A student prepares an 750.0 mL buffer solution with a pH of 4.85 by adding sodium acetate to a solution of acetic acid. However, they forgot to document the mass of NaC2H3O2 added to the beaker. Fortunatelly, they know that the concentration of HC2H3O2 is 0.235M. Determine the mass, in grams, of NaC2H3O2 that must have been added to the solution. (Molar Mass of NaC2H3O2=82.0343 g/mol)

Q: You make 1.00 L of a buffered solution (pH = 4.00) by mixing acetic acid and sodium acetate. You…

A: We have 1.0 M solution of HC₂H3O2 , and 1.0 M solution of NaC₂H3O2 (in other words, we have 1.0 M…

Q: An analytical chemist is titrating 226.9 mil. of a 0.5200M solution of benzoic acid (HC H,CO,) with…

A:

Q: Which of the following statements is FALSE? A) The limiting reactant is completely consumed in a…

A: Limiting reactant is the reactant species which limits the amount of product formed in a chemical…

Q: NOTE: The following 4 questions involve the titration of a 100.00 mL sample of 0.500 M methylamine,…

A: As per our guidelines we can only solve first question. Please resubmit other questions as next…

Q: An analytical chemist is titrating 242.9 mL of a 0.7800M solution of cyanic acid (HCNO) with a…

A: pH of resulting solution can be determine by the compound formed and the remaining or excess…

Q: An analytical chemist is titrating 185.4 mL of a 0.3800M solution of propionic acid (HC₂H5CO₂) with…

A: Given,  Molarity of propionic acid (HC2H5CO2 ) = 0.3800 M.  Volume of propionic acid (HC2H5CO2 ) =…

Q: An analytical chemist is titrating 247.8 mL of a 1.100M solution of acetic acid (HCH, CO₂) with a…

A:

Q: The active ingredient in aspirin is acetylsalicylic acid. A 2.08 g sample of acetylsalicylic acid…

A: Number of moles of acetylsalicylic acid and NaOH will be equal since one carboxylic acid group is…

Q: You need to make 1.0 L of a bu CH3COOH and NaCH3COO answers with reasonable ratio Ka for CH3COOH =…

A:

Q: An analytical chemist is titrating 223.5 mL of a 0.8500M solution of ammonia (NH3) with a 0.2900M…

A: First, we need to calculate the number of moles of NH3 and HClO. The number of moles is calculated…

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: An analytical chemist is titrating 158.1 mL of a 1.100M solution of benzoic acid (HC6H₂CO₂) with a…

A: The volume of the benzoic acid solution = The concentration of the benzoic acid solution = The…

Q: A student has a sample of 0.50 M lactic acid (HC3H5O3). She adds 10 mL of this solution to 40 mL of…

A: Given : Concentration of lactic acid = 0.50 M Volume of lactic acid solution used = 10 mL = 0.010 L…

Q: A 0.263 g sample of Na2CO3 requires 28.35 mL of HCl to completely react with it. What is the pH of…

A:

Q: An analytical chemist is titrating 211.6 mL of a 0.3800M solution of hydrazoic acid (HN,) with a…

A:

Q: An analytical chemist is titrating 213.8 mL of a 0.2800M solution of butanoic acid (HC3H,CO₂) with a…

A: Volume of butanoic acid, V1 = 213.8 mL = 0.2138 L ( 1L = 1000 mL) Concentration of butanoic acid, M1…

Q: An analytical chemist is titrating 178.1 mL of a 1.200M solution of hydrazoic acid (HN) with a…

A: Hydrazoic acid ( HN3 ) is a weak acid.NaOH is a strong base .the volume of HN3 = 178.1 mL = 0.1781…

Q: A buffer is made by dissolving 10.5 g of sodium dihydrogen phosphate, NaH2PO4 and 12.0 g disodium…

A:

Q: Determine the pH at the point in the titration of 40.0 mL of 0.200 M HC₄H₇O₂ with 0.100 M Sr(OH)₂…

A: Any acid/alkali's strength defines any solution's pH. The strong acid's presence with weak base…

Q: solution is prepared by mixing 500 mL of 0.1 M HNO3 with 500 mL of 0.1 M Ca(OH)2. What is the pH of…

A: We will calculate pH by the help of given information

Q: An analytical chemist is titrating 169.6 mL of a 0.4900M solution of acetic acid (HCH3CO₂) with a…

A: The question is based on the titrations.  we are titrating a weak acid with a strong base. we need…

Q: Phosphoric acid is a triprotic acid (Kal To find the pH of a buffer composed of H₂PO¯ (aq) and…

A: The Ka values for the phosphoric acid areThe phosphoric acid has the following ionizations  H3PO4 ⇌…

Q: Calculate the pH of a buffer solution made by mixing 300 mL of 0.3 M acetic acid, CH;COOH, and…

A: Given, a buffer solution is made by mixing 300 mL of 0.3 M acetic acidand 200 mL of 0.2 M of its…

Q: Calculate the pH of 70.0 mL of the buffer solution (0.10 M HC₂H3O2 and 0.20 M NaC₂H30₂) to which…

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

Q: An analytical chemist is titrating 226.3 mL of a 0.3900M solution of hydrazoic acid (HN3) with a…

A: The objective of the question is to calculate the pH of the acid solution after the addition of .It…

Q: A buffer solution is prepared by dissolving  1.300 g  of ammonium chloride (NH4Cl) into  100.00 mL…

A: Mass of ammonium chloride is 1.3 g. Molar mass of ammonium chloride is 53.491 g/mol.

Q: An analytical chemist is titrating 199.1 mL of a 0.7400M solution of hydrazoic acid (HN₂) with a…

A: Given,Molarity of hydrazoic acid ( HN3 ) = 0.7400 Mvolume of HN3 solution = 199.1 mLMolarity of KOH…

Q: A 100. mL sample of 0.10 M HCl is mixed with 50. mL of 0.14 M NH3. What is the resulting pH? (Kb for…

A:

Q: A 1.40 L buffer solution consists of 0.256 M propanoic acid and 0.105 M sodium propanoate. Calculate…

A: This is an acidic buffer solution.  Moles of propanoic acid = .256*1.4 = 0.3584  Moles of sodium…

Q: Assume you titrate 20.0 mL of 0.11 M NH3 with 0.10 M HCl.          (a)  What is the pH of the NH3…

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

Q: A solution is formed by adding 2.40 grams of solid barium cyanide, Ba(CN)2, to 200.0 ml of 0.130M…

A: Given: Mass of barium cyanide (Ba(CN)2) is 2.40 grams The volume of sodium cyanide (NaCN) is 200.0…

Q: An analytical chemist is titrating 145.8 mL of a 0.7500 M solution of propionic acid (HC₂H₂CO₂) with…

A:

Q: A buffer solution is prepared by dissolving  1.600 g  of ammonium chloride (NH4Cl) into  100.00 mL…

A:

Q: A solution NH3 that contains 78 mL of 0.043 M ammonia, NH 3, is titrated with 0.083 M HCI. The K₁ of…

A: Given,Molarity of NH3 = 0.043 Mvolume of NH3 = 78 mLMolarity of HCl = 0.083 MKb of NH3 = 1.8 x 10-5

Q: An analytical chemist is titrating 232.9 mL of a 0.2400M solution of cyanic acid (HCNO) with a 1.200…

A: Given titration is between weak acid, cyanic acid and strong base, KOH. Based on the moles of excess…

Q: What’s the PH=

A: Given that, 2.05 g of sodium acetate is dissolved in 85.0 mL of 0.10 M of acetic acid solution. The…

Q: solution is made by titrating 8.00 mmol (millimoles) of HA and 1.00 mmol of the strong base. What is…

A: The calculation is as follows:

Q: An analytical chemist is titrating 123.0 mL of a 0.1500M solution of dimethylamine ((CH3)₂NH) with a…

A: Dimethyl amine is a base , so when a solution is acid , HNO3 is added, they will react to form salt…

Q: n each of the following questions, assume that there is no volume change when HCl is added to water…

A: ANSWER : (a) Concentration of HCl = Concentration H+ = moles of HCl / Volume of solution = 0.091…

Q: You were asked to estimate the pH of a 15mL of 0.09N of HCl when 16.9mL of 0.085N NaOH is added to a…

A:

Q: Calculate the pH of the following buffer solutions:

A: a)Moles of KH2PO4 =2.668g/136gmol-1 =0.019617 mol Moles of K2HPO4=2.095g/174.2gmol-1 =0.0120264 mol…

Q: A buffer solution contains 0.476 M ammonium bromide and 0.339 M ammonia. If 0.0340 moles of…

A:

Q: A buffer is prepared by adding 20.0 g of sodium acetate(CH3COONa) to 500 mL of a 0.150 M acetic…

A: (a) Given, The initial concentration of acetic acid is 0.15 M The initial mass of sodium acetate…

Q: A solution is prepared by dissolving 35 millimoles of solid NaOH in 500.0 mL of 100 mM H2A. How is…

A: pH of a buffer solution is calculated using the following equation:  pH = pKa + log ([salt]/[acid])…

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.