Quiz on unit 8 must knows

#1 Which of the following definitions matches the term?

pH + pOH =

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 14 always!! pH = 7 @ 25 C / 298 K

#2 Which of the following definitions matches the term?

strong acid-weak base reaction

7, could be acid (pH) or base (pOH) within 1 pH of its pKa, up or down 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) 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

#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 = how to increase/decrease buffering capacity weak acid-strong base reaction how do you calculate a buffer's pH

#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

weak acid-strong base reaction pH + pOH = H2O pH is always... how to increase/decrease buffering capacity

#5 Which of the following terms matches the definition?

True

False

Section 1: Multiple Choice questions

pH + pOH =

strong acid-weak base reaction

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

pH = pKa

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

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)

in what range are buffers effective

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

what is a buffer

solution that is resistant to a small pH change, it has to contain a weak acid or base pared with its conjugate salt(Na+, H3O-, etc...) and it creates neutral compounds, keeping pH relatively stable

H2O pH is always...

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

Triple-checked your answers?

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