4. Identify the Brønsted-Lowry in each reaction: Acid & Base, and also the conjugate acid and conjugate base HCIO3(aq) + H₂O(1) H₂0 (aq) + ClO3(aq) 5. Which of the following combinations make a buffer solution? Explain your choice a. HCI and KCI b. H₂CO₂ and NaHCO3 c. H₂PO4 and NaCl d. HC₂H₂O₂ and KC₂H₂O₂

Q: Phosphoric acid is often added to colas to give them the tart flavor people like. Coke Classic® has…

A: H3PO4 dissociates as: H3PO4↔H++H2PO4-                            Ka1=6.9×10-3H2PO4-↔H++HPO42-…

Q: Consider the Ka information to answer parts a-b. Ka 7.2 x 10 * K 4.2 x 10- Formula Kat 6.3x 10 a.…

A: Answer:- This question is answered by using the simple concept of calculation of Ka and Kb value…

Q: What is the pH of a solution when 4.9 g of ammonium bromide, NH,Br (M=98) , is used to make 200 mL…

A: Mass of NH4Br = 4.9 g Volume of solution = 200 mL K = 5.6E-10 pH =?

Q: If a buffer solution is 0.420M in a weak acid (a=4.8x10-6) and 0.230M in its conjugate base, what is…

A:

Q: Predict whether Fe(NO3)2 and sodium acetate will be acidic or basic salts. Please explain based on…

A: Salt is formed by reaction of acid with base. So it has cationic part which comes from base while…

Q: is solution is prepared by mixing 25 mL of 0.1 M HCHO2 with 25 mL of .2 M NaCHO2. The pH of the…

A: Given values-> Volume of HCHO2 = 25ml Molarity of HCHO2 = 0.1 M Volume of NaCHO2 = 25 ml Molarity…

Q: Which of the following statements about indicators is incorrect? a. An indicator is an organic…

A: C. Phenolphthalein is colorless when the pH > 8 Phenolphthalein is actually colorless below pH 8…

Q: To make a common phosphate buffer using potassium hydrogen phosphate and potassium dihydrogen…

A: Answer: A buffer solution is the type of solution that resist the change in its pH on adding small…

Q: a buffer solution is 0.210 Min a weak base (?b=1.6×10−5) and 0.490 M in its conjugate acid, what is…

A: Given-> Concentration of weak base (BOH) = 0.210 M Kb = 1.6 × 10-5  Concentration of conjugate…

Q: 11. A 80 mL solution containing 0.25 M formic acid (HCOOH) and 0 35 M sodium ascorbate (NaCoH;Oe)…

A:

Q: HF dissociates according to the following equilibrium: HF(aq) ⇌ H+(aq) + F-(aq) If 1.0 M NaF is…

A:

Q: Which of the following is/are true when CH3COOH is dissolved in water? I.            At…

A:

Q: HF is a weak acid. If a solution of HF with a pH of 4.5 is made, Which of the following would be the…

A:

Q: u make 50.00mL of a 0.045M solution of NaOH from a 2.5M stock solution. 9. How many milliliters of…

A: Answer: As, for the dilution, we add water in the solution, therefore moles of NaOH taken from stock…

Q: What is the pH of a solution when 4.9 g of ammonium bromide, NH4B (M=98) , is used to make 200 mL of…

A:

Q: 6. Consider the reaction of 50.0 mL of 2.0 M nitric acid with 90.0 mL 1.0 M potassium hydroxide.…

A: The equation of given reaction is,

Q: . The equilibrium constant for the dissociation of a weak acid of the type, HA⇌H++ A-, would be:…

A:

Q: Which of the following acid / base conjguate pairs is the best to make a buffer Solution? OA.…

A: A buffer is a solution that resists any change in pH on adding small amount of acid or base to it.…

Q: 1. Buffers are made from weak conjugate acid-base pairs. In Part A, step 4, of the procedure a weak…

A: Given preparation of buffer solutions. An acidic buffer solution can be prepared by the following…

Q: Which of the following is/are true when CH3COOH is dissolved in water? I.             At…

A: Acid can be defined as a species that donate hydrogen ions in aqueous solution. Acid can be weak or…

Q: Please don't provide handwriting solution

A: Ka = C2Here  Ka = Disociation constant = ?          C = concentration = 1.43 M           = Digree of…

Q: A buffer solution is composed of 1.00 mol of acid and 6.25 mol of the conjugate base. If the p?a of…

A: If the solution is resistant to any change in pH when small amount of acid or base is added to that…

Q: Consider the weak acid H2A and its Conjugate base HA-. Which diagram below represents a buffer…

A:

Q: An aqueous solution contains 1x 10^-5 M hydrogen ions. How much hydronium ions does it contain?*

A: Hydrogen ions or hydronium ions are considered to be same.

Q: react

A: At pH = 12,  HPO4^2-(aq) + H2O(l) <-----> PO4^3-(aq) + H3O+(aq)  When an external acid H3O+…

Q: 5. When 50.0 mL of 0.125 mol/L ethylamine (CH,CH2NH2) is titrated with o. 00 mol/L HCI, what is the…

A: According to the mole concept, in terms of mass, the amount of substance in moles is equal to the…

Q: A solution that contains a weak acid and its conjugate base in roughly equal concentrations is A.…

A:

Q: Which of the following is TRUE when 2.0 mL of 0.10 M KOH is mixed with 15 mL distilled water?…

A:

Q: 1. Consider the following three statements about neutralisation reactions: I. A neutralisation…

A: 1) A neutralization reaction always defines the reaction between an acid(strong/weak) and a…

Q: Lactic acid solution is formed. a. b. Write the reaction where Lactic acid is reacted with water.…

A:

Q: solution. WFiat Is fhe 8. What is the Hydrogen ion concentration in 500 ml of a 0.100 M solution of…

A:

Q: 4. A 0.30 M solution of a salt NaA has pH-8.11. What is the value of K, for the parent acid HA? 5. A…

A: The objective of the question is to determine the value of  for the parent acid HA.It is given…

Q: None

A: Part 2: Explanation:Step 1: Determine the moles of hydrazine.Volume of hydrazine solution: 125.00 mL…

Q: 5. Calculate the molar concentration of Mg when the pH of the solution is adjusted to 11.50. The Kp…

A: pH = 11.50 Ksp = 8.9 × 10-12

Q: H,A is a diprotic acid, for which K, = 5.7 × 10* and K,2 = 1 × 1o ". Determine the concentration of…

A: Given: Ka1=5.7×10-8Ka2= 1×10-19[H2A]= 0.10M To find: The concentration of A2-

Q: trong base is dissolved in 675 mL of 0.200 M weak acid (?a=3.87×10−5) to make a buffer with a pH of…

A: In this problem, we are dealing with a chemical equilibrium scenario involving a weak acid (HA) and…

Q: a solution is made from 0.23 M CH3NH2 (a weak base) and 0.24 M CH3NH3Cl. what is the pH of the…

A: The pH of this buffer solution can be calculated by using Handersson-Hesselbalch equation-

Q: HCN is a weak acid (?a=6.20×10−10) , so the salt, KCN , acts as a weak base. What is the pH of a…

A: First write down the reaction between KCN and H2O. Then find OH- or H3O+ and using that find pH of…

Q: You are given a diprotic acid H₂A. 10.00 mL of this acid solution of 0.0200 M is titrated with NaOH…

A:

Q: 5. A 25.0 mL sample of 0.500 M formic acid (HCOOH) is titrated with 60.00 mL of 0.300 M NaOH. What…

A: The question is based on the concept of pH of the solution.  It is defined as a negative logarithm…

Q: Which of the following acid-base pairs may be used to prepare buffer systems? Explain. a. C6H5NH2…

A: A buffer is an aqueous solution which consist of a mixture of a weak acid and its conjugate base or…

Q: Of the following solutions, which has the lowest buffering capacity? OA. 0.521M HC2H3O2 and 0.217M…

A: A buffer is a solution which resist any change in pH on adding a small amount of acid or base .it is…

Q: you want to make a common ion solution from Nitrous Acid (HNO2) and its conjugate, sodium Nitrite…

A:

Q: Which of the following pairs of substances can be used to make a buffer solution?   a. HBr & KOH…

A: A multiple choice question based on buffer solution, which is to be accomplished.

Q: Can someone answer this question? My friends have three different answers 3.6, 3.47, and 1.6. Who is…

A:

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.