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WorksheetsBuffer Solution Quiz
Total questions: 72
Worksheet time: 40mins
What is a buffer solution?
A buffer solution is a concentrated solution of a single substance.
A buffer solution is a solution that changes pH drastically when acid or base is added.
A buffer solution is a solution that resists changes in pH when small amounts of acid or base are added to it.
A buffer solution is a solution that has no effect on pH.
Explain the concept of buffer capacity.
Buffer capacity is determined by the ratio of the concentrations of the weak acid and its conjugate base in the solution.
Buffer capacity is influenced by the size of the container.
Buffer capacity is determined by the temperature of the solution.
Buffer capacity is related to the color of the solution.
How does a buffer solution resist changes in pH?
By containing a strong acid and its conjugate base
By having a high concentration of water
By releasing ions into the solution
By containing a weak acid and its conjugate base (or a weak base and its conjugate acid), which react with added acids or bases to minimize pH changes.
What are the components of a buffer solution?
Strong acid and its conjugate base
Salt and water
Weak acid and strong base
Weak acid and its conjugate base, or weak base and its conjugate acid
What is the Henderson-Hasselbalch equation used for?
Solving quadratic equations
Balancing chemical equations
Predicting reaction rates
Calculating the pH of a buffer solution
Discuss the importance of buffer solutions in biological systems.
Buffer solutions are used to increase the pH in biological systems
Buffer solutions are important in biological systems to maintain a stable pH level, resist changes in acidity or alkalinity, and ensure optimal conditions for biochemical reactions.
Buffer solutions have no impact on biochemical reactions
Buffer solutions are only necessary in non-living systems
How can you prepare a buffer solution?
Mix a strong acid and its conjugate base
Dilute a strong base with water
Combine a weak acid and a strong base
Mix a weak acid and its conjugate base or a weak base and its conjugate acid in the desired ratio.
What is the pH range of a buffer solution?
Between 5-10
Exactly at the pKa value
Above 14
Within one unit of the pKa value of the weak acid or base in the buffer
Explain the difference between acidic and alkaline buffer solutions.
Acidic buffer solutions have a pH above 7.
Acidic buffer solutions have a pH below 7 and resist changes in pH when small amounts of acid are added, while alkaline buffer solutions have a pH above 7 and resist changes in pH when small amounts of base are added.
Acidic buffer solutions resist changes in pH when small amounts of base are added.
Alkaline buffer solutions resist changes in pH when small amounts of acid are added.
What are some common examples of buffer solutions?
Nitric acid/sodium nitrate
Acetic acid/sodium acetate, Citric acid/sodium citrate
Hydrochloric acid/sodium chloride
Sulfuric acid/sodium sulfate
Which of the following would be the most effective buffer system for maintaining a solution at pH 9?
Acetic acid (pKa = 4.76) and sodium acetate
Hydrochloric acid (pKa = –6) and sodium hydroxide
Sulfuric acid (pKa = –3) and sodium sulfate
Ammonium hydroxide (pKa = 9.25) and ammonium chloride
A salt bridge _____.
is not necessary in order for the cell to work
acts as a mechanism to allow the mechanical mixing of the solutions
allows change balance to be maintained in the cell
is tightly plugged with firm agar gel through which ions cannot pass
In a reduction reaction, the species that acts as the oxidizing agent _____.
gains electrons
loses electrons
gains protons
loses protons
What is a buffer solution?
A solution with a high concentration of solute.
A solution that resists changes in pH.
A solution that reacts with acids to form salts.
A solution with a low concentration of solute.
What is the oxidation number of oxygen in H₂O₂?
–2
–1
+1
+2
Which of the following species could be a Bronsted–Lowry base?
Cl-
LiOH
Both Cl- and LiOH
Cl- only
Which of the following factors can disrupt the effectiveness of a buffer system?
Adding a strong acid or base in equal amounts to the buffer
Diluting the buffer solution with water
Adding a salt of a strong acid and a strong base to the buffer
Increasing the concentration of the buffer components
Which of the following statements about buffer capacity is correct?
Buffer capacity is independent of the ratio of acid to base.
Buffer capacity increases with increasing concentration of the buffer components.
Buffer capacity is a measure of the amount of acid or base a buffer can neutralize.
Buffer capacity is inversely proportional to the pH of the buffer solution.
Which of the following elements is most likely to act as a reducing agent?
Oxygen (O)
Fluorine (F)
Hydrogen (H)
Chlorine (Cl)
If the pH of a buffer solution is equal to the pKa, what can you conclude about the buffer?
The buffer is not effective and cannot resist pH changes.
The buffer has reached its maximum buffer capacity.
The buffer contains equal concentrations of the weak acid and its conjugate base.
The buffer contains equal concentrations of the strong acid and the strong base.
Which of the following statements is true regarding half–reactions?
The reducing agent is always the reactant in the oxidation half–reaction.
The oxidizing agent is always the product in the reduction half–reaction.
Both half–reactions must have the same number of electrons.
Half–reactions are independent and can occur separately.
Which of the following is not a component of a buffer solution?
Weak acid
Weak base
Salt of a weak acid or base
Strong acid
Which of the following is an example of a redox reaction?
Dissolving sugar in water
Burning of paper
Mixing oil and water
Melting ice
Which of the following relationships is true for an acidic solution?
[H+] > [OH-]
[H+] < [OH-]
pH = 7.00
pH > 7.00
Which of the following pH values represents the optimal range for most biological buffers?
pH 2–3
pH 7–8
pH 4–5
pH 10–11
In an electrolytic cell, the electrode at which the electrons enter the solution is called the _____, and the chemical change that occurs at this electrode is called _____.
anode, oxidation
cathode, oxidation
anode, reduction
cathode, reduction
Which of the following statements is true regarding oxidation?
It involves a gain of electrons
It involves a loss of electrons
It occurs only in acidic solutions
It is not related to the transfer of electrons
Which of the following is an example of an acid-base reaction?
CH4 + 2O2 → CO2 + 2H2O
Cu + 2AgNO3 → 2Ag + Cu (NO3)2
HCl + NaOH → NaCl + H2O
N2 + 2H3 → 2NH3
In the standard notation for a voltaic cell, the double vertical line, ||, represents _____.
a phase boundary
a wire (metal) connection
a gas electrode
a salt bridge
What is the Henderson–Hasselbalch equation used for?
To calculate the molarity of a buffer solution
To determine the pKa of a weak acid or base
To calculate the pH of a buffer solution
To measure the buffer capacity of a solution
How does a buffer solution maintain its pH?
By releasing or accepting protons (H+ ions)
By undergoing a chemical reaction with water
By neutralizing all the acid or base added to it
By diluting the added acid or base
In the electrolytic cell, the flow of electrons is from _____.
cathode to anode in solution
cathode to anode through external supply
anode to cathode through internal supply
cathode to anode through internal supply
Which of the following is true about the oxidation number of an uncombined element?
It is always zero
It is always positive
It is always negative
It depends on the specific element
pH is a measure of _____.
density
H+ concentration
OH- concentration
solute concentration
In the reaction: 2Na + Cl2 → 2NaCl, which species is reduced?
Na
Cl2
NaCl
None of the above
A solution with a pH of 5.0 ______.
has a hydrogen–ion concentration of 5.0 M
has a hydrogen–ion concentration of 1×10−5 M
is basic
is neutral
A solution in which [OH-] exceeds [H+] is said to be _____.
acidic
basic
neutral
salt
In a redox reaction, the species that loses electrons is the _____.
oxidizing agent
reducing agent
reactant
product
Which of the following best defines a redox reaction?
A reaction where atoms are rearranged to form new substances.
A reaction where there is a transfer of electrons between species.
A reaction where energy is released in the form of light.
A reaction where reactants combine to form a single product.
Which of the following will not conduct electricity in aqueous solution?
Copper (II) sulfate
Sugar
Common salt
None of these
pH is a measure of _____.
density
H+ concentration
OH- concentration
solute concentration
In the reaction: 2Na + Cl2 → 2NaCl, which species is reduced?
Na
Cl2
NaCl
None of the above
What is the relationship between [H+] and pH?
As the pH value decreases, the concentration of H+ increases.
As the pH value decreases, the concentration of H+ also decreases.
As the pH value increases, the concentration of H+ also increases.
As the pH value decreases, the concentration of H+ has no significant effect.
A solution in which [OH-] exceeds [H+] is said to be _____.
acidic
basic
neutral
salt
According to Bronsted–Lowry, a base is defined as ______.
An electron pair acceptor
A hydroxide donor
A proton acceptor
A proton donor
A solution with a pH of 7.0 _____.
is acidic
is basic
is moderate
is neutral
Which of the following best defines a redox reaction?
A reaction where atoms are rearranged to form new substances.
A reaction where there is a transfer of electrons between species.
A reaction where energy is released in the form of light.
A reaction where reactants combine to form a single product.
According to Bronsted–Lowry, an acid is defined as ______.
An electron pair acceptor
A hydroxide donor
A proton acceptor
A proton donor
What is the relationship between [H+] and pH?
As the pH value decreases, the concentration of H+ increases.
As the pH value decreases, the concentration of H+ also decreases.
As the pH value increases, the concentration of H+ also increases.
As the pH value decreases, the concentration of H+ has no significant effect.
According to Bronsted–Lowry, a base is defined as ______.
An electron pair acceptor
A hydroxide donor
A proton acceptor
A proton donor
A solution with a pH of 7.0 _____.
is acidic
is basic
is moderate
is neutral
A buffer solution is prepared by mixing equal volumes of 0.1 M acetic acid (pKa = 4.76) and 0.1 M sodium acetate. What is the pH of this buffer solution?
pH 2
pH 4
pH 7
pH 9
According to Bronsted–Lowry, an acid is defined as ______.
An electron pair acceptor
A hydroxide donor
A proton acceptor
A proton donor
A buffer solution is prepared by mixing equal volumes of 0.1 M acetic acid (pKa = 4.76) and 0.1 M sodium acetate. What is the pH of this buffer solution?
pH 2
pH 4
pH 7
pH 9
Which of the following statements ARE TRUE about buffer solution?
(you may choose more than one answer)
pH of buffer solution will never change despite addition of small amount of base or acid
Buffer can be made by mixing weak acid and salt of its conjugate base or by mixing weak base with salt of its conjugate acid
Buffer has acid and base components that can work specifically to resist pH change
the closer the ratio of concentration weak acid/base to the concentration of salt of its conjugate base/acid, the less effective the buffer to resist pH change
What statements CAN BE TRUE about acidic buffer?
(you may choose more than one answer)
It's made of a mixture of weak acid and salt of its conjugate base
Concentration of H+ ions in acidic buffer is greater than concentration of OH- ions which is present in the solution
Dilution of buffer by adding small amount of water doesn't change the pH of buffer solution
acidic buffer usually works effectively at pH range of above 7
What statements CAN BE TRUE about basic buffer?
(you may choose more than one answer)
basic buffer usually works effectively at pH range of above 7
It's made of a mixture of strong base and salt of its conjugate acid
adding small amount of strong acid to the solution of basic buffer can significantly alter the pH of the buffer solution
diluting solution of basic buffer cause pH of that solution to change drastically
Which of the following statements ARE TRUE about buffer solution?
(you may choose more than one answer)
pH of buffer solution will never change despite addition of small amount of base or acid
Buffer can be made by mixing weak acid and salt of its conjugate base or by mixing weak base with salt of its conjugate acid
Buffer has acid and base components that can work specifically to resist pH change
the closer the ratio of concentration weak acid/base to the concentration of salt of its conjugate base/acid, the less effective the buffer to resist pH change
What statements CAN BE TRUE about acidic buffer?
(you may choose more than one answer)
It's made of a mixture of weak acid and salt of its conjugate base
Concentration of H+ ions in acidic buffer is greater than concentration of OH- ions which is present in the solution
Dilution of buffer by adding small amount of water doesn't change the pH of buffer solution
acidic buffer usually works effectively at pH range of above 7
What statements CAN BE TRUE about basic buffer?
(you may choose more than one answer)
basic buffer usually works effectively at pH range of above 7
It's made of a mixture of strong base and salt of its conjugate acid
adding small amount of strong acid to the solution of basic buffer can significantly alter the pH of the buffer solution
diluting solution of basic buffer cause pH of that solution to change drastically
a buffer solution is made of mixture of aqueous methanoic acid, HCOOH, with aqueous sodium methanoate, NaHCOO.
the equilibrium reaction takes place in buffer solution is :
HCOOH ↔ HCOO- + H+
small amount of NaOH is then added to that buffer solution.
What reaction take places at the buffer solution to resist change of pH caused by addition of base?
HCOOH + H+ → HCOOH2
HCOO- + H+ → HCOOH
HCOOH + OH- → HCOO- + H2O
HCOO- + OH- → COO2- + H2O
a buffer solution is made of mixture of aqueous ethanoic acid, CH3COOH, with aqueous potassium ethanoate, KCH3COO.
the equilibrium reaction takes place in buffer solution is :
CH3COOH ↔ CH3COO- + H+
small amount of HCl is then added to that buffer solution.
What reaction take places at the buffer solution to resist change of pH caused by addition of acid?
CH3COO- + H+ → CH3COOH
CH3COO- + OH- → CH2COO2- + H2O
CH3COOH + H+ → CH3COOH2
CH3COOH + OH- → CH3COO- + H2O
Which of the following mixture that may produce buffer solution to work at pH of below 7?
(you may choose more than one answer)
NaOH (in excess) + HCN
KOH + NaCH3COO
HCOOH + NaHCOO
KOH + HF (in excess)
HCOOH + CH3COOH
Which of the following mixture that may produce buffer solution to work at pH of above 7?
(you may choose more than one answer)
HCl + NH3 (in excess)
Mg(OH)2 + HF (in excess)
NaCN + HCN
NH3 + NH4NO3
H2SO4 (in excess) + NH3
Which of the following composition or mixture will, in general, form a solution of acidic buffer ?
(you may choose more than one answer)
strong acid + weak base (in excess)
strong base + weak acid (in excess)
weak acid + salt of its conjugate base
weak base + salt of its conjugate acid
strong acid (in excess) + strong base
Which of the following mixture that won't produce a buffer solution?
(you may choose more than one answer)
LiOH + LiF
HCl (in excess) + KOH
HNO3 (in excess) + NH3
NaOCl + NaOH
CH3COOH + Mg(CH3COO)2
Which of the following composition or mixture will, in general, form a solution of basic buffer ?
(you may choose more than one answer)
strong acid + weak base (in excess)
strong base + weak acid (in excess)
weak acid + salt of its conjugate base
weak base + salt of its conjugate acid
strong acid + strong base (in excess)
a buffer solution is made by mixing HA, a weak acid, with salts containing A- ions.
HA ↔ H+ + A-
a formula that can be used for the calculation of the pH of this buffer solution is
Which one actually take place when small amount of strong acid is added to a buffer solution?
(you may choose more than one answer)
the added acid will react with basic component of the buffer to minimize pH change caused by the former
the pH value of the solution slightly increase
the concentration of basic component and acid component of the buffer slightly decrease and slightly increase, respectively, after a new equilibrium is established
the numerical value of equilibrium constant of equilibirum involved in buffer solution change after addition of acid
Which one actually take place when small amount of strong base is added to a buffer solution?
(you may choose more than one answer)
the pH value of the solution doesn't change after the addition of base
the concentration of H+ ion in solution slightly decrease after the addition of base
the concentration of basic component and acid component of the buffer slightly increase and slightly decrease, respectively, after a new equilibrium is established
the added base is consumed by the acid component of the buffer to minimize pH change caused by the former
One of the buffer in blood plasma is a mixture of dihydrogenphospate ions (H2PO4-) and hydrogen phosphate (HPO42-) ions.
H2PO4- + H2O ↔ HPO42- + H3O+
which of the following pair acts as base-conjugate acid pair?
H2PO4- and HPO42-
H2O and H3O+
H2PO4- and H3O+
H2O and HPO42-
Equilibrium reaction of carbon dioxide (CO2) and hydrogencarbonate (HCO3-) ions in blood is one of the important buffer system that contribute to stabilise pH of the blood
CO2(aq) + H2O(l) ↔ H+(aq) + HCO3-
Which one take place on the buffer system when blood are slightly acidic than it would be normally ?
equilibrium of the buffer system shifts to the right
more hydrogencarbonate (HCO3-) ions are consumed in reaction with excess acid to produce more dissolved CO2
more dissolved CO2 are consumed from the blood to remove excess acid and produce more hydrogencarbonate (HCO3-) ions
No shift of the equilibrium take place on the buffer system
