Concordia University Buffers Solubility and KSP Worksheet I have chemistry questions I need help with, the questions about buffers, and solubility and Ksp. | Course Hero

Concordia University Buffers Solubility and KSP Worksheet I have chemistry questions I need help with, the questions about buffers, and solubility and Ksp.please make the answer and steps clear.you can review the questions on the files. #28
The following problem will be used for the next three questions.
Suppose a buffer is prepared at a pH = 3.75 by mixing 150 mL of 0.271 M HF with sodium
fluoride (NaF). How much sodium fluoride is needed (in grams) to prepare the buffer? The Ka of
HF is 7.2×10-4. Assume the molar mass of NaF is 41.99 g/mol
Question 1
Use the Henderson – Hasselbach equation to calculate the ratio of NaF to HF. In other words,
solve the Henderson Hasselbach equation for: [NaF]/[HF] or [F?]/[HF].
Report your answer to 2 decimal places.
Question 2
Next, use your answer to Question 1 to solve for the moles of NaF (or F-). Report your answer
to 3 decimal places and do not include units.
Question 3
Next, calculate the mass of NaF required to prepare the buffer solution.
Report your answer to 2 decimal places and do not include units.
____________________________________________________________________________
The next four questions will be based on the following:
Suppose a buffer is prepared at a pH = 3.75 by mixing 125 mL of 0.150 M HF with 0.10 M
sodium hydroxide. How much sodium hydroxide is needed (in moles and mL) to prepare the
buffer? Assume Ka of HF is 7.2×10-4.
Question 4
The reaction that occurs to form the buffer is:
HF +NaOH? NaF +H2O
Generate a RICE table to describe the change in moles between HF and NaOH during the
reaction. Use the table to describe the change in moles of each species in terms of x, the moles
of sodium hydroxide added. Report the expressions for the equilibrium concentrations in the
blanks below.
In blank # 1: Report the expression for the equilibrium concentration for HF.
In blank # 2: Report the expression for the equilibrium concentration for NaOH.
In blank # 3: Report the expression for the equilibrium concentration for NaF.
For any number greater than 0, use 4 significant figures in decimal notation. For example, if the
expression is 0.152342-x, type 0.1523-x. Do not include spaces or units. Be sure to include the
leading zero too. If your answer is 0, then type 0.
Blank # 1
Blank # 2
Blank # 3
Question 5
Next, use the Henderson – Hasselbach equation to calculate the ratio of NaF to HF. In other
words, solve the Henderson Hasselbach equation for: [NaF]/[HF] or [F?]/[HF].
Report your answer to 2 decimal places.
Question 6
Next, solve for x, the moles of NaOH added to create the buffer.
Report your answer with 3 significant figures using scientific notation, using the E notation. For
example, if your answer is 0.00100, then type 1.00E^-3. Do not include units.
Question 7
Next, use the calculated moles to solve for the volume of 0.10 M NaOH that is added. Report
your answer in milliliters with 2 significant figures and without units.
EX-Question
A 52.00 mL 0.0850 M NaOH solution is titrated with 0.0750 M HCl. Meaning NaOH is the
analyte and HCl is the titrant.
In blank # 1: Calculate the initial pH.
In blank # 2: Calculate the pH after 25.00 mL of HCl are added.
In blank # 3: Calculate the pH at the equivalence point.
In blank # 4: Calculate the pH after 75.00 mL of HCl are added.
Report your answers to 2 decimal places.
Blank # 1
Blank # 2
Blank # 3
Blank # 4
Ex-Question
A 40.00 mL 0.250 M NH3 solution is titrated with 0.100 M HCl. Meaning ammonia is the analyte
and HCl is the titrant. The Kb of NH3 is 1.8×10-5.
In blank # 1: Calculate the initial pH.
In blank # 2: Calculate the pH after 15.00 mL of HCl have been added.
In blank #3: Calculate the volume of HCl required to reach the equivalence point.
In blank #4: Calculate the pH at the equivalence point.
Report your answers to 2 decimal places. Do not include units.
Blank # 1
Blank # 2
Blank # 3
Blank # 4
31-Ex-Question
The Ksp for Ag2CO3 is 8.1×10-12, respectively. calculate the solubility (solve for x) for Ag2CO3.
Report your answers to 2 significant figures using scientific notation. Use the E notation. For
example, 0.0010 should be written as 1.0E-3.
31-Ex-Question
Rank the following salts from most soluble (1) to least soluble (4).
silver carbonate
nickel (II) carbonate
silver chloride
calcium fluoride
31-Ex-Question
Which of the following solids will be less soluble in a solution that is buffered at pH = 12.00 than
in pure water?
a. AgF
b. AgBr
c. AgCl
d. AgOH
e. AgNO3

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