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13 Dec 2019

pH Shift

Unbuffered Buffered

Acid added to acidicsolutions: Solution 2: -2 Solution 5: 0

Base added to acidicsolutions Solution 2: 0 Solution 5: 0

Acid added to basicsolutions Solution 3: 0 Solution 6: 0

Base added to basicsolutions Solution 3: +2 Solution 6: 0

Acid added to nearly neutral solutions Solution1: -1 Solution 4: 0

Base added to nearly neutral solutions Solution 1: +1 Solution 4: 0

1. Which of the unbuffered solutions, 1,2 or 3, was the mostsubject to pH change? Explain why.

2. What concluding statement can you make, on the basis of yourobservations regarding the fluctuations in pH for buffered andunbuffered solutions when small amounts of acid and base areadded?

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Related questions

ACID-BASE NEUTRALIZATION REACTIONS. In this lab, we were given several vials which each contained 5 mL of NaOH solution with a pH level of 9. We then added 1 mL of various HCl solutions with varying pH's to these vials.

Vial #1: 5 mL pH 9 NaOH solution
Vial #2: 5 mL pH 9 NaOH solution + 1 mL pH 13 HCl solution = 6 mL pH 12.13 solution
Vial #3: 5 mL pH 9 NaOH solution + 1 mL pH 11 HCl solution = 6 mL pH 3.12 solution
Vial #4: 5 mL pH 9 NaOH solution + 1 mL pH 5 HCl solution = 6 mL pH 6.55 solution
Vial #5: 5 mL pH 9 NaOH solution + 1 mL pH 3 HCl solution = 6 mL pH 6.95 solution
Vial #6: 5 mL pH 9 NaOH solution + 1 mL pH 1 HCl solution = 6 mL pH 1.81 solution

We're working with the chemical equation: HCl + NaOH <--> H2O + NaCl
Net Ionic chemical equation: H+ + OH- = H2O

Q) Calculate the number of moles of either OH- or H3O+ in the solution that was added (OH- if the solution was a base or H3O+ if the solution was an acid).


QUESTION 1

Which of the following substances is most acidic?

Cowรขย€ย™s milk - pH 6.6

Apple juice - pH 3.0

Tomato juice - pH 4.5

Distilled water - pH 7.0

2 points

QUESTION 2

A buffer is a substance that converts:

Alkaline solutions to neutral solutions.

Acidic solutions to alkaline solutions.

Strong bases or acids to weak bases or acids.

Acidic solutions to neutral solutions.

QUESTION 3

How does a solution of pH 7 compare to a solution of pH 10?

pH 7 has more OH- ions

pH 7 is more basic

pH 7 has a higher pH

pH 7 has more H+ ions

2 points

QUESTION 4

According to the Arrhenius Theory of acids and bases, a base is:

A substance that decrease the amount of hydroxide ions present.

A substance that increases the amount of hydroxide ions present when it is dissolved in water.

A substance that increase the amount of hydrogen ions present.

A substance that increases the amount of hydrogen ions present when it is dissolved in water.

QUESTION 5

Which of the following are true regarding acid-base titrations?

They are used to determine the concentration of an unknown acid or base.

The acid or the base must be a standard solution with a known concentration

The standard solution is titrated into the chemical with the unknown concentration.

All of the above are true regarding acid-base titrations.

2 points

QUESTION 6

Which of the following is not an example of a neutralization reaction?

HCl + NaOH NaCl +H2O

2 NaOH + H2CO3 Na2CO3 +2 H2O

H2SO4 + 2 NH4OH (NH4)2SO4 + 2 H2O

2 AgNO3 + Zn 2Ag +Zn(NO3)2

QUESTION 7

Which acid base theory defines an acid as a proton donor and a base as a proton acceptor?

Arrhenius Theory

Bronsted-Lowery Theory

Conjugate Pairs Theory

Lewis Theory

2 points

QUESTION 8

The Arrhenius Theory states that acid-base reactions create a solution composed of a water and a salt. This is because mixing an acidic and basic solution together yields:

A neutral solution

A solution with a pH at or near 7

Both A and B are correct

QUESTION 9

Which of the following correctly defines a standard solution?

A solution which always has the same molecular geometry.

A solution in which the concentration is precisely known.

A solution in which the volume is precisely known.

A solution which always has different levels of solutes and solvents.

2 points

QUESTION 10

Acids naturally present in food are generally safe to eat because they are usually:

Concentrated

Dilute

Weak

Strong

None of the above are correct

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