the ?a of a monoprotic weak acid is 7.3×10−6,7.3×10−6, what is the pH of a 0.44 M0.44 M solution of this acid?

Q: If the ?b of a weak base is 3.6×10−6, what is the pH of a 0.35 M solution of this base?

A: In order to figure out any certain basic solution's pH, first evaluate the hydroxide ions levels…

Q: Calculate [OH-] and pHfor each of the following solutions: (a) 0.105 M NaF,(b) 0.035 M Na2S, (c) a…

A: The chemical reaction is as follows:

Q: what is the ph of a 0.33 M solution of licn  ka hcn =4.9x10^-10

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Q: (a) Acid rain is no threat to lakes in areas where the rock is limestone (calcium carbonate), which…

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Q: The hydronium ion concentration in an aqueous solution at 25°C is 2.8x1o-2 M. The hydroxide ion…

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Q: A 1.25 M solution of the weak acid HA is 9.2% dissociated. What is the pH of the solution?

A: The pH of a solution expresses the basicity and acidity of the given solution, which is calculated…

Q: An aqueous solution has a hydrogen ion concentration of 1×10-13 M   (10 -13 M). (1) What is the…

A: Given: H3O+=1×10-13 M Formula used:pH+pOH=14

Q: What is the PH of each of the followig?   (a)  0.0010 M HCl (b)  0.76 M KOH (c)  2.8x10^-4 M…

A: The pH of a given solution can be termed as a measure of its basicity or acidity. It is a measure of…

Q: If the ?b of a weak base is 5.8×10−6, what is the pH of a 0.33 M solution of this base?

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Q: what is the pH?

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Q: If the ?b of a weak base is 6.2×10−6, what is the pH of a 0.10 M solution of this base?

A: From given  Kb of weak base is 6.2 ×10-6  By using base dissociation constant formula and from the…

Q: If the  ?a  of a monoprotic weak acid is  2.9×10−6,  what is the  pH  of a  0.29 M  solution of this…

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Q: 0.117 M solution of a weak base has a pH of 11.77. What is the value of K, for the weak base? Kb =

A: In this question, we will determine the Kb value of weak base.  Given that,  Concentration of weak…

Q: The pH of a 0.70 mol/L weak base solution is 10.22. What is the Kb of the base?

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Q: 20.0 mL of 0.10 M solution of HNO2 is reacted with 10.0 mL of 0.15 M KOH solution. Which of the…

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Q: Be sure to answer all parts. Calculate the pH of each of the following solutions. (a) 2.7 ×10−4M…

A: (a)  2.7×10-4 M  Ba(OH)2    Ba(OH)2 is a strong electrolyte whose ionization is given as:    Ba(OH)2…

Q: If a buffer solution is 0.200M in a weak acid (?a=9.0×10−5)and 0.550M in its conjugate base, what is…

A: Ka = 9.0 x 10-5  pKa = -log Ka = - log ( 9.0 x 10-5)  pKa = 4.046 [Acid] = 0.200 M  [Conjugate base]…

Q: A certain weak base has a ?bKb of 8.80×10−7.8.80×10−7. What concentration of this base will produce…

A: 0.057 M

Q: 0.1 M NaCl 0.1M C,H;NH,Br 0.1M C,H;NH;Ci 0.1M NaF Use the following data to answer the question: K,…

A: We. Can observe with the mixture of salt  NaF is mixture of NaOH and HF which is strong base and…

Q: NH3 is a weak base (?b=1.8×10−5) and so the salt NH4Cl acts as a weak acid. What is the pH of a…

A: Calculating for pH given the value Kb :- In solving this problem we need the right dissociation…

Q: The pH of 0.0720M solution of a weak acid is 2.670. What is the Ka of the acid

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Q: What is the pH of a 3 M HNO2 solution if the Ka of HNO2 is 4x10^-4

A: pH helps in determining the level of acidity or basicity of any chemical. Mathematically, pH is…

Q: A sample of 7.80 L of NH3 (ammonia) gas at 22 ∘C and 735 torr is bubbled into a 0.400 L solution of…

A: To calculate the pH of the resulting solution after adding ammonia () gas to hydrochloric acid (HCl)…

Q: What is the pH of a solution made by mixing 2.222 grams of ammonium chloride solution, NH4Cl, with…

A: Given :Mass of Ammonium chloride = 2.222 gMolar mass = 53.49 gKb = 1.8x10-5

Q: Which pair of chemical species is NOT a conjugate acid-base pair? A) H,CO3 and CO, В) ОН аnd H,О C)…

A: Hi, Since you have posted multiple questions, we will solve first only. If you want the answer for…

Q: 4• 16.84 Predict whether aqueous solutions of the following sub- stances are acidic, basic, or…

A: SOLUTION: Step 1: (a) AlCl3 acts as Lewis acid. Aluminium has 6 electrons in its valence shell, and…

Q: An aqueous solution has a hydrogen ion concentration of 1×1013 M (10-13 M). (1) What is the…

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Q: 7. Calculate [H3O+] and [OH-] for each solution of either a strong acid or a strong base. Calculate…

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

Q: Whats pH of a solution that is 0.010 M in HClO Ka = 3.5 × 10–8 and 0.010 M in HCl?

A: Since HCl is a strong acid, it is completely dissociated into H+(aq) and Cl-(aq).  Hence [H+(aq)] =…

Q: Calculate the pH of a solution that is (a) 1.50 x 10^-1 M NH4Cl (b) 1.50 x 10^-2 M NH4Cl (c) 1.50 x…

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Q: The ?a of a weak monoprotic acid is 2.32×10−5. What is the pH of a 0.0787 M solution of this acid?

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Q: The ?a of a weak monoprotic acid is 1.52×10−5. What is the pH of a 0.0852 M solution of this acid?…

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Q: solution is 3.75. what is the percent ionization for

A: Concentration of Acid(C) = 0.012 M pH = 3.75 pH = -log([H+)] = 3.75 [H+] = 10-3.75 = 0.000178 M

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.