Ten milliliters of 0.20 M AgNo3 is added 10ml of 0.10M NaCl calculate the concetration of Cl- remaining in solution at equilibrium and the solubuility of the AgCl

Q: You have been asked to prepare a maleate buffer( Ka 3.908  x 10-4 ) using sodium maleate (M.W. =…

A: Buffer is a solution whose pH does not changes much when small amount of strong acid or base is…

Q: Which of the following aqueous solutions are good buffer systems? . 0.26 M nitric acid + 0.16 M…

A: Buffers are formed by weak acid and its salt, weak base and its salt or salt or weak acid and weak…

Q: True or False 1. Weak acids and weak bases ionize completely and irreversibly in a solution. 2.…

A: 1) False because weak acids and weak bases don't dissipated into H+or OH- completely it's an…

Q: Which of the following aqueous solutions are good buffer systems? 0.37 M potassium chloride + 0.24 M…

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Q: Define the following 1. Acidimetry 2. Alkalimetry 3. Titration 4. Equivalence point 5. End point 6.…

A: 'since you have posted a question with multiple parts, we will solve only first three parts for you.…

Q: An analytical chemist is titrating 196.9 mL of a 0.5300M solution of butanoic acid (HC3H,CO₂) with a…

A: Here we are required to find the pH of the solution.

Q: Explain how a buffer solution of carbonic acid and bicarbonate will react when: a strong acid,…

A: pH of a buffer solution remain unchanged with addition of few drops of acid and base.

Q: Malic acid (C4H5O5) is one of the alpha hydroxy acids which is naturally found in apples. The…

A: Given data,                     Concentration of HCl = 7.29 x…

Q: Answer the following three questions based on the information given below. Consider a buffer made…

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Q: A chemistry graduate student is given 450. mL of a 0.20M ammonia (NH,) solution. Ammonia is a weak…

A: GivenpH = 9.14pOH + pH = 14pOH + 9.14 = 14pOH = 4.86

Q: An analytical chemist is titrating 143.9 mL of a 0.6100M solution of acetic acid (HCH3CO₂) with a…

A: Given data : Concentration of HCH3CO2 = 0.6100 M Volume of HCH3CO2 = 143.9 mL Concentration of NaOH…

Q: A chemistry graduate student is given 100. mL of a 1.20M ammonia (NH solution. Ammonia is a weak…

A: 31 gm of NH4Br added to NH3 to make a buffer solution of desired pH.

Q: What concentration of NaF do you need to add to a 0.15M HF solution to get a buffer solution pH of…

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Q: A chemist titrates  160.0mL  of a  0.3384M  hydrobromic acid  HBr  solution with  0.6847M…

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Q: A 50.0 mL volume of 0.15 mol L-1HBr is titrated with 0.25 mol -1 KOH. Calculate the pH after the…

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Q: Which statement is FALSE for indicators? Indicators are chosen to change color as close to the end…

A: An indicator is a substance that changes its color in acidic and basic medium. An indicator could…

Q: What is the pH of a buffer 0.10M (Salt) Na2HPO4/0.15M (acid) NaH2PO4? [ Ka2 = 6.2x10-8]

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Q: A 20.00-ml sample contains 2.39 g of KHC, H,O,, known as KHP. This sample is used to standardize an…

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Q: One of the most important blood buffers is the carbonic acid / bicarbonate system (H2CO3 + HCO3-).…

A: The given equilibrium reaction is as follows: H2CO3  <--> H+ + HCO3- The initial number of…

Q: What are the components of the buffer solution when 0.20 mol H3PO4 is mixed with 0.30 mol of the…

A: Given statement is :  What are the components of the buffer solution when 0.20 mole H3PO4 is mixed…

Q: For the following question, select all that are true. The end point ( or equivalence point ) your…

A: During the titration of strong acid HCl and strong base NaOH, both are completely neutralized to…

Q: Mass of NaCl needed for 50.0 mL of 0.200 M NaCl solution. (Show calculation below.) Change in pH…

A: Since you have posted a question with multiple sub-parts, we will solve first three subparts for…

Q: The figure below is a graph of a sodium borate-boric acid buffer solution. Refer to the following…

A: Answer 2 : As the amount of base is increased it neutralize more amount of acid hence the…

Q: A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 MKOH. a) Calculate the pH at the…

A: (a)At equivalence point, moles of acid and base are equal.

Q: A 30.0-mL sample of 0.165 M propanoic acid is titrated with 0.300 MKOH. A) Calculate the pH at 0 mL…

A: Since we only answer up to 3 sub-parts, we’ll answer the first 3. Please resubmit the question and…

Q: Select any systems that could be used to buffer a solution at a pH of 6. Mark all appropriate…

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Q: 1. Which of the following aqueous solutions are good buffer systems? .  0.35 M ammonia + 0.31 M…

A: Hi, we are supposed to answer one question. To get the remaining questions solved please mention…

Q: Shown below is the titration curve for phosphoric acid. What is the composition of a solution of…

A: The question is based on the concept of titrations. we have to identify composition of phosphoric…

Q: iently basic solution, the carbonate ion does not react significantly with water to form hydrogen…

A: The CaCO3 exists in equililibrium with its ions as follows-CaCO3↔Ca+2+CO3-2Ksp=Ca+2CO3-2

Q: What are the components of the buffer solution when 0.40 mol H3PO4 is mixed with 0.50 mol of a…

A: Buffer solution: The solution that resists the change in pH is known as a buffer solution. The…

Q: A 25.0-mL sample of 0.50 M HCl is titrated with 0.50 M NaOH. What is the pH of the solution after…

A: pH of a solution is given by the equation: pH = -logH+

Q: a)  What is the pH of a buffer prepared by adding 0.506 mol of the weak acid HA to 0.507 mol of NaA…

A: the solution is as follows:

Q: Determine the pH of a carbonate buffer system that contains 0.0065 M of HCO3- and 0.0084 M of CO32-.…

A: Given :-  [HCO3-] = 0.0065 M  [CO32-] = 0.0084 M  Ka of HCO3- = 4.7x10-11  To calculate :-  pH of…

Q: 50.00 mL of an acetic acid solution is titrated with 0.1000 M NaOH. 23.90 mL NaOH is required to…

A: Given : Volume of acetic acid = 50 ml Volume of NaOH = 23.90 ml Molarity of NaOH = 0.1000M

Q: Buffer : HC₂0/C₂02- You are trying to create a pH 4.35 buffer using HC2O4- and C2O4-2. The Ka of…

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Q: For each combination of substances dissolved in water shown below, determine whether it forms or…

A: A buffer solution is an aqueous solution that consists of mixture of a weak acid and its conjugate…

Q: If you have a ka = 8.25x10^-8, what buffer system will you use? Acetic acid (HC2H302) - Acetate ion…

A: Given: Ka of acid = 8.25 × 10-8

Q: 120-mL buffer solution is prepared from 0.90 M HA (K, = 0.00029) and 0.90 M NaA. Calculate the pH…

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Q: A 50.0 mL solution of 0.139 M KOH is titrated with 0.278 M HC1. Calculate the pH of the solution…

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Q: Given two buffer solutions:       Buffer 1 : 0.200 M CH3COOH - 0.200 M NaCH3COO       Buffer 2 :…

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Q: A 50.0 mL of a 0.100 M ammonia (NH3) solution is titrated with 0.150 M HCl. The ka of ammonia is…

A: This problem can be solved through the concept of acid-base titration.

Q: Thymol blue is a unique indicator that has two set of color change, red to yellow near pH = 1.5 and…

A:

Q: Which of the following aqueous solutions are good buffer systems? 0.40 M nitrous acid + 0.21 M…

A: A buffer is a solution that with the inclusion of acidic or critical components will resist the pH…

Q: A 150.0 mL sample of 0.20 M HF is titrated with 0.10 M NaOH.  Determine the pH of the solution after…

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Q: 1. Explain how a buffer made of hydrofluoric acid (0.20M) and fluoride ion (0.20M) adjusts to a…

A: Buffer is solution which have tendency to resist pH change on addition of small amount of strong…

Q: What are the components of the buffer solution when 0.20 mol H3PO4 is mixed with 0.30 mol of the…

A: Here we have to choose the correct components of the buffer solution, when 0.2O mol H3PO4 is mixed…

Q: A sample of acetic acid is titrated with a standardized NaOH solution. Before the end-point of the…

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Q: 3. Write an appropriate indicator given the following equivalence points Equivalence Point pH 2 pH 4…

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Q: 25.0 mL sample of 0.30 M HCl is titrated with 0.30 M KOH. What is the pH of the solution after 5 mL…

A: According to the question, HCl reacts with KOH . We have: 25.0 ml of 0.30 M HCl and 0.30 M KOH. The…

Acid Base Titration

An acid-base titration is the method of quantitative analysis for determining the concentration of an acid and base by exactly neutralizing it with a standard solution of base or acid having known concentration.