Quiz on unit 8 must knows

#1 Which of the following terms matches the definition?

14 always!!

H2O pH is always... pH + pOH = weak acid-strong base reaction what is a buffer

#2 Which of the following terms matches the definition?

if weak base is in excess --> a buffer --> Hendeson Hasselbalch equaiton if strong acid is in excess, the moles of excess acid are used to determine pH if acid and base are equimolar then the equilibrium concentrations are used to determine pH

in what range are buffers effective strong acid-weak base reaction strong acid-weak base reaction maximum buffering capacity

#3 Which of the following terms matches the definition?

increasing/decreasing concentrations of buffer components, but keeping the ratios constant (if you don't it'll change the buffer capacity for either acid or base respectively)

Kw = strong acid-weak base reaction maximum buffering capacity how to increase/decrease buffering capacity

#4 Which of the following terms matches the definition?

HA(aq) + OH- --> A-(aq) + H2O(L) if weak acid is in excess --> a buffer --> Hendeson Hasselbalch equaiton if strong base is in excess, the moles of excess hydroxide ions is used for pH if acid and base are equimolar then the equilibrium concentr

maximum buffering capacity in what range are buffers effective weak acid-strong base reaction weak acid-strong base reaction

#5 Which of the following definitions matches the term?

maximum buffering capacity

1.0 x 10^-14 at 25 C or 298 K if weak base is in excess --> a buffer --> Hendeson Hasselbalch equaiton if strong acid is in excess, the moles of excess acid are used to determine pH if acid and base are equimolar then the equilibrium concentrations are used to determine pH pH = pKa + log [A-]/[HA] ---> acids pOH = pKb + log [BH+]/[B] ---> bases the conjugate salt is on top, and the bottom is either the base or the acid assume there is a limiting and excess reagent (because it will contain either a strong acid or base) pH = pKa

#6 Determine if the following combination is true or false.

strong acid strong base equivalence point

pH = 7 @ 25 C / 298 K

True

False

#7 Determine if the following combination is true or false.

how do you calculate a buffer's pH

pH = pKa + log [A-]/[HA] ---> acids pOH = pKb + log [BH+]/[B] ---> bases the conjugate salt is on top, and the bottom is either the base or the acid assume there is a limiting and excess reagent (because it will contain either a strong acid or base)

True

False

#8 Determine if the following combination is true or false.

in what range are buffers effective

1.0 x 10^-14 at 25 C or 298 K

True

False

#9 Determine if the following combination is true or false.

what is a buffer

HA(aq) + OH- --> A-(aq) + H2O(L) if weak acid is in excess --> a buffer --> Hendeson Hasselbalch equaiton if strong base is in excess, the moles of excess hydroxide ions is used for pH if acid and base are equimolar then the equilibrium concentr

True

False

#10 Determine if the following combination is true or false.

H2O pH is always...

7, could be acid (pH) or base (pOH)

True

False

Section 1: Multiple Choice questions

14 always!!

if weak base is in excess --> a buffer --> Hendeson Hasselbalch equaiton if strong acid is in excess, the moles of excess acid are used to determine pH if acid and base are equimolar then the equilibrium concentrations are used to determine pH

increasing/decreasing concentrations of buffer components, but keeping the ratios constant (if you don't it'll change the buffer capacity for either acid or base respectively)

HA(aq) + OH- --> A-(aq) + H2O(L) if weak acid is in excess --> a buffer --> Hendeson Hasselbalch equaiton if strong base is in excess, the moles of excess hydroxide ions is used for pH if acid and base are equimolar then the equilibrium concentr

maximum buffering capacity

Section 2: True/false questions

strong acid strong base equivalence point

pH = 7 @ 25 C / 298 K

how do you calculate a buffer's pH

pH = pKa + log [A-]/[HA] ---> acids pOH = pKb + log [BH+]/[B] ---> bases the conjugate salt is on top, and the bottom is either the base or the acid assume there is a limiting and excess reagent (because it will contain either a strong acid or base)

in what range are buffers effective

1.0 x 10^-14 at 25 C or 298 K

what is a buffer

HA(aq) + OH- --> A-(aq) + H2O(L) if weak acid is in excess --> a buffer --> Hendeson Hasselbalch equaiton if strong base is in excess, the moles of excess hydroxide ions is used for pH if acid and base are equimolar then the equilibrium concentr

H2O pH is always...

7, could be acid (pH) or base (pOH)

Triple-checked your answers?

Quiz menu