A certain weak base has a Kb of 8.40 × 10-7. What concentration of this base will produce a pH of 10.39? anwser in M

Q: The pH of a basic solution is 12.17. What is [H]? M 3 4 6. C 7 8 +/- x 100

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Q: e pH of a solution  with [H+]  = 1.5x 10-1

A: The pH of the solution is a measure that how much the given solution is acidic and basic in nature.…

Q: The hydroxide ion concentration of a solution is 6.7 X 10-8. What is the pH level of the solution?…

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Q: A certain weak base has a K, of 7.20 x 10-7, What concentration of this base will produce a pH of…

A: Base dissociation constant Kb is utilized to determine the basic nature of a solution. It refers to…

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

A: Assuming the weak base is monoprotic which can be written as BOH. Hence the dissociation reaction of…

Q: A certain weak base has a K, of 8.50 × 10-7. What concentration of this base will produce a pH of…

A: Suppose the base is "B". Equation for the dissociation of the base is: B(aq) + H2O(l)  <----->…

Q: Consider an aqueous solution that is 0.050 M in H2Se (Ka = 1.29 x 104) and 0.075 M in NaHSe. Out of…

A: The acid ionization constant for acid is 1.29×10 -4.

Q: What is the pH of 0.180M NH4Cl. Ka NH4+: 5.80x10^-10

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Q: What is the pH of a solution that contains 3.9 x 10-5 [H30+]?

A: Given :-  [H3O+] = 3.9 × 10-5 M  To calculate :-  pH of solution

Q: Calculate the (a) pH (b) pOH (C) percent ionization of 0.100M ammonia. NH3 Kb = 1.8x10¬s

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Q: The pH of an aqueous solution at 25°C was found to be 9.80. The pOH of this solution is The…

A: 1) Given that : pH of the solution = 9.80 pOH of the solution is, pH + pOH = 14 pOH = 14 - pH = 14 -…

Q: What is the pH of a solution with a hydroxide ion (OH-) concentration of 10-10M?

A: pH is related to pOH by the following expression: pH + pOH = 14  ⋯⋯⋯⋯(1) Also pOH is related to the…

Q: A certain weak base has a K, of 8.90 × 10-7. What concentration of this base will produce a pH of…

A: Concentration of base required can be calculated using equation: [OH-] = √(Kb × [Base])

Q: is the pH of a solution when the concentration of hydronium and hydroxide ions are equal. O greater…

A: we are to discuss what is the pH when concentration of hydronium ion and hydroxide ion are same.

Q: . What is [OH⁻]?

A: The pH of a solution is determined as the negative logarithm of the concentration of hydrogen ions…

Q: Calculate the pH of the following acid or base: 1. 3.6 x 10-7 M HNO3 2. 2.0 x 10-4 M NaOH

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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: 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: Determine the pH of each of the following solutions: (a) 0.723 M CaCl2 (b) 1.55 M C6H5N (c) 0.00443…

A: Since you have posted a question with multiple subparts, we are entitled to answer first three…

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: I. Calculate pH from the following hydrogen ion concentration (M). Identify each as an acidic pH or…

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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: A certain weak base has a ?b of 7.50×10^-7. What concentration of this base will produce a pH of…

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Q: what was the pH of the AOm(OH)m unknown aqueous solution? The hydrogen ion concentration of the…

A: Given Hydogen ion concentration of unkown solution is [H+] =1×10-5m We have to calculate the ph of…

Q: 7.30×10−7. What concentration of this base will produce a pH of 10.14?

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Q: The pH of an aqueous solution at 25°C was found to be 3.40. ail The pOH of this solution is The…

A: The pH of the solution is equal to the negative logarithm of hydronium ion while pOH is equal to the…

Q: What is pH of a solutionwith a H+ concentration of 10^-4M

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Q: A solution which has [OH-] = 5.6 × 10-12 M is Group of answer choices acidic. basic. neutral.

A: since the concentration of OH- ion i.e [OH-] = 5.6 × 10-12 M Hence pH = 14 + log[OH-]  => pH = 14…

Q: The pH of an aqueous solution at 25°C was found to be 5.40. The pOH of this solution is M. The…

A: Note : Since you have posted multiple questions, we are entitled to answer the first only. Please…

Q: Consider the folowing data on some weak acids and weak bases: acid base K name formula formula name…

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Q: The [H+] in a particular lake is 10-8.5. Use the formula pH = -log [H+] to determine the pH of the…

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Q: A certain base has a Kb of 7.8 × 10-6 . What concentration of the base will produce a pH of 11.32?

A: Fristly we calculate the concentration of OH- from the pH : pOH = 14-pH  = 14-11.32 =2.68…

Q: All of the following expressions are equivalent to pH   a)  log [1/H+(aq)]   b) 14-pOH   c)…

A: No, all the given expressions are not equivalent to pH.

Q: What is the pH of a solution that is 0.150 M in acetic acid (aka=1.8 x 10^-5)? What is the percent…

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Q: The pH of a solution with [H3O+] = 1x10¯4 M is

A: pH = -log [H3O+]

Q: ertain weak base has a K, of 8.50 × 10-7. What concentration of this base will produce a pH of…

A: Weak base dissociated less in solution

Q: A certain weak base has a ?b of 7.90×10−7. What concentration of this base will produce a pH of…

A: As per the given information  certain weak base has a kb is 7.90×10-7. pH=10.03 The chemical…

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: Determine the pH of an HNO2 solution of each concentration. In which cases can you not make the…

A: To solve this table will be created with initial and equilibrium concentration. The reactant is…

Q: True or False

A: This statement is true you are creating a buffer, which is an equilibrium mixture of a weak acid…

Q: Calculate the pH of a 0.400M solution of quinoline, C₉H₇N.

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Q: I. Calculate pH from the following hydrogen ion concentration (M). Identify each as an acidic pH or…

A: Note: As per our guidelines, we are supposed to answer only three subparts. Please repost the…

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 7.20 × 10-7. What concentration of this base will produce a pH of…

A: Given  Kb = 7.20 x 10-7 pH = 10.14  we know  pH + pOH = 14  pOH = 14 - 10.14 = 3.86 and   [OH-] =…

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: Calculate the pH of the following solutions: a) 1.9x10 10 M LIOH b) 6.6x10 MHCIO4 c) 0.35x10 2 M KOH…

A: Interpretation- To determine the pH of given solutions - 1.9 ×10-10 M LiOH  6.6×10-5 M HCIO4…

Q: certain weak base has a  ?b  of  7.80×10−7.  What concentration of this base will produce a pH of…

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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.