A certain weak base has a Kb of 7.80 × 10-7. What concentration of this base will produce a pH of 10.38?

Q: What is the pH of an aqueous solution that is 0.1M NH4Cl? The Kb value for NH3 is 1.8 x 10-5

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Q: Which of the following 1.0 M solutions would have the highest pH? Weak Acid Ka HCN 4.9 x 10-10 HNO2…

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Q: What is the pH of a neutral solution at 10°C, where Ku equals 3.6 × 10-18? pH =

A: Given : Kw at 10 oC = 3.6 X 10-15  Since in neutral solution, the equilibrium reaction taking place…

Q: Calculate the pH of a solution that has [ OH-] = 5.2 x 10-7 M pH=  _?_

A: Given, Concentration of OH-, [OH-] = 5.2*10-7M. The pOH of the solution can be calculated as…

Q: Calculate pH of the following solutions: a) 0.25 M HNO3 in 0.065 M CH3COOH (K,=1.75x10). b) 0.33 M…

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

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Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

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Q: Calculate the pH of each of the following solutions at 25°C. a 0.125 M HONH2 (K = 1.1 x 10-8) %3D pH…

A: “Since you have posted a question with multiple sub-parts, we will solve first three sub-parts for…

Q: What is the pH of a solution of 0.79 M acid and 0.55 M of its conjugate base if the ionization…

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Q: Find the pH of the following solution and state whether the solution is acidic, basic or neutral.…

A: Given Hydrogen ion concentration is [H+]=4.5×10-10M As we know, pH=-log[H+] pH=-log[4.5×10-10]use…

Q: If 0.10 M aqueous solutions are prepared of each of the following acids, which produces the solution…

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Q: If the Kb of a weak base is 5.7 × 10-6, what is the pH of a 0.16 M solution of this base?

A: From the relation, pOH is calculated as,

Q: Determine the pH of a 0.16M NH3 where kb = 2.4 x 10-6  follow the format: a) [OH-] in 0.16M NH3…

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Q: I'm not sure how to do this question

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Q: A solution that has a hydrogen ion concentration equal to 3.52 x 10-3 has a pH = _____________?

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

A: pH is the negative logarithm of the hydrogen ion concentration. It is a measure of acidity or…

Q: HCl is a strong acid.  What is the pH of a solution of concentration 1 x 10-3M?

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

A: The solutions given are of KCl, CH3NH3Cl, NaCN and C2H5NH3Br.

Q: Which would have a higher pH, a solution whose pOH is 5.00 or a solution whose hydrogen ion…

A: pH of solution is calculated based on the hydrogen ion concentration. pH = -log[H+] pH = 14 - pOH

Q: If you mix 100. mL of 0.11 M HCl with 50.0 mL of 0.22 M NH3, what is the pH of the resulting…

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Q: Determine the pH of a solution of a weak acid (HA) that is 0.17 M. The Ka of the weak acid is 7.5 x…

A: Given a concentration of weak acid (HA) =0.17M Acid dissociation constant value =        7.5 x 10-5…

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

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

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Q: Calculate the pH of a weak acid (HA) which concentration is 0.236 M. Ka = 0.00000175

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Q: Calculate the pH of 0.30 M methylamine, CH3NH2, which has a Kb of 4.4 x 10-4.

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Q: weak Mandalorious acid (HMaO3): 4.5 x10-1 M, Ka = 6.7 x 10-5  Determine the pH of the solution

A: The acid dissociation constant for the HMaO3 is = 6.7×10-5 The concentration of HMaO3 solution is =…

Q: Based on the Kb determined in the previous part, what is the pH of the initial 1.0 M base solution?…

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Q: Ammonia, a weak base with a Kb value of 1.8 x 10^-5 (a) What is the pH of a 0.155 mol L^-1 ammonia…

A: Given data is as follows:      The Kb value of ammonia = 1.8×10-5 The concentration of ammonia…

Q: What is the pH of a solution that has a [OH] = 3.3 x 10-³ M

A: pH is the negative logarithm of the concentration of H+. pOH is the negative logarithm of the…

Q: Calculate the pH of the following solutions: (a) 0.0500 M NaOH (b) 0.0500 M sodium acetate (c)…

A: A)   0.05 M  NaOH    As NaOH is a strong base, it will dissociate completey.   NaOH (aq) → Na+ (aq)…

Q: What is the pH of 0.80 M methylamine (CH3NH2). Kb = 4.4x10-4.

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

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Q: Calculate the pH of a solution with an H+1 concentration of 2.90 x10-12and identify the solution as…

A: Given: Concentration of H+ ions =  2.90×10-12

Q: Calculate the pH of a 1.7 M Ca(OH)2 aqueous solution. a.13.8 b.14.5 c.13.5 d.14.2

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Q: What is the pH of a solution with 10.2mL 0.10M NH3 and 0.15mL 1.0M NaOH ? Kb = 1.8x10^-5

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Q: Calculate the [OH-], [H3O+], pOH and pH of a 0.075 M NH3 Ka NH4+ = 5.70 x 10-10

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Q: For questions 7-9 state which species (chemical) is the acid, which is the base, and which are the…

A: Bronsted Lowry acid-base theory. Acid is the chemical species that donates protons in the solution…

Q: Calculate the pH of each of the following solutions at 25°C. a. 0.125 M HONH2 (K = 1.1 x 10-8) pH =…

A: Since you have posted multiple sub-parts questions, as per our company guidelines we are supposed to…

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

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Q: The Kb for aniline (C6H5NH2) is 4.3 x 10-10. What is the pH of a 0.15 M solution of aniline?

A: From the ICE table, we have

Q: The pH of a 0.10 M solution of a weak base is 9.67. What is the Kb of the base?

A: Assuming the weak base is monoprotic base Hence the dissociation of base will have below reaction…

Q: Aniline, C6H5NH2, is a weak base with Kb = 4.2 x 10–10.  What will be the pH of a 0.188 M aniline…

A: Given, kb = 4.2 x 10-10 molarity = 0.188 M  PH = ?

Q: What is the pH of a solution that has [OH-] = 6.5 x 10-3 M?

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Q: The acid ionization constant, Ka, of a certain weak acid HA equals 1.4 x 10-11. What does Kb for the…

A: Since for any acid and its conjugate base, the Ka and Kb respectively are related to each other as…

Q: You have a 7.4x10-4M Sr(OH)2 solution. What is the pH of this solution?

A: First of all we will calculate pOH then pH

Q: Step by step please clearly

A: Given reaction,

Q: Consider the following data on some weak acids and weak bases: name acetic acid hydrocyanic acid 0.1…

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Q: The pH of a solution containing a hydrogen ion concentration of 1 x 10-5 is 5 and its pOH is 9 show…

A: pH of a solution measures acidity or basicity of solution. pH is less than 7 indicate solution is…

Q: The formula for the pH of a solution of hydronium ions is given by the logarithmic equation pH = -…

A: We will calculate the pH by using its formula.

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.