24. A solution is prepared by mixing equal volumes of 0.20M HC,H3O2 and 0.40M Nac,H3O2. Which of the following correctly describes what occurs if a small amount of HCl(aq) or NaOH(aq) is added?

Q: Is the following solution a buffer? Each solution was prepared by mixing and diluting appropriate…

A: The mixture cannot serve as a buffer solution.

Q: A buffer solution is made that is 0.498 M in HNO2 and 0.498 M in KNO2. If Ka for HNO2 is 4.50 x…

A:

Q: Classify the solution that results, if you mix 50.0 mL of 0.20 M KOH(aq) and 50.0 mL of 0.20 M…

A:

Q: Starting with 0.1 mol L−1 HNO2(aq), which one of the following operations would cause the pH of the…

A:

Q: 30.0 ml of 0.1 M NaOH is mixed with 20.0 ml of 0.1 M Ba(OH)2 and 20.0 ml of 0.2 M HClO4. What is the…

A: In this question, we want to determine the the pH of the resulting solution.  You can see details…

Q: . Calculate the moles of H2O that can be obtained from 15.0 mL of 0.250 M HCl according to the…

A: The given balanced chemical reaction is as follows: 2KMnO4(aq) + 16HCl(aq) → 2MnCl2(aq) + 5Cl2 +…

Q: The pK, values for the dibasic base B are pKb1 = 2.10 and pKb2 = 7.42. Calculate the pH at each of…

A: Here a dibasic base is titrated with HCl. Let us consider the base to be B.  pkb1 = 2.10 , pkb2=…

Q: 7) What is the pH of a solution (aq., 25 oC) of a 25.0 mL sample of 0.300 M Ba(OH)2 that has 50.0 mL…

A: Given data contains, Molarity of Ba(OH)2 is 0.300 M. Volume of Ba(OH)2 is 0.025 L. Molarity of HNO3…

Q: Write a net ionic equation for the reaction with OH- by which antimony(III) hydroxide dissolves when…

A: Here we have to write the net ionic equation for the reaction of hydroxide ion with antimony (III)…

Q: A27.7 mL sample of 0.236 M methylamine, CH;NH, is titrated with 0.337 M hydroiodic acid. After…

A:

Q: Calculate the pH of the resulting solution if 27.0 mL of 0.270 M HCl(aq) is added to 32.0 mL of…

A:

Q: A 44.6 mL of 0.103 M HCI is added to an antacid sample. The solution is titrated to a bromophenol…

A: Given, Volume of HCl = 44.6 mL = 0.0446 L   (1mL = 0.001 L) Molarity of HCl = 0.103 M = 0.103 mol/L…

Q: A 5.10 mLmL sample of an H3PO4 solution of unknown concentration is titrated with a 1.100×10−2…

A:

Q: A 250.0 mL sample of 0.328 M HOCl(aq) (Ka = 2.9 x 10−8) is titrated with 0.457 M NaOH(aq). How many…

A:

Q: Why is the pH of the HCl (aq) solution initially lower than the pH of the CH3COOH solution in a…

A: We have asked for the reason why the pH of the HCl(aq) solution initially lower than the pH of the…

Q: Describe what happens when you mix an aqueous solution of NaOH with an aqueous solution Fe(NO3)2? In…

A: An aqueous solution of NaOH mixed with an aqueous solution Fe(NO3)2

Q: What volume (in mL) of a 0.153 M sodium hydroxide solution must be added to a 20.0-mL sample of a…

A: The question is based on the concept of titration. We are titrating a strong acid with a strong…

Q: temine the concentration of a NaOH(ag) solution, s student titreted a 50. ml. sample with 0.10…

A:

Q: Which of the following describes the titration of HCl(aq) with Ba(OH)2(aq): strong acid with strong…

A: Which of the following describes the titration of HCl(aq) with Ba(OH)2(aq) has to be given.

Q: A 25.00 ml sample of methylamine ,CH3NH2, of unknown concentration was titrated with 0.1000 M HCl.…

A: Volume of CH3NH2 = 25.0 mLConcentration of HCl = 0.10 MVolume of HCl = 28.55 mLKb = 4.4x10-4

Q: A 20.0 mL 0.150 M HF (aq) was titrated with 0.125 M KOH(aq) to convert all the initial acid to…

A: The pH of a solution helps us to determine the acidity or alkalinity of a solution. The pH is…

Q: Which of the following reactions are not consistent with the concept of acid base amphoterism? OA)…

A: The aim of this question is to show the metal oxides or hydroxides, amphoterism is crucial for…

Q: Chan the chemistry student carries out a titration by adding an aqueous solution of NaOH to an…

A:

Q: c. Identify one other difference that you would expect if you tested these two solutions. Include…

A: Both nitric and nitrous acids contain nitrogen as the central atom. In nitric and nitrous acids, the…

Q: 0.115 M KOH solution was used to titrate a 32.90 mL sample of a weak acid solution, HC3H5O2, of…

A:

Q: When answering this problem, report the answer with the appropriate number of significant figures.…

A: Given data is as follows: The volume of acetic acid = 1.130×101 mL The concentration of acetic acid…

Q: A buffer solution is made that is 0.482 M in HS and 0.482 M in NaHS. If Ka for H2S is 1.00 x 10-7,…

A: Given: Concentration of weak acid H2S = 0.482 M Concentration of conjugate base salt of weak acid…

Q: A buffer solution is made that is 0.408 M in HClO and 0.408 M in NaClO. If Ka for HClO  is 3.50 x…

A:

Q: The pK, values for the dibasic base B are pKbl = 2.10 and pKb2 = 7.38. Calculate the pH at each of…

A: pkb1 = 2.10 pkb2 = 7.38 [B] = 0.95 M [HCl] = 0.95 M V = 50.0 mL

Q: Chadwick the chemistry student carries out a titration by adding an aqueous solution of NaOH to an…

A: Chadwick the chemistry student carries out a titration by adding an aqueous solution of NaOH to an…

Q: Propionic acid, HC3H5O2, has a Ką value of 1.3 x 105. A buffer solution is prepared by mixing 20.0…

A: Given:- Propionic acid, HC3H502, has a Ką value of 1.3 x 10-5. A buffer solution is prepared by…

Q: A buffer is prepared by mixing 60.0 mL of 0.422 M HBrO and 75.0 mL of 0.375 M KBrO. Ka = 2.5 x 10^-9…

A: Henderson-Hasselbach equation shows the relationship between pH of a solution, the acid dissociation…

Q: A buffer solution is made that is 0.322 M in H2S  and 0.322 M in KHS . If Ka1 for H2S is 1.00 x…

A: Buffer solution :-         Buffer solutions are those solutions which resist a change in pH  upon…

Q: Consider the following information to answer the questions below. A volume of 10.00 mL of 0.100 M…

A: At equivalence point,  Number of moles of acid = Number of moles of base  Therefore for acid-base…

Q: Determine the volume in mL of 0.251 M HBr(aq) needed to reach the equivalence (stoichiometric) point…

A: Given information, Molarity of HBr = 0.251 M Volume of (CH3)2NH = 25.92 mL Molarity of (CH3)2NH =…

Q: write the formula for the salt formed by mixing Pb2+(aq) and OH- ions as PbOH or PbOH2. Explain why…

A:

Q: The mineral tri-magnesium phosphate (Mg3(PO4)2, denoted TMP) is widely used in the pharmaceutical…

A: 1.) Reaction is: 3 Mg Cl2 + 2 K2HPO4 = Mg3(PO4)2 + 4 KCl + 2 HCl Moles of Mg Cl2=0.5 x 0.2=0.1 moles…

Q: solution containing H2CO3 and HCO3- is a buffer (in blood). Which of the two would be consumed if a…

A: Given-> Buffer ->H2CO3/HCO3-

Q: 1. THE SHIFTING OF AN EQUILIBRIUM: THE COMMON ION EFFECT Weak Acids and Weak Bases • • • Let us now…

A: Citations: Libretexts. (2023b, July 12). 18.3: Common-ion effect in solubility equilibria. Chemistry…

Q: The table has data from the titration of four 10.0 mL samples of a solution containing hydrochloric…

A: Titration of 10.0mL of HCl(aq) with 0.229mol/L NaOH(aq)

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.