pH Measurement and Buffer Prep

LAB 6

PH MEASUREMENT AND BUFFER PREPARATION

DISCUSSED BY: PROF. JOHN LORENCE A. VILLAMIN

Multiple Choice

1. What does the pH value represent in an aqueous solution?

• The concentration of hydroxide ions (OH-)

• The concentration of hydrogen ions (H+)

• The concentration of oxygen ions (O2-)

• A)The concentration of sodium ions (Na+)

Multiple Choice

2. A solution has a pH of 4.5. What does this pH valueindicate about the solution?

• The solution is acidic.
• The solution is alkaline.
• The solution is basic.
• The solution is neutral.

Multiple Choice

3. A solution has a pH of 9. What can be inferred about thenature of this solution?

• The solution is neutral.
• The solution is a strong acid.
• The solution is acidic.
• The solution is basic.

Multiple Choice

4. What  does  the  term  "pOH"  represent  in  a solution?

• The concentration of hydroxide ions (OH-)

• The concentration of hydrogen ions (H+)

• The concentration of oxygen ions (O2-)

• A)The concentration of sodium ions (Na+)

Multiple Choice

According  to  the  definition,  how  are  acids  and  bases distinguished  based  on  their  behavior  in  aqueous solutions?

• Acids decrease H+ concentration; bases decrease OH- concentration.
• Acids and bases do not affect H+ or OH- concentrations in solutions.
• Acids increase OH- concentration; bases decrease H+ concentration.
• Acids increase H+ concentration; bases increase OH- concentration in aqueous solutions.

Multiple Choice

In the given rationale of conjugate base-acid pairing, why is HCl considered an acid?

• HCl is an acid because it donates protons (H+) in solution.
• HCl is an acid because it has a high pH.
• HCl is an acid due to its strong ionic bonds.
• HCl is an acid because it absorbs protons in solution.

Multiple Choice

According to the rationale, what is the conjugated base of HCl?

• HClO
• Cl2
• H2Cl
• Cl-

Multiple Choice

The difference between the definition of Lewis and Bronsted-Lowry in Acid and Bases is:

• Lewis acids are defined by proton transfer, while Bronsted-Lowry acids are defined by electron transfer.
• Bronsted-Lowry bases accept electrons, while Lewis bases donate protons.
• Lewis acids and bases are defined by electron transfer, while Bronsted-Lowry acids and bases are defined by proton transfer.
• Lewis bases are defined by proton transfer, while Bronsted-Lowry acids are defined by electron transfer.

Open Ended

What is the H+ concentration of a solution of a solution with a pH of 5.4

Open Ended

What is the pOH value of a solution with a pH of 8.4

Open Ended

How about the OH- concentration?

Multiple Choice

All are the common errors in measuring pH using pH Meter, EXCEPT:

• Using a pH meter with a dead battery
• Measuring pH in a dirty container
• Ignoring temperature effects on pH readings
• Using a properly calibrated pH meter

Multiple Choice

What is the important step in calibrating a pH Meter?

• Use distilled water for calibration.
• Calibrate using only tap water.
• Use standard buffer solutions for calibration.
• Adjust the meter without buffers.

Multiple Choice

What will happen if the pH Meter is not callibrated?

• Erroneous temperature readings.
• Stable calibration results.
• Inaccurate pH readings.
• Consistent pH measurements.

Multiple Choice

What is the important of buffer system specially in the body?

• Buffer systems are crucial for maintaining stable pH levels in the body.
• Buffer systems are primarily for energy production.
• Buffer systems are only important for digestion.
• Buffer systems help in nutrient absorption in the body.

THINGS TO DO

• GO TO YOUR BREAKOUT ROOM

• READ THE ACTIVITY SHEET

• PERFORM THE ACTIVITY AS A GROUP

• RECORD THE STEP-BY-STEP PROCESS

• ANSWER THE GUIDE QUESTIONS

• SUBMIT THE RECORDINGS AND THE ACTIVITY SHEET BY UPLOADING IT TO YOUR GDRIVE