ou are to prepare 100. mL of an acetate buffer of pH 5.00 using 1.0 M acetic acid (CH3CO2H, also written as HC2H3O2) and solid sodium acetate (NaC2H3O2). To prepare for the investigation, complete the following calculations. The pKa for HC2H3O2 is 4.74.     The Henderson-Hasselbach equation is pH = pKa + log ([conjugate base]/[acid])    (a) What ratio of [NaC2H3O2] to [CH3CO2H] is required for a pH = 5.00?   (b) You will want the concentrations relatively dilute, so use an acid concentration of 0.10 M. What volume of 1.0 M CH3CO2H would be needed to prepare 100. mL of buffer with the desired concentration of 0.10 M? Use M1V1 = M2V2  (c) Use the ratio from (a) and the concentration desired (discussed in (b)) to calculate how many grams of NaC2H3O2 · 3 H2O would be needed to prepare 100. mL of buffer if the acid concentration is 0.10 M?

Q: An analytical chemist is titrating 140.2 mL of a 0.5600M solution of isopropylamine ((CH3)2CHNH2)…

A: Step 1: 1. Calculate moles of isopropylamine initially:   Initial moles of isopropylamine=0.1402…

Q: buffer of pH = 7.5 is desired. Which two of the following compounds should be dissolved in water in…

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

Q: A0.1 M CH₂COOH solution is titrated with 0.1 M NaOH. At what point in the titration will the pH of…

A: During a titration of an acid with the base, the pH value changes as the concentration of the base…

Q: An analytical chemist is titrating 139.4 mL of a 0.7600M solution of isopropylamine ((CH3)₂CHNH₂)…

A: Volume of isopropyl amine solution=  139.4 mL  Molarity of isopropyl amine solution= 0.7600M…

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: nate (Na2CO3)corresponds to the following values: 0.53 M.   (Ka for HCO3− is 5.6 ×10−11.)  Report…

A: Ka = 5.6×10-11 pKa = -log(Ka)   = -log(5.6×10-11) = 10.25 1) As it is Acidic buffer,  pH = pKa +…

Q: Which

A: Those solution when resist to change the pH when small amount of acid or base added on it's then…

Q: The pH of a bicarbonate-carbonic acid buffer is 6.62. Calculate the ratio of the concentration of…

A: The question is based on the concept of chemical equilibrium. we need to calculate the required…

Q: A 1.40 L buffer solution consists of 0.182 M butanoic acid and 0.322 M sodium butanoate. Calculate…

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

Q: A 1.44 L buffer solution consists of 0.289 M propanoic acid and 0.189 M sodium propanoate. Calculate…

A: Solution contains weak acid and its salt of strong base. So this is buffer solution.On addition of…

Q: Calculate the amount of solid sodium acetate NaC 2 H 3 O 2 which must be added to 0.300 L of a 0.50…

A: The relation between the pH and the concentration of salt and acid is given by the…

Q: A chemist titrates 50.0 mL of a 0.4173M nitrous acid (HNO₂) solution with 0.2299 M KOH solution at…

A:

Q: A 1.44 L buffer solution consists of 0.323 M propanoic acid and 0.132 M sodium propanoate. Calculate…

A: pKa  = - log Ka            =  - log (1.34  * 10-5)          = 4.8729

Q: A chemist titrates 240.0 mL of a 0.4685M acetic acid (HCH3CO₂) solution with 0.3845 M NaOH solution…

A: The objective of the question is to calculate the  at the equivalence point.

Q: Determine the mass of solid NaCH₃COO that must be dissolved in an existing 500.0 mL solution of…

A: Given   The volume of CH3COOH solution is 500.0 mL. The molarity of CH3COOH solution is 0.200 M. The…

Q: A buffer is composed of 0.200 M (CH3)2NH (Kb = 5.9 × 10–4) and 0.250 M (CH3)2NH2NO3. What is the pH…

A: pKb  = - log Kb            =  - log (5.90  * 10-4 )          = 3.23pKa = 14-pKb       = 14- 3.23…

Q: A buffer is composed of 0.200 M (CH3)2NH (Kb = 5.9 × 10–4) and 0.250 M (CH3)2NH2NO3. What is the pH…

A: The given solution is a buffer solution composed of (CH3)2NH and (CH3)2NH2NO3. Molarity of (CH3)2NH…

Q: A 15.0 mL sample of 0.20 M of an unknown weak acid is titrated with 0.15 M NaOH at 25 oC. At 25 oC,…

A: Molarity of NaOH = 0.15 mol/LMolarity of weak acid = 0.20 mol/LpKa = 4.06

Q: The pH of a bicarbonate-carbonic acid buffer is 6.18. Calculate the ratio of the concentration of…

A: The ratio of [H2CO3] to that of [HCO3-] is determined by using Henderson-Hasselbalch equation.

Q: If you wanted to prepare a buffer with a pH pf 7.25, which acid would be the best choice?…

A: A buffer solution is a type of aqueous solution that resists changes in its pH level when small…

Q: How many grams of dry NH4 Cl need to be added to 2.10 L of a 0.100 M solution of ammonia, NH3, to…

A: Given: Volume of ammonia solution  = 2.10 L Molarity of ammonia solution = 0.100 M pH of buffer…

Q: A solution is formed by adding 6.00 grams of solid potassium acetate, KC₂H₃O₂, to 200.0 ml of…

A: Answer: Basic nature of the solution will be the outcome of the hydrolysis of acetate ion which will…

Q: What is the pH of a buffer solution if you dissolve 300 ml of 1.65M Formic Acid (HCO2H) and 250 ml…

A: Given -> Volume of formic acid = 300 ml  Molarity of formic acid  = 1.65 M = M1 Volume of sodium…

Q: You prepare a buffer by mixing 0.15 mol propanoic acid (pKa = 4.87) and 0.25 mol sodium propionate.…

A: Mole of propanoic acid = 0.15 molMole of sodium propionate = 0.25 molpKa = 4.87 Mole of NaOH = 0.025…

Q: I want to make a buffer solution containing 1 M glycene pH = 10 (Na+), 1 mM ZnCl2 , 1 mM NaOH. I…

A: In the given question we have to calculate the volume of each solution that is present in the…

Q: Answer the following questions with respect to a buffer solution containing 1.00 L of 0.150 M acetic…

A: PH is defined as the negative logarithm of the H+ ion concentration. The buffer solution is the…

Q: We are looking for the molar mass and the pKa value of a weak monoprotonic acid. Two experimentswere…

A:

Q: A 1.0-L buffer solution contains 0.100 mol HC2H3O2 and 0.100 mol NaC2H3O2. The value of Ka for…

A: pH = pKa + log [NaC2H3O2]/[HC2H3O2] pKa = -log Ka Number of mol = Molarity x Volume (L)

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.