how many liters of 0.54 monoprotic acid should be added to 685000 L of water with ph 7 to reach ph to 5.2? ka = 7.1 * 10-4

Q: What is the pH of a solution that contains 0.12 M HC2H3O2 and 0.29 M C2H3O2? Use Kb = 5.6 x 10-10…

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Q: What volume of 0.120 M NaOH must be added to 100 mL of 0.100 M NaHC204 to reach a pH of 4.70? H2C204…

A: The solution is given below -

Q: How many grams of NaIO (Kb (IO-)=5x10-4 ; MW=213.9 g/mole) must be added to 40.0 ml of 0.1 M HCl to…

A: pOH = pKb + log [NaIO]/[HOI] pH = 14 - pOH

Q: A 101.3 mL sample of 0.090 M HCl is mixed with 41.0 mL of 0.090 M NH3.  What is the resulting pH?…

A: Given that

Q: Mass of NaCl needed for 50.0 mL of 0.200 M NaCl (Show calculation below.) utiön 50.OMLX1000 =0.05…

A: Only the last column i.e the pH change after addition of base is given

Q: What is the pH of 25.00 mL buffer solution which is 2.00M in HC2H3O2 and 2.00M in NaC2H3O2? Ka =…

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Q: that is 0.192 M in lactic acid and 0.155 M in sodium lactate? The Kaof lactic acid is 1.4 × 10-4.…

A: Buffer is the solution of mixture of weak acid/weak base with its salt of strong base/strong acid

Q: A litre of solution containing 0.1 mol of CH3COOH and 0.1mole of CH3COONa provided buffer of pH…

A: Given : Moles of CH3COOH taken = 0.1 mol. Moles of CH3COONa taken = 0.1 mol. And moles of NaOH added…

Q: What concentration of sodium benzoate must be used to create a buffer solution with a pH of 5.63 if…

A: Use a udic buffer equation to get MOLARITY of sodium benzoate. Buffer mixture is defined as an…

Q: How many grams of sodium fluoride should be added to 612 mL solution of hydrofluoric acid (Ka =…

A: Here there are two questions. According to Q&A guidelines of Bartleby, I am allowed to answer…

Q: ) How many moles of BHCl (acidic salt) would need to be added to 452 mL of 1.66 M B (a weak base) to…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: What is the pH of 500 mL of water after the addition of 1 mL of 2M NaOH? HINT: you cannot use H-H…

A: A solution that resist any change in the pH is called a buffer solution. The pH of a buffer solution…

Q: A chemist named Ed Sheerin titrates X mL of a 0.5379 M butanoic acid (HA) solution with 0.581 M…

A: Number of moles of butanoic acid = 0.5379 × 0.001X = 0.0005379X mol At equivalence point, number of…

Q: 1. A 0.0722 M solution of a weak acid has a pH of 3.11. Calculate the Ka of this acid.. х 10-6 2. A…

A:

Q: Anilinium chloride (C6H5NH3Cl) is a weak acid (Ka = 2.4 x 10-5). A sample of anilinium chloride…

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

Q: 11. What equation or expression would be used to calculate the pH of a solution prepared by…

A: Given : moles of weak acid i.e benzoic acid = 0.280 mol And moles of conjugate base salt of weak…

Q: 22.5 mL of a 0.200 M HBr solution was added to a 50.00 mL sample of 0.250 M Sodium benzoate…

A: Molarity of HBr is 0.200 M. Volume of HBr is 22.5 mL. Molarity of sodium benzoate is 0.250 M. Volume…

Q: What is the pH of a buffer system prepared by dissolving 10.70 grams of NH4Cl and 20.00 mL of 12 M…

A: Mass of NH4Cl = 10.70 g  Molarity of NH3 = 12 M Volume of NH3 = 20 mL = 0.020 L  Volume of buffer…

Q: What is the pH of a solution prepared by mixing 30.00 mL of 0.10 M CH 3CO 2H with 30.00 mL of 0.030…

A: The question is based on the concept of titrations.   we are titrating  a weak acetic acid with a…

Q: At 40.°C the value of Kw is 2.92 x 10-14 a. Calculate the H] and [OH ] in pure water at 40.°C. [H*]…

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Q: What is the pH of 50.00 mL buffer solution which is 2.00M in HC2H3O2 and 2.00M in NaC2H3O2? Ka =…

A:

Q: Ka for benzoic acid, c6h5cooh, 6.5x10^-5. Calculate the pH of solution after addition of the…

A: a) The pH of 10mL of 0.10 M NaOH to 40mL of 0.10 M benzoic acid

Q: 5 mL acid mixture with a concentration of HCl 0.12 M and a weak acid HA (Ka = 1x10-14) concentration…

A: The acid gives hydrogen ions in the solution,while the base gives hydroxide ions in the…

Q: How many grams of BHCl(acidic salt , 69.83g/mol

A: We have to find the mass of BHCl

Q: What is the percent ionization of acetic acid (CH3COOH) in a solution that contains 0.10 M acetic…

A: Ionic solids are metal salts. They formed when metals form an ionic bond with non-metals. Ionic…

Q: What is the pH of a 500.00 mL buffer containing 0.350 moles of HCO2H and 0.400 moles of HCO2Na? (Ka…

A:

Q: Question attached

A: The pH value of the buffer solution is based on the pKa values of the acid When the pKa value of the…

Q: 1. The Ka for benzoic acid is 6.5 x 10-5. Calculate the pH of a 0.10 M benzoic acid solution. . 2. A…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: What is the pH of a solution containing 1.50 M Acetic acid (CH3COOH) (Ka = 1.8 X 10-5) and 2.5 M…

A: Solution, which resist in pH change value upon addition of small amount of strong acid or base (less…

Q: Ka for benzoic acid, c6h5cooh, 6.5x10^-5. Calculate the pH of solution after addition of the…

A: a. The balanced equation for this reaction is given as,

Q: . The acetate buffer contains 0.200 M acetic acid and 0.0500 M sodium acetate. Given that the Ka of…

A: PH of buffer solution is calculated by using Henderson Hasselbalch equation

Q: What volume of 1.50 M NaOH must be added to 200.0 mL of 1.00 M glycolic acid (HC2H3O3) to produce a…

A: We have to calculate the volume of base needed.

Q: 10-13. How many milliliters of 0.202 M NaOH should be added to 25.0 mL of 0.023 3 M salicylic acid…

A: We know that  pH of buffer is  pH = pka + log {[salt] / [ acid]}

Q: What is the pH of a solution created by mixing 25.00 mL of 0.10 M formic acid and 25.00 mL of 0.10 M…

A:

Q: 1.)  What is the molar solubility of a hypothetical compound AB in pure water given a Ksp = 6.4 x…

A: 1) Given that: Ksp = 6.4 × 10-2 Molar solubility = ?

Q: Hydroxylamine HONH2 readily forms salts such as hydroxylamine hydrochloride which are used as…

A:

Q: What is the pH of the sodium lactate solution? C3H5O3 + H₂O = HC3H5O3 + OH- [C3H5O3] = 3.22 × 10-¹ M…

A:

Q: What volumes of 0.50 M HNO2 and 0.50 M NaNO2 must be mixed to prepare 1.00 L of a solution buffered…

A:

Q: Find the pH of a 1L buffer solution that is 0.600 M HC2H3O2 (aq) solution and 0.700 M Na C2H3O2 (aq)…

A: Buffer solution is made from a weak acid and the conjugate base of the acid.  Now,  pH of such…

Q: The titration curve as shown is for the titration of 25.00 mL of 0.100 M CH3CO2H with 0.100 M NaOH.…

A: We are authorized to answer three subparts at a time, since you have not mentioned which part you…

Q: Aniline, the molecule pictured above, is 0.125 M with a volume of 350 mL and is titrated with 0.250…

A: Given data,Molarity of aniline=0.125MVolume of aniline=300mLMolarity of HBr=0.250MKb of…

Q: Propanoic acid has a Ka=1.3x10-5. The titration starts with 40.00 mL of 0.1000 M propanoic acid…

A: Titration is a quantitative analysis in which the concentration of unknown solution can be find by…

Q: Suppose you have 150 mL of a buffer containing 0.100 M acetic acid and 0.0500 M sodium acetate.…

A:

Q: Which of these procedures would not make a pH =4.75buffer?(a)  Mix 50.0 mL of 0.10 M acetic acid and…

A: A buffer is a solution which by virtue of the ionic equilibria present in the solution and it can…

Q: = H+ + HPO;- Ka = 6.2 x 10-8 = H+ + SO?- Ka = 1.3 x 10-2 From the systems above, identify the…

A: The question is based on the concept of buffer solution.   A buffer is a solution which resist any…

Q: 0-5 HCN               Ka = 4.9 X 10-10                      HClO2             Ka = 1.1 X 10-2 The…

A: Buffer range is the range of pH which is used for the determination of the working of buffer…

Q: An aqueous solution has [HC7H5O2] = 0.100 M and [Ca(C7H5O2)2] = 0.200 M. Ka= 6.3 × 10-5for HC7H5O2.…

A: We have to find the pH

Q: The pH of 0.010 M trimethylamine is 10.88. What is the value of Kb for this base? 1.3 * 10-11…

A: we have given that   Concentration of trimethylamine = 0.010M pH = 10.88 pOH = 3.12   (CH3)3N   +…

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.