How many grams of sodium lactate, NaC3H5O3, should be added to 1.00L of 0.150M lactic acid, HC3H5O3, to form a buffer of pH = 3.90?                                  C = 12     H = 1     O = 16     KaHLac =  1.4x10-4

Q: What is the molar solubility of Agl Ksp= 8.3 x 10^-17 in the presence of 0.05 M KNO3? A. 1.29x10^-16…

A: Molarity of KNO3 = 0.05M KNO3 is a strong electrolyte and dissociates completely to furnish ions.…

Q: Two solutions of an unknown slightly soluble salt, A(OH)2, were allowed to equilibrate—one at 25 °C…

A: Given: Volume of A(OH)2 =15 mL Concentration of HCl = 0.20 M At 25oC Volume of HCl =6.37 mL At 80oC…

Q: What is the pH of the buffer solution that contains 1.6 g of NH4Cl in 250 mL of 0.060 M NH3? Is the…

A: pH of a basic buffer can be calculated using Henderson-Hasselbach equation: pH=14-(pKb+logB+BOH)

Q: Calculate the pH for a buffer that is 0.050 M benzoic acid and 0.150 M sodium benzoate. The Ka for…

A: The pH of buffer solution can be calculated by using Henderson Hesselbach equation - pH = pKa + log…

Q: Find the pH of a buffer that consists of 1.3 M sodium phenolate (C6H5ONa) and 1.2 M phenol (C6H5OH)…

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Q: What are the molar concentrations of acetic acid (CH,COOH) and sodium acetate (CH, COONA) in an…

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Q: A buffer is prepared such that [CH3COOH]0 = [CH3COO−]0 = 0.050 M. Calculate the volume of 0.10 M…

A: Buffer capacity is used to determine the buffer solutions resistance to changes in pH when a strong…

Q: What are the [H3O+] and the pH of a propanoic acid– propanoate buffer that consists of 0.35 M…

A: Given Values:

Q: What is the PH of a buffer system that is 0.200 M hydrocyanic acid (HCN) and 0.120 M sodium cyanide…

A: Given: The concentration of acid, [HCN]= 0.200 M The concentration of salt, [NaCN]=0.120 M…

Q: Consider the reaction of a 20.0 mL of 0.220 M C̟H̟NHCI (Ka = 5.9 x 10*) with 12.0 mL of 0.241 M…

A: Given molarity of C5H5NHCl or C5H5NH+ = 0.220 M  Volume of C5H5NHCl solution = 20.0 mL = 0.020 L…

Q: How many grams of sodium hypochlorite, NACIO, need to be added to 227 mL of a 0.185 M solution of…

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Q: grams

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Q: The half-equivalence point of a titration occurs half way to the equivalence point, where half of…

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Q: A benzoic acid-sodium benzoate buffer is prepared by dissolving a certain amount of sodium benzoate,…

A: A buffer solution is an aqueous solution. It consist of a mixture of a weak acid and its conjugate…

Q: . What is the pH of a buffer prepared by adding 0.405 mol of the weak acid HA to 0.507 mol of NaA in…

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Q: 2) How many grams of NaOH should be mixed with 5.4 g of oxalic acid (H,C.O.) and completed to 100 ml…

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Q: Calculate the molar solubility of Hg₂C₂O₄(Kₛₚ=1.75X10⁻¹³) in 0.13 M Hg₂(NO₃)₂.

A: Introduction: The solubility (molar solubility) of a solid is the concentration of the "dissolved…

Q: You are given a 40.0mL sample of 0.80M CH3CH2COOH is titrated with 0.30M NaOH.  What is the pH of…

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Q: What mass (in g) of sodium formate, HCOONa, must be added to 10.0 L of a 0.483 M aqueous solution of…

A: Here, we have to find the mass of sodium formate that must be added to 10.0 L of a 0.483 M aqueous…

Q: How much solid sodium acetate (CH3COONa) is needed to prepare a buffer solution at ph 5 if you have…

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Q: A buffer solution contains 0.384 M KHCO3 and 0.239 M Na₂CO3. If 0.0464 moles of potassium hydroxide…

A: The constituents of the buffer solution are: conjugate base, [Na2CO3(aq)] = [CO32-(aq)] = 0.239 M…

Q: Consider a buffer made by adding 32.7 g of (CH₃)₂NH₂I to 250.0 mL of 1.42 M (CH₃)₂NH (Kb = 5.4 x…

A: Number of Mole- Ratio of given mass of substance to the molar mass of substance is called number of…

Q: Pls help ASAP.

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Q: What mass (in grams) of sodium acetate (CH3COONa) must be added to 100.00 mL of a 0.127 M solution…

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Q: Consider the reaction of a 20.0 mL of 0.220 M C₅H₅NHCl (Ka = 5.9 x 10⁻⁶) with 12.0 mL of 0.241 M…

A: When CsOH ( a base ) is added to C5H5NHCl ,  It will act as an acid and lose H+ ions and give its…

Q: From the following choose the most appropriate weak base (when added to its conjugate acid) for…

A: Solution

Q: You are making a buffer solution in the lab by combining the weak acid H2PO4- with its conjugate…

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Q: How many grams of NaH2C6H5O7 must be added to a 300 mL solution of 0.15 M H3C6H507 (Ka= 3.2x 10) to…

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Q: What are the [H₃O⁺] and the pH of a propanoic acid–propanoate buffer that consists of 0.35 M…

A: First of all write the  equation for given compound: CH3CH2COONa→CH3CH2COO-+Na+ CH3CH2OOH=0.15…

Q: A buffer solution contains 0.200 M CH3NH2 and 0.250 M CH3NH3Cl. What is the pH of the buffer…

A: The number of moles of methylamine in 50 mL buffer solution is calculated as follows:

Q: Consider a buffer made by adding 52.3 g of (CH3),NH2I to 250.0mL of 1.42 M (CH3)¿NH (Kb = 5.4 x…

A: The concentration or Molarity of salt is calculated by - M = w×1000/m×V Here, M = Molarity of Salt,…

Q: 6. What is the pH of a mixture of 5 ml of 0.1 mol/litre sodium acetate and 4 ml of 0.1 mol/litre…

A: Solution: In this problem we will calculate pH using henderson equation.

Q: suitable

A: Buffer solution worked at pH =  pKa-1 to pKa +1  Here pH = 7.0 then range should be 6 to 8 at this…

Q: How many mL of 1.0 M NaOH must be added to 100. mL of 0.050 M HC2H3O2 to make a buffer with a pH =…

A: We have given that pH = 5.0 Ka = 1.8×10-5 Pka = -log(1.8×10-5) = 4.74 Concentration of Acetic Acid =…

Q: a) Calculate the pH of a buffer system made up of 0.25 M C6H5COOH and 0.35 M C6H5C00NA. b)What is…

A: a) pKa of acetic acid = 4.75 As per Henderson Hasselbalch equation; pH = pKa + log [salt]/ [acid]…

Q: The half-equivalence point of a titration occurs half way to the equivalence point, where half of…

A: In this question, we will determine the pH of the solution at half - equivalence point.  You can see…

Q: A phenol/phenolate buffer was made up by mixing 0.0125 mol of phenol (C6H5OH) and 0.0135 m of…

A: Given : Moles of phenol = 0.0125 mol Moles of phenolate = 0.0135 mol Volume of buffer = 500 mL = 500…

Q: Calculate the pH of a buffer system containing 0.280 M NH3 and 0.430 M NH4Cl at 298.15K…

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Q: A volume of 500.0 mL of 0.180 M NaOH is added to 545 mL of 0.250 M weak acid (K, = 6.39 x 105). What…

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Q: What mass (in g) of ammonium chloride (NH4Cl) should be added to 2.60 L of a 0.155 M NH3 to obtain a…

A: Buffer solution is made of weak acid or base and their corresponding conjugate base or acid…

Q: What mass of sodium glycolate (98.03 g/mol) must be added to 300.0 mL of 1.00 M glycolic acid…

A: Given: pH of the buffer = 4.00 Ka of glycolic acid = 4.48×10-4 Molarity of glycolic = 1.00 M Volume…

Q: The buffer capacity of a solution may be defined as the number of moles of H+ that will change the…

A: Given Ka, find pKa as pKa = -log (Ka) = -log (1.8 x 10-5) = 4.74. Find the pH of the buffer by using…

Q: Determine the pH of a buffer solution containing 0.451 M benzoic acid (C6H5COOH) and 0.317 M sodium…

A: GivenC6H5COOH = 0.451 MC6H5COONa = 0.317 MKa = 6.3 * 10-5pKa = -log KapKa = -log (6.3 * 10-5)pKa =…

Q: Consider the following buffer system: 0.96 M H2CO3 and 1.08 M HCO3-. What is the pH of such a system…

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Q: What mass of sodium benzoate should you add to 158.0 mL of a 0.16 MM benzoic acid (HC7H5O2) solution…

A: Given, pH = 4.29 Ka of benzoic acid = 6.5 × 10-5

Q: How many grams of solid sodium fluoride should be added to 0.500 L of a 9.49x10-2 M hydrofluoric…

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Q: What is the pH of a buffer solution made by adding 0.41 g of NaC2H3O2 to 100. mL of 0.10 M HC2H302?…

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Q: The half-equivalence point of a titration occurs half way to the equivalence point, where half of…

A: Given that, Number of moles of monoprotic weak acid = 0.34 moles Ka of monoprotic weak acid =…

Q: How many grams of NH4CI would have to be added to 250.0 mL of a 0.420 M NH3 solution to prepare a…

A: The minimum concentration of NH4Cl that must be present in the solution to have a pH of 10 is;…

Q: Twenty-five mL of 0.100 M lactic acid (K, = 1.4 x 10) is titrated with 0.097 M KOH. %3! a) What is…

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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.