Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate the ionization constant for the weak acid 10-2 O 10-6 10-5 O

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

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

Q: (b) What is the pH of 0.39 M methylammonium bromide, CH3NH3Br? (Kb of CH3NH2 = 4.4 10-4.)

A: Methylammonium bromide dissociates into quartnary ammonium ion (CH3NH3+) and bromide ions (Br-).…

Q: Calculate the hydronium ion concentration and the pH when 35.0 mL of 0.45MN*H_{3} is mixed with 35.0…

A:

Q: Determine the pH of a 1.0M solution of sodium acetate (NaC2H3O2). Ka = 1.8x10-5 for acetic acid.

A: Dear student,  As you have asked multiple question but according to guidelines we will solve first…

Q: For H3PO3, Ka1= 4.06x10^-2 and Ka2= 3.92x10^-7. Calculate the pH of 0.295 molar solution H3PO3

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Q: Halpinious acid, H2JHO3, is a weak diprotic acid with Ka1 = 2.40 x 105 and Ka2 = 4.79 × 10-11 at…

A: Given Ka2 <<<< Ka1 so, [H+] = Ka1.C [H+] = 2.40 × 10-5×0.500 = 3.46 × 10-3 M  pH = -log…

Q: solution made by adding soilid NaClO to water resulted in a baasic equilibrim with a pH of 10.50.…

A: Given data set: Volume = 2 L pH = 10.50 Ka(HClO) = 3.0*10-7 Calculating the value of pOH using the…

Q: 10 10 mL 0.05 M NAOH Hd

A: Henderson's equation: pH = pKa + log[salt]/[acid] at equivalent point: [salt] = [acid] pH = pKa

Q: What is the pH (to two decimal places) of a 50.0 mL 0.15 M HNO2 aqueous solution (at 25 °C) after…

A: Given that, 50.0 mL of 0.15 M HNO2 aqueous solution (at 25 °C) and 15.0 mL of 0.20 M NaOH are mixed.…

Q: What is the pH of a 80.0 mL solution which is 0.23 M in IO and 0.47 M in HIO? The Ka for HIO is 2.3…

A: When a weak acid(eg HIO) mixed with its conjugate base (ege IO-) they form a buffer solution. pH of…

Q: Complete the reaction H₂SO4 + 2 H₂O mplete ionization of HSO4-¹ What is the pH of a 0.001000 M H₂SO4…

A: ->H2SO4 is strong acid which can dissociate completely into ions H+ and SO42-. Molarity of H2SO4…

Q: A tablet containing 500 mg of aspirin was dissolved in enough water to make 100 mL of solution.…

A: Given, Mass of aspirin, C9H8O4 = 500 mg = 0.500 g     (1 mg = 0.001 g) Volume of solution = 100 mL =…

Q: 1. What is the pH of a neutral solution at 37°C, where Kw equals 2.5 x 10-14 (a) 7.00 (b) 6.80 (c)…

A: In this question, we want to determine pH of the neutral Solution.  How we can determine pH for this…

Q: What is the pH of a solution made from combining 2.49 mol (CH3)2NH2Cl and 5.18 mol (CH3)2NH in a…

A: Henderson-Hasselbalch equation explains the relationship between  of solution and  of acid. For a…

Q: volumes of 1.20 M sodium hydroxide. HgHis + H* + H2His" Kal = 3.98x103 H2His + H* + HHIS²- Ka2 =…

A: NOTE: please note according to our policy , we can only answer first three subparts of a question.…

Q: What is the pH (to two decimal places) of a 0.15 M NH3 and 0.15 M ammonium chloride aqueous solution…

A: The pH of buffer can be calculated by using Handerson equation . Ammonia and ammonium chloride forms…

Q: O. Calculate the Ka for a monoprotic acid, HX, if a 0.100000 M solution has a pH of 3.333. Write the…

A: The pH of a solution depends upon the concentration of H3O+ ions present in it. It is calculated by…

Q: When added to pure water in equal quantities, a Base with a Kb = 2.4 x 10-8 will cause greater pH…

A: when base B is added to water it abstract hydrogen ion from water to form BH+  the reaction  is…

Q: At 40.°C the value of Kw is 2.92 x 10-14 a. Calculate the H] and [OH ] in pure water at 40.°C. [H*]…

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Q: Calculate the pH and the equilibrium concentrations of HCO3- and CO32- in a 0.0257 M carbonic acid…

A:

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A:

Q: 1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous…

A: 1)  The ionization constant for the weak acid is = 3.1 x 10-13 The initial NaA concentration is =…

Q: The pH of 30.0 mL of 0.80 M Benzoic acid (Ka = 5.6 x 10-5) is _____________ (with 3 significant…

A: There are two types of types of acids/bases. Strong acids and strong bases are those acids and bases…

Q: Given a diprotic acid, H₂A, with two ionization constants of Kal = 4.0 x 104 and K₁2 = 4.7 x 10-¹1,…

A: 1. Given that, a diprotic acid H2A. The two ionization constants of H2A are Ka1 = 4.0×10-4, Ka2 =…

Q: 9. ОН 10. Calculate the pH of each of the following solutions at 25 °C: 12, 0.0010 M HNO3 13.0.1 M…

A: 12. Since HNO3 is a strong acid  hence it will dissociate completely => concentration of H+…

Q: Q1//A solution of 0.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A:

Q: . Morphine is a weak base for which Kb is 8 × 10-7 . Calculate the pH of a solution made by…

A: Let 'B' represents morphine. Initial concentration of B=moles/volume…

Q: Calculate the pH of 0.750 M pyridinium chloride, C5H5NHCl? Given Kb of C5H5N is 1.70×10-9.

A:

Q: 1.) HA is a weak acid. Its ionization constant, Ka, is 3.1 x 10-13. Calculate the pH of an aqueous…

A: Answer:- This question is answered by using the simple concept of calculation of weak acid and the…

Q: What is the pH of 100.0 mL of 0.10 M HNO;? nooulos M 005.0s ai nois 01 x 02.1 g CH'COOH What is the…

A: pH = -log [H+]

Q: Qi//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A:

Q: What is the pH of a 80.0 mL solution which is 0.27 M in IO and 0.49 M in HIO? The Ka for HIO is 2.3…

A:

Q: Calculate [H3O+] of the following polyprotic acid solution: 0.125 M H2CO3 (Ka = 4.3*10^-7, Ka2 =…

A: We have given that  Calculate [H3O+ ] of the following polyprotic acid solution: 0.125 M H2CO3 (Ka =…

Q: What is the pH of 0.025 M aqueous acetate ion? (Kb of CH3C

A: According to Ostwald’s Dilution Law and the pH (& pOH) scales, we can derive pOH =…

Q: The concentration of a solution is measured with a potentiometer called a pH meter. O H* O H20 OH…

A:

Q: What is the pH of the solution of 35.0 mL 0.20-M formic acid and 55.0 mL 0.10 M sodium formate in…

A: given data formic acid 35.0ml or 0.20 M sodium formate 55.0ml or 0.10M water 110ml find PH

Q: chemist named Ciara titrates X mL of a 0.7633 M hypochlorous acid (HA) solution with 0.3245 M…

A: The pH of a solution is guided by the concentration of the hydrogen ions. When a base is added, it…

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

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

Q: What is the pH of a solution that is 0.25 M CH3NH2 (methylamine) and 0.43 M CH3NH3Cl (methylammonium…

A: pH is the negative logarithm of hydronium ion. Henderson Hasselbalch equation for weak base: pKb…

Q: At 35°C water has Kw = 2.09 x 10^-14. Calculate the pH of pure water at 35°C.

A:

Q: For H2CO3, Ka1= 4.3 x 10^-7, Ka2= 4.7 x 10^-11. What is the pH of a 0.28 M solution of carbonic…

A: H2CO3 is a weak acid.  pH = 0.5pKa - 0.5logC ....(1) Here, pKa1 = -logKa1 = -log(4.3*10^-7) = 6.37…

Q: Calculate the concentration of each species present in a 0.025 M solution of phthalic acid,…

A: Pthalic acid is a weak acid and Ka is an equilibrium expression. The Ka is calculated by the…

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A: Use pH formula, used to calculate the pH of salt formed by weak acid and strong base to find the…

Q: Calculate the pH of the following mixture 500 ml 0.35 M CH3CH2NH2 + 500 ml 0.25 M HNO3

A: Given : The volume of CH3CH2NH2= 500 ml Molarity of CH3CH2NH2 =0.35 M The volume of HNO3=500 ml…

Q: Q1//A solution of o.1 M of BX salt with pH=9.5, the HX is weak acid and BOH a strong base. Calculate…

A: molarity of the solution = 0.1 M The pH of the solution  = 9.5

Q: What is the hydronium ion concentration [H3O+] of a 0.010 M acetic acid solution in water? (Ka for…

A:

Q: What is the pH of a solution that is 0.025M formic acid, HCHO2, and 0.018M sodium formate,…

A:

Q: A solution of 0.05 M benzoic acid (C6H5COOH) and 0.10 M sodium benzoate (C6H5COONa) has a pH of 4.50…

A: The above-given problem can be solved using the Henderson-Hesselbalch equation. pH = pKa +…

Q: In the following equation HNO2 (aq) + H2O (l) ↔ H3O+ (aq) + NO2-(aq), 0.37 M of nitrous acid was…

A: Given : Initial concentration of acid = 0.37 M ka for HNO2 = 4.5 × 10-4

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.