Why do you have to titrate until or above pH = 12.5 ± 0.2 to properly identify the unknown acid solution?

Q: The titration of 50.0 mL of 0.100 M acetic acid (Ka = 1.75 x10^-5) with 0.200 M sodium hydroxide at…

A: We need to calculate pH for the given titration

Q: Discuss the titration curve (variation of pH with respect to addition of titrant) with suitable…

A: A question based on pH titration curve, which is to be accomplished.

Q: Three-point calibration was not performed on the pH meter prior to titration.   Is there a…

A: Three-point calibration is performed on the pH meter when pH of a solution that can be both acidic…

Q: Explain: While you are performing the halogen test, and before the addition of AGNO3 you should…

A: While performing the halogen test, before the addition of AgNO3, we should acidify the sodium fusion…

Q: Why is a lower concentration of NaOH or HCl used for titration while a solution with higher…

A: Given information: NaOH or HCl

Q: How will the amount of hydrochloric acid titrant used for the analysis be affected if the mixture of…

A:

Q: Write two features of Erichrome black- T which makes it a suitable indicator in complexometric…

A: Two features of Eriochrome black- T has to be written The medium it undergoes complex formation has…

Q: An indicator was not used during potentiometric titration of a weak acid   Is there a positive…

A: A question based on potentiometric titration that is to be accomplished.

Q: Write the reaction between formic acid (Appendix B) and KOH. What is the equivalence volume (Ve) in…

A: As there are many subparts of the question and any specific subpart is not mentioned here, so solve…

Q: Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after…

A: (a)

Q: Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after…

A:

Q: Use the titration curve for the weak acid to calculate the pH of a 0.150 M solution of that weak…

A: The pKa of the acid will be equal to the pH at half equivalence point which can be determined by…

Q: For the titration: 30.0mL of 0.150 M NH3 (Kb = 1.8 x 10-5) with 0.250 M HBr Calculate the pH after…

A: For the given titration we have to calculate the pH

Q: 3. Why do the glasswares need to be rinsed with 0.1 M HNO3 prior to use?

A: M symbol denote molarity that determines concentration of nitric acid. Acid is a substance that give…

Q: A Mohr titration of NaCl is done at pH 2. Is there a positive error, negative error, no effect, or…

A: A question based on general chemistry that is to be accomplished.

Q: 5. Why should the titration solution be buffered at pH 10.0?

A: In complexometric titration the titrant used is EDTA. EDTA forms a complex with the metal ions which…

Q: In compleximetric titration, why should the conditional formation constant between the indicator and…

A: In complexometric titration, the metal ion concentration is determined with the help of a…

Q: What do you call the type of titrimetry in which you measure the quantity of charge in coulombs…

A: The titrimetry in which we measure the quantity of charge in coulombs required to complete a…

Q: Calculate the pH during the titration of 30.00 mL of 0.1000 M KOH with 0.1000 M HBr solution after…

A: The molarity of KOH is 0.1000 M. The volume of KOH used is 30.00 mL. The molarity of HBr is 0.1000…

Q: 13. What is the pH range should be maintained in an argentometric titration for the estimation of…

A: This method determines the chloride ion conc. of a  solution by titration with AgNO3. As the AgNO3…

Q: Why is the equivalence point pH necessarily below 7 when a weak base is titrated with strong acid?

A: Equivalence point of a acid-base titration is a point when equivalent amount of acid and equivalent…

Q: After preparing 500 mL of 0.1019 M NaOH solution, the cap is left open and it absorbs 0.652 g  CO2.…

A:

Q: Calculate the pH during the titration of 50.00 mL of 0.0500 M NaOH with 0.100 M HCl at 25oC after…

A:

Q: Acetic acid, HC2H3O2 (aq), was used to make the buffers in this experiment. Write the ionization…

A: Buffer solutions are geenrally used to  control the pH change of the solution. It resist to change…

Q: Acetic acid, HC2H3O2 (aq), was used to make the buffers in this experiment. Write the ionization…

A: Ionisation Equation of Acetic Acid

Q: Explain the factors that need to be considered in choosing the possible analyte-titrant-indicator…

A:

Q: At any stage of the saponification experiment of ethyl acetate, when the 25mL sample taken from the…

A: First we will calculate the amount of HCl used for reacting with excess NaOH left in saponification…

Q: In the determination of Mass% NaOCI in Bleach Sample (Titration), does addition of water to the…

A: During the mass % determination of NaOCl in bleach sample, first NaOCl is converted to HOCl in…

Q: In which cases are the wet Electorstatic Precipitators used?

A: In which cases are the wet Electrostatic Precipitators used?

Q: Calculate the pH of the mixture containing 12.0mL 0.125M NH,Br(aq), 15.0mL 0.175M NH3(ag), and 2.5mL…

A:

Q: What is the graduated glass tube used to add the titrant (base) to the analyte (acid)?

A: 1) To identify the graduated glass tube which is used to add the titrant (base) to the analyte…

Q: Would the indicator bromocresol green, with a transition range of pH 3.8–5.4, ever be useful in the…

A: weak acid react with strong base, it give basic solution. So, the pH of the solution after…

Q: How would you create a buffer solution at a pH of your choosing (between pH 4-6) by adding solid…

A: Given: Molarity of acetic acid=0.1 M Volume of acetic acid =50 ml Ka=1.75×10-5 pH=4-6 To find: Mass…

Q: Calculate the pH of the NH3/NH4Cl buffer after the addition of NaOH. How does it compare to the…

A: The pH of a basic buffer solution is determined using the Henderson-Hasselbalch equation - pOH =…

Q: Is the standardization of titrant always the first step in all titrimetric analysis? Why or why not?

A: To find: If the standardization of titrant always the first step in all titrimetric analysis?

Q: If the concentration of the weak base ammonia is 0.10 M and it is titrated with 0.1 M HCl, and the…

A: Calculation of pH of ammonia solution

Q: calculate the pH during the titration of 30.00 mL of .1000 M KOH with .1000 M HBr solution after the…

A:

Q: The titration curve from the reaction of a strong base with a weak acid is shown below. Recalling…

A:

Q: Why are the standard reagents used in neutralization titrations generally strong acids and bases…

A: During titration, chemical reaction takes place. Generally am acid reacts with a base. When the…

Q: if 15.00mL of 0.0500 M HCl is used to titrate 30.00mL saturated Ca(OH)2, calculate the molar…

A:

Q: Use the titration curve for the weak acid to calculate the pH of a 0.150 Msolution of that weak…

A: Solution:   Equivalence point volume = Veq Half equivalence point volume = 1/2 Veq pH at half…

Q: Consider the titration of 30.0 mL of 0.263 M weak base B (Kb = 1.3 x 1010) with 0.150 M HI. What…

A: Usually pH of a weak base and strong acid is given by  pH = pKa  But we will solve the full given…

Q: What are the effects produced by photo composition on an improperly stored standard solution of…

A: Since the end point does not exactly coincide with the equivalence point, the titrant should the…

Q: How will the reported molar solubility for calcium hydroxide be affected if the mixture of solid…

A: Molar solubility is the degree to which any particular compound undergoes dissolution process in a…

Q: The pH of amino acid is adjusted to 1.5 prior to titration to make sure that the amino acid has a…

A: There are 20 naturally occurring amino acid. They contain one carboxylic group one amino group, an…

Q: You are asked to go into the lab and prepare an acetic acid -sodium acetate buffer solution with a…

A: The molar ratio of CH3COOH to CH3COONa has to be determined

Q: Calculate the pH during the titration of 20.00 mL of 0.1 M NaOH with 0.100 M HCl  after the addition…

A: Given - Volume of NaOH = 20.00 ml Molarity of NaOH= 0.1 M Molarity of HCl = 0.100 M

Q: Why is the center of the buffer region of a weak acid–strong base titration significant?

A: The reason why the center of the buffer region of a weak acid–strong base titration significant gas…

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.