A student prepared a 1:1 buffer, for which [HAc] = [Ac-] = 0.05182 M. Using their 1:1 buffer and a 0.10229 M HCl solution, the student prepared Solution C in Part 3 of the experimental procedure. Given this information, how many moles of Ac- were there in the student's Solution C after a reaction took place? Report your final answer, in moles, to 6 decimal places and only include the numerical value (no units). Solution C contains 20mL of buffer and 5mL of HCl.

A student prepared a 1:1 buffer, for which [HAc] = [Ac-] = 0.05182 M. Using their 1:1 buffer and a 0.10229 M HCl solution, the student prepared Solution C in Part 3 of the experimental procedure. Given this information, how many moles of Ac- were there in the student's Solution C after a reaction took place? Report your final answer, in moles, to 6 decimal places and only include the numerical value (no units). Solution C contains 20mL of buffer and 5mL of HCl.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter15: Additional Aqueous Equilibria

Section: Chapter Questions

Problem 111QRT: Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong...

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Consider the nanoscale-level representations for Question 111 of the titration of the aqueous strong acid HA with aqueous NaOH, the titrant. Water molecules and Na+ ions are omitted for clarity. Which diagram corresponds to the situation: (a) After a very small volume of titrant has been added to the initial HA solution? (b) Halfway to the equivalence point? (c) When enough titrant has been added to take the solution just past the equivalence point? (d) At the equivalence point? Nanoscale representations for Question 111.
In a laboratory experiment, a student has 1 L of solution containing a weak base at a concentration of 0.300 M. In order to create a buffer, a strong acid is added, which converts some of the base in the solution to its conjugate weak acid to create a buffer. If the student wants to create the most effective buffer that can be equally resistant to both acids and bases how many moles of strong acid should the student add to the buffer? (Please provide your answer to 3 decimal places.)
The recipe of carbonate buffer is as follows: 15mM sodium carbonate Na2CO3 35mM sodium bicarbonate NaHCO3 3.1mM sodium azide NaN3 (poisonous) You want to make 500mL of this buffer for your upcoming experiments. However, you don’t have enough stock solution of each to make this buffer. Instead of preparing more of each stock you decide to just weight out and mix crystals/powder of each with water. Show your calculations on how much crystals (in grams) of each you should weight out. [Atomic Mass: Na – 23; C – 12; N – 14; O – 16]
A weak acid- strong base titration was performed as follows: 10.00 mL of 0.10 M acetic acid were collected in an Erlenmeyer flask, and then diluted to 100 mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100 M NaOH. The titration was started by slowly adding NaOH to acetic acid. (Note: The volume of two drops indicator is ignored as it is so tiny compared with 100 mL.) What is the pH of the solution in the Erlenmeyer flask after adding 10.00 ml of 0.100M NaOH? Select one:a. 8.35b. 6.9c. 7.22d. 7.00
A weak acid- strong base titration was performed as follows: 10.00 mL of 0.10 M acetic acid were collected in an Erlenmeyer flask, and then diluted to 100 mL with distilled water. After that, two drops of indicator were added. Then, the buret was filled with 0.100 M NaOH. The titration was started by slowly adding NaOH to acetic acid. (Note: The volume of two drops indicator is ignored as it is so tiny compared with 100 mL.) What is the pH of the diluted acid in the flask before adding NaOH? Select one:a. All options are incorrectb. 4.90c. 5.30d. 3.1e. 5.15
110.0 mL buffer solution is 0.110 molL−1 in NH3 and 0.135 molL−1 in NH4Br. What mass of HCl will this buffer neutralize before the pH falls below 8.70? (Kb(NH3)=1.76×10−5) Express the mass in grams to two significant figures
In this experiment, you will determine the amount (percent) of potassium hydrogen phthalate (KHP) that is in an impure sample. You will determine the percent of KHP via titration using NaOH with known molarity. The reaction will follow, KHC8H4O4 (aq) + NaOH (aq) ---------> KNaC8H4O4 (aq) + H2O (l) At the endpoint, the moles of KHP will equal the moles of NaOH. You will use phenolphthalein as the indicator. The endpoint of the reaction will be a light pink solution color. How will you know the reaction is over? About how much KHP will be used in the titration? Which 3 substances go into the 250 mL Erlenmeyer flask for the titration? What is the mole to mole ratio in the reaction of KHP and NaOH? What solution goes into the buret?
1. A 200 ml buffer solution contains 36.342 μg Tris and 23.376 µg NaCl, respectively.Determine the molarities in micromolar (μM) of the above mentioned compounds in thebuffer solution. [Mw Tris = 121.14 g/mol and Mw NaCl = 58.44 g/mol] 2. What volume of cefoxitin (50 mg/ml) should be added to 500 ml of tryptone soya brothto yield a solution with a final concentration of 8 µg/ml?
A student conducting this experiment measures out 0.913 g of an unknown monoprotic weak acid and dissolves it in 110 mL of water. After adding an indicator, the student titrates the weak acid with 15.55 mL of 0.380 M NaOH to reach the equivalence point. What is the molar mass of the unknown acid?
In a titration of 20.37 mL of 0.1773 M H2SO4, 35.89 mL of a NaOH solution are needed. What is the concentration (in mol/L) of the NaOH solution? Include only the numerical answer (no units). In carrying out the first standardization in this experiment, a student used 0.5067 g of potassium hydrogen phthalate (KHP) and 24.97 mL of a NaOH solution are needed to reach the equivalence point. What is the concentration (in mol/L) of the student's NaOH solution? Include only the numerical answer (no units).
1. A solution of HCl is prepared by an unknown dilution of concentrated HCl. It is standardized by titrating 0.2897 grams of dried primary standard Na2CO3 with 54.76 mL acid, 0.2475 g Na2CO3 with 53.46 mL acid, and 0.2279 g Na2CO3 with 55.12 mL acid. Calculate the mean molar concentration of the HCl solution. 2. a) What is the uncertainty in the molarity in the previous problem determined by the propagation of typical uncertainties: emass = ±0.0002 g and evolume = ±0.02 mL? (You may use any one trial from Problem 2 to illustrate the propagation). b) What is the uncertainty in molarity in the previous problem if we take the uncertainty to be the standard deviation? c) For what reason(s) are the answers to B and A different? What is the cause of the difference?
The answers to the questions are already given. Please show the solution how to get the answers. A solution containing 0.5 mM CO32- and 2.5 mM F- is to be separated using Mg(NO3)2 as precipitating agent. Ksp of MgCO3=3.5x10-8. Ksp of MgF2=3.7x10-8. Which ion will precipitate first? Answer: CO32- How much of the first ion (in M) will be left when the second ion starts to precipitate? 5.91x10-6 M