A 0.055 M solution of HX is 6.7% ionized. Calculate Ka of this acid.

Q: of each of these salts. Why?/rationale (based upon ions present) NANO3 Acidic Basic Neutral NH4C1…

A: As per our guidelines we can only solve first question. Please resubmit the other questions as next…

Q: What will be the Ka of an acid solution that is 0.012 % ionized when it is 0.20 M?

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Q: A 0.051 M solution of a weak acid has a pH of 2.09. Calculate the acid ionization constant (Ka) of…

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Q: the solution acidic or basic? How did you know?

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Q: OH H OH CF3 1 2 3 4

A: ->Which specie give H^+ easily that is most acidic . ->The conjugate base is stablized then it…

Q: Calculate the [H-] and identify if its acidic, basic or neutral [OH-] = 1.8 x 10^-2 M

A: Answer:- This question is answered by using the simple concept of calculation of hydrogen ion…

Q: In a solution with a pH value of 7.0, hypochlorous acid a0 and Find the a1 values. (ka for HOCI=…

A: ·Solution of Hypochlorous acid HClO·pH of the solution = 7.0·Ka of HClO = 3×10-8We need to calculate…

Q: Determine the pH of a 0.62 M NH4NO3 solution at 25°C.  The Kb for NH3 is 1.8 × 10-5. Express your…

A: NH4NO3 is a salt of strong acid and weak base.  Given Kb of ammonia is 1.8×10-5 and concentration of…

Q: Classify each of the following compounds as a strong acid, weak acid, strong base, or weak base, and…

A: Acids are the substance that produces H+ ion when dissolved in water. Bases are the substances that…

Q: Calculate Kh using the equations, whichever is applicable. (If the ion is conjugate acid of a weak…

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Q: Be sure to answer all parts. A 0.205-mol sample of HX is dissolved in enough H20 to form 605.0 mL of…

A: Given, pH = 3.00 0.205mol of 605mL HX

Q: Codeine (C18H21NO3) is a derivative of morphine that is used as an analgesic, narcotic, or…

A: Kb is the base dissociation constant which is a measure to know the extent of dissociation of base…

Q: A 0.100 M solution of a weak acid (HA) is 4.6% ionized. Calculate Ka.

A: Given, Molarity of Weak acid  = 0.100 M  Ionization = 4.6 %  Acid, dissociation constant Ka = ?

Q: ons that show NH3 as both a conjugate acid and a conjugate base. l. NH3 tHt >NHj 2 NH3→NHる+H b. Show…

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Q: A strong acid has a large or small Ka value?

A: Strong acid is a type of acid which has a high tendency to dissociate into ions in the aqueous…

Q: 30. A 0.530 M solution of a weak monoprotic acid has a percent ionization of  0.30%. Determine the…

A: Given, % ionisation = 0.30% Concentration = 0.530 M

Q: Calculate the percent ionization for each of the 3 acid solutions. What trend do you notice when…

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Q: Be sure to answer all parts. The pH of a 0.064 M weak monoprotic acid is 3.09. Calculate the Ka of…

A: Given,The pH of a 0.064 M weak monoprotic acid is 3.09

Q: A 0.035 M solution of a weak acid has a pH of 2.21. Calculate the acid ionization constant (Ka) of…

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Q: Select the weakest acid from amongst the set below. Assume the same concentration in aqueous…

A: The strength of an acid says , how much it is capable to ionize into its constituent ions. Strong…

Q: Calculate the [HA] of 0.0644M anilinium chloride solution.  Calculate the concentrations of the…

A: Structure of anilinium chloride: pKa value for anilinium ion = 4.6 Since pKa = -logKa Ka = 10-4.6 =…

Q: Predict whether an aqueous solution of the following salts will be acidic, basic or neutral. Justify…

A: For this , we would first write equation of salt in aqueous solution. Then we check the nature of…

Q: For each of the following ions, correctly identify if it is acidic, basic, or neutral. (HINT:…

A: A Danish chemist, Johannes Bronsted and an English chemist, Thomas Lowry proposed that acid is a…

Q: Font Paragraph Styles Complete the following table. [H,0*] [Or] Acidic pH pOH or Basic? a) 7.5 x…

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Q: Maleic acid (H2C4H2O4) is a diprotic acid with ?a1=1.20×10−3 and ?a2=5.37×10−7. Determine the pH of…

A: 1- First we will determine the H+ ion concentration :  Most H+ ion comes from first dissociation.…

Q: A solution containing a hydronium ion concentration of  3.28 X 10-9 has a hydroxide ion…

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Q: Determine rather each salt is acidic, basic, or neutral. (Hint: You will need the Ka table provided…

A: The salts are acidic, basic, or neutral should be determined

Q: Since the pH of 0.1 M acetic acid solution is measured as 2.88, the Ka value of acetic acid…

A: The degree of ionization has to be calculated, Given, The pH of the solution is 2.88. We know that…

Q: A 0.763 M solution of a weak acid (HA) is made.  The solution has a pH of 5.32. Calculate the Ka of…

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Q: The pH of a 0.464 M solution of phosphorous acid (H3PO3) is 1.11.  Using this information, calculate…

A: We have pH of H3PO3 as 1.11, also all H+ comes from the first dissociation of given acid. We have to…

Q: Calculate the pH of a 0.20 mol L solution of KCN. Express the pH numerically to two decimal places.…

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Q: 1. Indicate whether each solution is acidic, basic, or neutral: а. 2х 104 МОН- b. бх 10-10 Мн 2.…

A: The pH of the solution is related to H+ concentration as,                      pH = - log[H+] If the…

Q: triprotic

A: For triprotic acid, Ka1 > Ka2 > Ka3  More H+ ion comes from first dissociation and second…

Q: Determine [H30*] in a solution where [OH] = 4.97 x 10-4 M. Identify the solution as acidic, basic,…

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Q: Show by computation which acid is the weakest based on its % ionization. The lesser its %…

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Q: HX is a weak acid: Ka = 5.52 × 10–7. Calculate the pH of a solution in which [HX] = 0.0501 M and…

A: Here HX is a weak acid. Given data, Ka =5.52×10-7 [HX]=0.0501 M and [X1-]=0.00845 M

Q: 1- H2SO4 is a strong acid in its first ionization; but a weak acid in its second ionization with Ka…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: An acid (HA) has a % Ionization of 2.1%. A solution of this acid has a molarity of 0.500 M.…

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Q: A 0.035 M solution of a weak acid has a pH of 2.21. Calculate the acid ionization constant (Ka) of…

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Q: Calculate the pH of an 0.025 M solution of HF. HF is a weak acid Ka = 0.00071

A: The PH of weak acids can be calculated as follows

Q: Select the weakest acid from amongst the set below. Assume the same concentration in aqueous…

A: The acidic strength of a compound depends upon its ability to lose H+ ions. The acid…

Q: Complete the following table by calculating the missing entries. In each case indicate whether the…

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Q: The proton concentrations of three solutions at 25 °C are given. Classify the solutions as acidic,…

A: Given, the hydrogen ion concentration for the first solution is--- [H+]=1.0×10-8 M We know, PH = -…

Q: Find the pH of a 0.011 M solution of HF. (The value of Ka for HF is 3.5×10−4

A: Given, initial concentration of HF= 0.011 M          and, Ka= 3.5 x 10-4 We know that, pH is equal…

Q: Construct the expression for Ka for the weak acid, NH,*. NH, (aq) + H,O(1) =H,Oʻ(aq) + NH,(aq) 1…

A: Construct the expression for Ka for the weak acid NH4+ ----

Q: [H₂O] 2[OH-] [NH₂]² Construct the expression for Ka for the weak acid, NH4*. NH4(aq) + H₂O(1) H3O+…

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Q: 3. Identify the following condition as representing an acidic, basic, or neutral solution at 25°C,…

A: Solution: We have pH values from that and corresponding temperature we want to conclude given…

Q: If the pH of a 0.800 M solution of an acid is 3.45, calculate the % ionization of this acid and…

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Q: Write the chemical equation for the reaction of carbonic acid (H, CO,) with water and identify the…

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Q: First, indicate which substance is acting as the: Acid, Base, Conjugate Acid, Conjugate Base.…

A: The given reaction is, CH3O- + NH3  ⇌  CH3OH + NH2-

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.