Which one of the following indicators is best suited for titrating 0.05 M methylamine (pK, = 3.19) with 0.05 M HCI? A. Bromophenol blue, pKa = 3.9 B. Methyl red, pKa = 5.0 O C. Phenol red, pK, = 7.9 O D. Bromocresol purple, pKa = 6.3 OE. Alizarin yellow, pK, = 11.2 O O

Q: 1.00 mL of 12.0 M HCl is added to 1.00 L of a buffer that contains  0.100 M  HNO2 and 0.200 M…

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Q: equivalence

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Q: . In a titration of a strong base with a weak acid at 25oC, the theoretical pH at equivalence point…

A: In a titration of a strong base with a weak acid at 25 oC, the theoretical pH at equivalence point…

Q: Which one of the following indicators is best suited for titrating 0.05 M pyridine (pKb = 8.82) with…

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Q: 3.) What is the pH at the equivalence point for the titration of 50.0 mL 0.20 M nitrous acid by 0.20…

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Q: Consider a titration of 40.00 mL of 0.1250 M Na2CO3 with 0.4000 M HCl.  Carbonic acid (H2CO3) has a…

A: The number of milliequivalents of sodium carbonate Na2CO3 = 40.00 x 0.1250 = 5 mmol The number of…

Q: For the buffer solution of weak acid HA and its conjugate base salt NaA, There are two equilibrium…

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Q: molar solubility

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Q: Which indicator would be the best to use for a titration between 0.30 M (CH3)2NH with 0.30 M HI? You…

A: An indicator gives the information about the equivalence point in an acid base titration by changing…

Q: Which one of the following indicators is best suited for titrating 0.40 M ammonia (pKb = 4.74) with…

A: The chemical reaction occurs in the given titration (strong acid+weak base) is: NH3 + HCl = NH4Cl…

Q: Calculate the pH of 1.00 L of a buffer that contains 0.110 M HNO2 and 0.185 M NaNO2. What is the…

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

Q: A buffer solution containing only 0.050 mol of CH3NH2 and 0.060 mol of CH3NH3CI has a total volume…

A: Given: Moles of CH3NH2 = 0.050 mol. Moles of CH3NH3Cl = 0.060 mol. And the moles of NaOH added =…

Q: 50.0 mL of HCIO2 is titrated with 16.38 mL of 0.25 M NaOH before the color change of the endpoint…

A: 50.0 mL of HClO2 is titrated with 16.38 mL of 0.25 M NaOH before the color change of the enpoint…

Q: a weak species is titrated with a strong acid or base. was the species a weak acid or a weak base…

A: This question is based on titration curve.

Q: What acid-base indicator should be used for the titration of 50.00mL of 0.0500 N HCl with 0.0500 N…

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Q: a. What is the pH of 50.00 mL buffer solution which is 2.00 M in HC,HO2 and 2.00 M in NaC2H3O2? (K,…

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Q: A mixture contains initially benzoic acid C6H5CO2(weak acid), Ka = 6.28 x 10^-5, and its…

A: Given data :  Ka of benzoic acid = 6.28 x 10^-5 , concentration of benzoic acid = 0.250 M…

Q: What volume of 1.35 M HCI must be added to 0.264 L of 0.213 M dimethylamine to produce a buffer with…

A: We are asked to find the volume of 1.35 M HCl that must be added to 0.264 L of 0.213 M dimethylamine…

Q: What masses of dimethylamine and dimethylammonium chloride do you need to prepare 3.00 L of pH =…

A: Given,  The volume of dimethyl amine and dimethyl ammonium chloride buffer = 3.00L The total…

Q: What is the relationship between pAg and pCl at the equivalence point in the titration of chloride…

A: Volumetric method based upon the formation of precipitate is called " precipitation titration "

Q: How many grams of solid potassium nitrite should be added to 1.00 L of a 0.262 M nitrous acid…

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

Q: What is the maximum concentration of Ag+ that can be added to a 0.00250 M solution of Na2CO3 before…

A: The solubility product (Ksp) constant is the equilibrium constant for the dissolution of a solid…

Q: Hd saibay 3. A new monoprotic weak acid is synthesized. This acid is titrated with NaOH (V(NaOH…

A: Titration curve: The curve obtained from the plot of pH vs the amount of titrant added. Typically,…

Q: 4. A buffer was prepared using 10.0 mL of 1.90M HAc and 1.20 M NaAc (where Ac- is C2H3O2- ). The Ka…

A: Buffer solution are those who resist the change in pH of solution on small addition of strong acid…

Q: 2. 100.0 mL of a 0.0875 M weak base solution is titrated with 0.250 M HCI. The pH after the addition…

A: Given,  Concentration of weak base (say B) = 0.0875 M  Volume of B in mL = 100.0 mL  Concentration…

Q: Calculate the change of pH of a buffer system with a pH of 7.323 if 0.217 mol potassium hydroxide…

A: If 0.217 mole of NaOH was added to the system  pH = 7.323Volume of phosphoric acid  525 mL = 0.525 L…

Q: Calculate the pH of 1.0 L of a buffer that is 0.130 M  HNO2 and 0.170 M  NaNO2. What is the pH of…

A: Given   The volume of buffer is 1.0 L. The molarity of HNO2 is 0.130 M. The molarity of NaNO2 is…

Q: What is the maximum concentration of Ag+ that can be added to a 0.00650 M solution of Na₂CO3 before…

A: Answer: At the saturation point  ionic product of silver carbonate will become equal to its…

Q: A 20.0 mL sample of 0.150 M ethylamine is titrated with 0.0981 M HCI. What is the pH after the…

A: Given  mmoles of base = 0.15 M x 20 mL = 3 mmoles of acid = 0.0981 M x 5 mL = 0.4905…

Q: Which of the following compounds is BEST to construct a buffer at pH 8.00? Аcetic acid (pKа %3D…

A: Answer Buffer :- weak acid and its conjugate base makes the buffer…

Q: Which of the following combinations would make a buffer closest to pH 5.0?

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Q: In an acid base titration of Ca(OH)2 (base) and HCl (acid), if the base is solid an equilibrium…

A: Given reaction  Ca(OH)2 (s) = Ca+2 (aq) + 2OH- (aq)  In accordance with  Le Chatelier’s principle  ,…

Q: 3..[CHEMISTRY] What will be the pH in the titration of 0.01 L of 200 millimolars H2CO3 by 100…

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Q: Consider a titration of 40.00 mL of 0.1250 M Na2CO3 with 0.4000 M HCl.  Carbonic acid (H2CO3) has a…

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Q: What volume of 0.50 M HNO3 should be added to 200. mL of 0.25 M NH3 in order to create a buffer with…

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Q: 1. 20.0 ml of 0.500 M Acetic Acid (CH3COOH) is titrated with 0.500 M KOH. Find the pH a. Before…

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Q: 9. Consider the titration of a sample of a weak acid with a strong base (titrant). What is the…

A: 9. A weak acid is titrated with a strong base.  Here, we have to select the correct option for the…

Q: Ammonium chloride has a pKa of 9.26. NH4+ = NH3 + H+. One adds 3.35 grans solid NH4Cl to 500.0 mL of…

A: Buffer system is a solution which resist the change in pH of solution upon addition of small amount…

Q: Calculate the pH of 1.00 L of a buffer that is 0.110 M  HNO2 and 0.190 M  NaNO2. What is the pH of…

A: HNO2 is a weak acid it reacts with conjugate base is NaNO2 , together they form a buffer solution.…

Q: What is the ph of a buffer composed of 1.00M NH4 and 0.50M NH4Cl? Kb=1.85x10^-5

A: The base ionization constant for acid is 1.85×10 -5.

Q: The gure below shows a utration table for the tree ammo acid glycine (which is diprotic). At which…

A: Ans is II. At low pH, glycine is in fully protonated form. Here, Carboxyl group (–COOH) has pKa of…

Q: What masses of bromoacetic acid (CH2BrCOOH) and sodium bromoacetate (CH2BrCOONa) are needed to…

A: pKa   = -log Ka           =  - log (2.00  * 10-3 )          = 2.70

Q: A 20.0 mL sample of 0.150 M ethylamine is titrated with 0.0981 M HCl.What is the pH after the…

A: The volume of 1 L is equal to 1000 mL. The number of mole (n) of ethylamine is calculated as shown…

Q: For the titration of a weak acid with a strong base, the pH at the midpoint was 5.06. What are the…

A: I

Precipitation Titration

Precipitation analysis is used to analyze drugs, and to measure the salt content in food and beverages. It is an important concept from the examination point of view many practical questions are asked on the topic. This topic is significant in the professional exams for both undergraduate and graduate courses, especially for