 0.0910 M has a pH of 12.30. What is the Kb of this…

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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: 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 0.450 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: 11. An unknown weak base with a concentration of 0.0910 M has a pH of 12.40. What is the Kb of this…

A: We have to calculate the Kb of the base.

Q: Kb

A:

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

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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: 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: A certain weak base has a K, of 8.80 x 10-7M. What concentration of this base will produce a pH of…

A: Given data: The Kb value of weak base = 8.80×10-7. The pH of the weak base = 10.28. To calculate:…

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.