A solution made with U.12 oles of a triprotic acid dissolved Dilowing AaS :Kal = 5.5e – 02; Ka2 = 9.2e – 05; Ka3 = 8.0e – 08; this solution was titrated with 1.330 M NaOH. Calculate the pH at the following points of the titration and the volume of base in mL needed to reach the final equivalence point:

Q: Compare the percent ionization of the base in (a) with the percent ionization of the base in (b).…

A:

Q: CHEMWORK Consider a buffered solution containing CH2NH3C1 and CH;NH,. Which of the following…

A: pOH = pKb + log salt / base  Salt = CH3NH3+ Base = CH3NH2 If base is more than salt than pOH is less…

Q: The labels came off four cleaning solution containers found under a k ink. Each of the cleaning…

A:

Q: Ca luck are the solubility of each of the following salts in moles per lister given the lap values.…

A:

Q: Ok thank you. What would I use if 60 ml of HI is added since that would remove the base? Do I use an…

A: Note: ICE table can used to solve this question but Ostwald's dilution law has been derived from ICE…

Q: Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry…

A: Given the pKa of aspirin, pKa = 3.5 => Ka = 10-pKa => Ka = 10-3.5  Given the pH of stomach, pH…

Q: Question: You added 8 drops of Alizarin Yellow indicato and your solution appears yellow and…

A: Alizarin, also known as 1,2-dihydroxyanthraquinone (C14H8O4), is a natural dye that, as an…

Q: A compound of gallium with chlorine has a melting point of 77 °C and a boiling point of 201 °C. Y…

A: We have compound of gallium and chlorine with melting point 77 °C and boiling point of 210 °C.We are…

Q: Using the known value for the Ka for acetic acid (1.76x10^-5),calculate the expected ph of an acetic…

A: Acetic acid, CH3COOH, is an organic acid. It is a weak acid with Ka of 1.76 x 10-5. It is a…

Q: Ine pH of a 500.00 ml buffer solution containing sodium mandelate and mandelic acid (ka- 3.89x10…

A: Given, Ka = 3.89 x 10-4 ao = 0.90 Formula Used, pKa = - log (Ka) pH is calculated by…

Q: 60 mL of 0.1M HOAc (Ka= 1.75X105) was titrated with 0.1M NaOH. a) What is the pH after addition of:…

A: "Dear student, as an expert we are only allowed to answer one question at a time and 3 sub-part at a…

Q: PROBLEM 1: Physics in Substances' Quality Control. Binary solutions are mixtures of two components,…

A: Density of a substance is physical property that is unique to the particular substance. It can be…

Q: What is the pH of a solution that is 0.753 M in ethylammonium chloride (CH3CH₂NH3CI)? The K, of…

A: Given , Kb(ethylammonia ) = 5.6×10-4

Q: Natural goldenrod pigment is a yellow dye that changes to a bright red color in the presence of a…

A: Given Natural goldenrod pigment is a yellow dye that changes to a bright red color in the presence…

Q: ) Create a protocol for preparing 500 mL of 0.1 M Borate buffer, at pH 8, assuming you already have…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: the Ka of an unknown acid

A: From the data given in the question, we have obtained the following titration graph using origin…

Q: Mark which of these apply to Image A in Document 1. Should have 4 answers. (A) low initial pH B)…

A:

Q: Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry…

A: GIVEN: Bicarbonate was an effective buffer in Molly’s situation To determine: what else could/does…

Q: Nitric acid readily dissolves UO₂. Why doesn't hydrochloric acid dissolve UO2?    Please provide…

A: Nitric acid - HNO3  Uranium dioxide - UO2

Q: ) Calculate mass of the acid required to prepare 100 cm' of 0.1 solution of this acid.(Molar mass of…

A: Solution: a) here we have to prepare 100 mL of 0.1 M  acid solution. given molar mass of acid is…

Q: Answer only letter a. 1.) Calcualte the pH of the 0.30 M NH3/0.36 M NH4Cl buffer system. a) What is…

A: Buffer solution are those solution which has constant pH and it contains both acidic as well as…

Q: What are the K1 and K2 (dissociation constants)? Given... Molarity NaOH: .3, Concentration of…

A: The question is based on the titrations.  we are titrating a weak diprotic acid with a strong base.…

Q: A solution contains0.023Macetic acid and0.0.018Msodium acetate. The Ka for acetic acid is1.8×10−5.…

A: Molarity of acetic acid = 0.023 M Molarity of sodium acetate = 0.018 M Ka = 1.8 ×10-5

Q: Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry…

A: Activated charcoal is made from sources of carbon like coal, wood, etc. which is treated at high…

Q: The following solution mixture which is/are buffer... Select one or more. Select 5 correct answer(s)…

A: The mixture of a weak acid and its salt can behave like a good acidic buffer. On the other hand, the…

Q: A 10.0 ml of 2.0M sulfuric acid needs 12.5ml 25tds do of NaOH to neutralize it. compute for the ff.…

A: Given: Volume of sulfuric acid = 10.0 ml Molarity of sulfuric acid = 2.0 M Volume of NaOH = 12.5 ml

Q: To prepare the buffer, a total volume of 500 mL is required. The stock solution of the weak base is…

A: Given: Buffer solution of weak base pyridine (assuming B) and its conjugate acid HB+. pH of solution…

Q: By mixing formic acid and sodium formate a buffer solution was prepared in a way that the [Formic…

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

Q: Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry…

A: A blood pH lower than the normal blood pH of 7.4 has many bad impacts in our body which are given…

Q: Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry…

A: Given the pKa of aspirin, pKa = 3.5 => Ka = 10-pKa => Ka = 10-3.5  Given the average pH of…

Q: IS. To prepare for laboratory: For each of the eight unknowns solutions that you will identify in…

A: The above 8 components are- H2SO4, Ba(NO3)2,NaHCO3,KSCN,NaOH,Fe(NO3)3, NH4OH,Cu(NO3)2

Q: Case Study Section 1 – pH Based on “The Case of the Mortified Mom: Acids, pH and Buffers” by Terry…

A: Human blood has a buffer system of carbonic acid(H2CO3) and bicarbonate ion (HCO3-).

Q: A certain weak acid, HA, with a K. value of 5.61 x 10-6, is titrated with NaOH.

A:

Q: To prepare the buffer, a total volume of 500 mL is required. The stock solution of the weak base is…

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

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.