Methylamine, CH3NH2, has a Kb of 4.4 x 10-4.  What is the pH of a 0.45 M solution of methylamine? Your answer should be to two places past the decimal.

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: Calculate the pH of  a 0.84 M HONH2 solution. Give your answer to three sig figs.  Kb(HONH2) = 1.0 x…

A: Given: The concentration of  HONH2 solution = 0.84 M  Kb(HONH2) = 1.0 x 10‒5 To Calculate: pH of the…

Q: Calculate the pH of a 1.88 M NH3 (Kb = 1.8 x 10^–5) solution

A: The pH is a scale that is widely used to measure the acidity or basicity of a solution. The pH is…

Q: If a sample of a certain solution is determined to have a [H30+] concentration of 7.74×10-3…

A: We know that, pH is the negative logarithm of hydronium ion concentration. i.e.,…

Q: What is the pH of a 0.65 M solution of pyridine, C5H5N?

A: Given,  The concentration of C5H5N is 0.65M The kb value of C5H5N is 1.7×10-9 To solve: pH of 0.65M…

Q: The weak acid, HA, has a Ka of 1.60 x 10-10. What is the Kb of its conjugate base, A™?

A: Given :-  Ka for weak acid (HA) = 1.60 × 10-10  To determine :  Kb of its conjugate base (A-)

Q: 11. The ionization constant, Kw, of water at 60 °C is 1.00 x 10-13. What is the pH of pure water at…

A: Given Kw = 1.00 x 10-13

Q: What is the pH of a 3.1 M potassium hydroxide, KOH, solution at 25oC  , knowing that Kw = 1.0 x…

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Q: Calculate the pH of a 0.10 M solution of hypochiorous acid, HOCl. Ka of HOCI is 3.5 x 10^-8 at 25…

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Q: Calculate the pH of a 0.081M NaCN solution at 25 degrees Celsius. Ka (HCN) = 4.9 x 10^(-10). You…

A: Given, Concentration of NaCN solution = 0.081 M Ka of HCN = 4.9 × 10-10 pH of the solution = ? Note:…

Q: Given a diprotic acid, H₂A, with two ionization constants of K₁ = 4.5 x 104 and K = 2.2 x 10-12,…

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Q: The acid dissociation K of propionic acid (C₂H₂CO₂H) is 1.3 × 105. Calculate the pH of a 2.2 x 10 M…

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Q: Aniline C,H5NH2 (K, = 3.8 x10-10) is a weak base. Calculate the pH and pOH of a 50.0 mL solution of…

A: Hydrolysis of weak base : Hydrolysis means dissociation in presence of water. When a weak base like…

Q: The pH of dissolving 1.48 g of propanoic acid (CH3CH2COOH, Ka 1.3X105) in 200 mL H20 is 4.82 O 3.71…

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Q: An aqueous solution has hydronium concentration [H3O+] = 9.8 x 10-5 mol L-1. What is the pH of the…

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Q: What is the pH of a peach with a [OH¯]=3.2x10-11 М ОН"?

A: In the Question, we want to determine the pH of the Solution.  You can see details Solution below.

Q: Calculate the pH of a 5.6 x 10 M -9. aqueous solution of perchloric acid (HCIO4). Round your answer…

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Q: A newspaper reported that the level of acidity in a sample taken from an extensively studied…

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Q: The hydroxide ion concentration, (OH'), of an aqueous solution of 0.364 M isoquinoline (a weak base…

A: The dissociation of weak base isoquinoline is, C9H7N  + H2O ↔C9H7NH+ + OH- By definition the value…

Q: The acid dissociation K, of acetic acid (HCH,CO,) is 1.8 x 10. Calculate the pH of a 2.1 x 10 M…

A: Recall the following expression to calculate pH of weak acid              pH=12pKa-12logCGiven…

Q: Abbreviating malonic acid, CH2(CO2H)2, as H2M, find the pH and concentrations of H2M, HM, and M2…

A: a.

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4. What is the pH of a 0.450 M  solution of methylamine?

A: Methylamine, CH3NH2 is a weak base which undergoes partial dissociation in aqueous medium. Let the…

Q: Can you show me an example of how to calculate an answer similar with a pH of 9.5?

A: We know that when pH is in between 0-7 then the solution is acidic and when it is in between 7-14…

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

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Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 x 10. Calculate the pH of a 4.8M…

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Q: What is the pH of a 0.25 M solution of sodium propionate, NaC3H5O2, at 25°C? (For propionic acid,…

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Q: Write the CAPITAL LETTER of the best answer on the space provided. For numbers 1 to 3, determine if…

A: we know, Kw=[H+][OH-] AT 298K, [H+][OH-] = 10-14 pH+pOH=14

Q: Calculate [OH–] , [H+] , and the pH of 0.20 M solutions of each of the following  amines. a.…

A: Aniline and pyridine both are weak bases. From the equilibrium table we have to determine its…

Q: What is the pH of a 5.50x10-2 mol L-' ammonia solution? Express your answer numerically to two…

A: Weak base degree of dissociation (α)  can be calculated by the given below formula α  = KbCwhere…

Q: Aniline, C6H5NH2, is a weak base with K, = 3.8 x 10-10. What is the pH of 0.750 M anilinium chloride…

A: Anilinium chloride is a salt made from strong acid HCl and weak base aniline.  So, solution of…

Q: the concentration of H3O+ of seawater is 3.16 x 10-9. what is the pH of seawater?

A: Ph depends on concentration of H+ ions...

Q: The acid dissociation constant K, of carbonic acid (H,CO3) is 4.5 x 10. Calculate the pH of a 3.4M…

A: All details  explained  in Handwritten solution

Q: A solution is prepared at 25°C that is initially 0.50M in methylamine CH3NH2, a weak base with K,=…

A: Calculate the pH for given solution using formula which contains both concentration of acid and base…

Q: What is the pH of a 0.21 M solution of methylamine

A: Given :-  Initial concentration of CH3NH2 solution = 0.21M  Kb = 4.4 × 10-4  To calculate :-  pH of…

Q: Ascorbic acid (vitamin C, C6H8O6) is a diprotic acid (Ka1 = 8.0×10–5 and Ka2 = 1.6×10–12). What is…

A: Solution -

Q: Trimethylamine, (CH3)3NH2, is a gas with a fishy, ammonialike odor. A 0.25 M aqueous solution of…

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

Q: Methylamine, CH3NH2, has a Kb = 4.40 x 10-4.  What is the pH of a 0.290 M  solution of methylamine?

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Q: What is the pH of a 3.0 x 10 M solution of CoHsNH2 (Kb= 4.3 x 1010? What is the percent error in…

A: As PhNH2 is an weak base,it can be calculated using a formula.

Q: The acid dissociation constant K of boric acid (HBO3) is 5.8 × 10¯¹0. Calculate the pH of a 2.5 M…

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Q: The base protonation constant K, of azetidine (C,H,NH) is 1.5 x 10 °. Calculate the pH of a 0.63 M…

A: Given :-  Concentration of azetidine = 0.63 M  Kb for azetidine = 1.5 × 10-8  To be calculated :-…

Q: By what factor does 3H+4 change for a pH change of 0.50 units?

A: The pH of a solution is related to the concentration of H+ as follows: pH=-log [H+][H+]=10-pH

Q: The base protonation constant K, of lidocaine (C4H2 NONH) is 1.15 x 10 . Calculate the pH of a 1.0 M…

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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: What is the pH for the following aqueous solutions?                  a.   0250 M Ammonia (Kb = 1.8…

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Q: The acid dissociation K, of benzoic acid (C6H5CO,H) is 6.3 × 10 –³. Calculate the pH of a 1.5 ×…

A: Since benzoic acid is monoprotic acid. hence we can write C6H5CO2H as HA  where A = C6H5CO2 group…

Q: What is the pH of a neutral solution at a temperature where K = 8.0 x 10-14? Express your answer…

A: Given that, Kw= 8.0×10-14 pH = ?

Q: The acid dissociation constant K, of carbonic acid (H,CO,) is 4.5 x 10 '. а Calculate the pH of a…

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Q: The base protonation constant K, of ammonia (NH,) is 1.8 x 10. Calculate the pH of a 1.2 M solution…

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Q: If the pH of a 1.00-in. rainfall over 1800 miles^2 is 3.90, how many kilograms of sulfuric acid,…

A: Given: pH = 3.90Area= 1800 miles2Ka2 = 0.012.

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.