For bromocresol green indicator, the pka of the indicator is about 4.7.  Estimate the pH range over which the color change occurs for bromocresol green.  What would be the effect on your results if methyl red indicator, pka = 5.0 were used during the experiment

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: Which are TRUE for the use of indicators with dichromate? Dichromate is orange and changes color to…

A: Please find the below attachment.   Please rate if it is helpful for you.   Thank you.

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: Assess the suitability of methyl orange to signal the equivalence point in weak acid and strong base…

A: Methyl orange is a widely used pH indicator in titrations.

Q: Answer 2A, 2B, and 2C. The pKa Values are in the separate pic.

A: 2A The acid with pKa close to the pH would be the best choice for preparing a buffer solution. pH of…

Q: In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the necessary…

A: Given: Volume of buffer solution = 100 mL pH of buffer solution = 9.02  Concentration of acid and…

Q: 25.0 cm3 of sodium hydroxide solution is tritrated against 0.2 mol dm–3 hydrochloric acid until the…

A: Given,  Volume of the NaOH = 25.0 cm3  Molarity of HCl = 0.2 mol/dm3  Volume of HCl = 27.5 cm3  At…

Q: The following is list of weak acids and their pka values weak acid „pKa benzoic acid 4.20 hydrogen…

A: The acid data given is,

Q: 3. The colour changes corresponding to the pH intervals for the three indicators are given in the…

A: So according to the given data and the indicator we have the following conclusion. :

Q: A biochemist working with bacteria requires a culture buffered at a pH of 3.6. Which of the…

A: Given that:  pH = 3.6 Buffer solution is mixture of weak acid and its conjugate base . Buffer…

Q: 21. For which of the following titrations would phenolphthalein (end point occurs at pH = 9.1) be…

A: The endpoint of the phenolphthalein occurs at pH 9.1. It states that this indicator is best for…

Q: A mixture of 0.15 M acetic acid and 0.34 sodium acetate is given. Calculate the pH of the medium if…

A: The given data contains, Acetic acid = 0.15 M. Sodium acetate = 0.34 M. pKa of acetic acid = 4.87

Q: A solution containing Mg2+ was buffered to pH 9.97 and titrated with EDTA. Eriochrome black T, with…

A: Eriochrome black T is a diprotic acid, represented as H2E.

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: Your goal is to make a buffer with a pH of 4.75 from acetic acid and sodium acetate. Assume the pka…

A: Given: pH = 4.95 ; pKa=4.74 find x=?

Q: Why is the electrometric method of pH determination more accurate than the colorimetric method?

A: The Electrometric Method for assessing a solution's Hydrogen Ion Concentration, or pH value, entails…

Q: Why is Potassium Chromate used as the indicator in Mohr Method Determination of Chloride? Explain

A: Potassium Chromate used as the indicator in Mohr Method for determination of Chloride.

Q: Given the chemical equation for the anthocyanin extract of red cabbage as an indicator. HIn + H20 S…

A: Indicator is a compound that indicates the acidic and basic character of the solution. These are…

Q: If 25,0 cm3 of the NH3 (concentration 0,10 mol∙dm–3) is titrated with the HCl (concentration 0,10…

A:

Q: Consider the list of acids and their pKa values attached What two compounds would be best to use in…

A: Buffers are effective when the pKa values are closest to pH.

Q: What will happen if large quantities of indicator solution are used for the determination of pH by…

A: To explain: What happens if large quantities of indicator solution is used for the determination of…

Q: What is selective precipitation?  What is confirmatory test and its significance?  What are the…

A: In selective precipitation only specifically the one which is desired is precipitated in presence of…

Q: Consider the list of acids and their pKa values attached What two compounds would be best to use in…

A: A buffer solution performs best when the concentration of acid/ base is equal to the concentration…

Q: escribe  the curve and why pH = pka at half equivalence point

A: pH is negative logarithm of Hydrogen ion concentration

Q: bottle of Na2EDTA.2H2O is labeled with an assay of 100.5%, what is this implied? What is the result…

A: A substance’s purity is a measure used to identify whether it is pure or not. Generally pure…

Q: Calculate the pH of a buffer solution containing 10.0 cm³ of 0.100 mol dm-³ NaOH and 20.0 cm³ of…

A: 1 dm^3 = litre  1 cm^3 = milli litre  Millimoles = molarity (mol/L)* volume (in ml)

Q: Given the chemical equation for the anthocyanin extract of red cabbage as an indicator. HIn + H2O ⇌…

A: An indicator is a substance that tells you how acidic or basic a solution is. These are mainly weak…

Q: What is a 3 point calibration in titration?

A: Detail about 3 point calibration in titration is given below.

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: All of the following criteria must be met for a titrimetric analysis to be feasible EXCEPT:

A: The following is the fundamental concept of titration:   A solution is applied to the sample to be…

Q: Why is the equilibrium between the acid NaH2PO4, and its conjugate base Na2HPO4, a suitable buffer…

A: When a solution is referred to as a weak acid or weak base, it means that the solution can undergo…

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

A:

Q: The pKa of a weak acid was determined by measuring the pH of a solution containing the weak acid at…

A:

Q: A 50.0 mL of acidic solute (Ka = 2.6 x 10-2) is titrated with a 25.0 mL of 0.001 M NaOH solution.…

A: Since you have posted multiple questions, we are entitled to answer the first only.

Q: For PbCl2, Ksp = 1.7 × 10−5 . What will occur if 250 mL of 0.12 M Pb(NO3)2 is mixed with 250 mL of…

A: Solubility product constant Ksp is an equilibrium constant that is defined as the product of the…

Q: Your goal is to make a buffer with a pH of 4.75 from acetic acid and sodium acetate.  Assume the pKa…

A: Buffers are solutions that resists the change in pH on addition of small amount of acid or base to…

Q: After a buffer solution of carbonic acid (with pKa of 3.75) was added with 1ml of sulfuric acid, the…

A: Buffer solution is that which resist the change in pH value pH of a weak acid and it's conjugate…

Q: In the experiment of the acid dissociation constant of a weak acid using potentiometric titration,…

A: Solid NaOH can absorb water molecules from the atmosphere and hence, they are hygroscopic.…

Q: 2. In an iodometry titration, the appearance of blue colour upon addition of starch indicator is…

A: Iodometry titration can be defined as a method of volumetric analysis where the appearance or…

Q: Inorganic Chemistry: Qualitative Analysis of Anions What is the importance or purpose of adding…

A:

Q: Given that the Ka value of Thymolphthalein, weak acid and acid-base indicator, is equal to 1 x…

A: 1- In this question, we want to determine the pH of the solution in which indicator change the color…

Q: A sodium hydrogen carbonate/sodium carbonate buffer system is to be prepared with a pH of 9.89.  The…

A: Answer is explained below.  The given information are as follows:

Q: A weak acid (HA) with a pKa of 4.0 has a distribution constant of 5.2 between an organic and aqueous…

A: The fraction of HA acid in the organic phase at pH 2 and 6 is calculated:

Q: For which of the following titrations would phenolphthalein (end point occurs at pH = 9.1) be the…

A: Indicator in chemical reaction is chemical substance which changes color in a chemical change. An…

Q: The acid-base indicator "Thymol Blue" has two transition ranges as listed below (with the…

A: The pKa values of the forms of thymol blue can be calculated as:   pKa=-log Ka

Q: Which of these compounds would be the best buffer at pH 5.0: formic acid (pKa = 3.8), acetic acid…

A: Given: The pH of the buffer solution = 5.0 The pKa of formic acid = 3.8 The pKa of acetic acid =…

Q: In this exercise, using the Henderson-Hasselbach equation, you will be asked to make the necessary…

A: Answer-a Henderson-hasslebalch equation is: pH=pKa+log[Base][Acid] if [Base]=[Acid}, then…

Q: Dr. Stone and Princess Bubble gum wanted to run an experiment to determine at what volume they will…

A: Given: Titration of CF3COOH with a pKa of 0.52 with 0.1 M NaOH.

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.