If equal moles of acid and base react in a neutralization reaction, they cancel out many of each other's properties.

TRUE ------
FALSE

A neutral salt is formed by which type of reaction?

strong acid-weak base
strong acid-strong base
weak acid-strong base------
weak acid-weak base


Which could be the original acid and base that react to produce the salt KCl?

KOH and HCl-------
KBr and H2O
HClO4 and K2O
NaCl and KCl


Net ionic equations for strong acid-strong base reactions are always: H+ (aq) + OH−(aq Imported Asset H2O (l).

TRUE------
FALSE


Which net ionic equation best represents a weak acid-strong base reaction?

H3BO3 (aq) Imported Asset BO3− (aq) + H2O (l)---------
2 OH− (aq) Imported Asset H2O (l)
H3BO3 (aq) + OH− (aq) Imported Asset BO3− (aq) + H2O (l)
H3BO3 (aq) + KOH (aq) Imported Asset KBO3 (aq) + H2O (l)


The equation, H2SO4 (aq) + Sr(OH)2 (aq) Imported Asset SrSO4 (aq) + H2O (l), represents:

overall equation for a strong acid-weak base neutralization reaction
overall equation for a strong acid-strong base neutralization reaction--------
net ionic equation for a weak acid-weak base reaction
net ionic equation for a weak base-strong acid reaction


When choosing which indicator to use in a titration reaction, you should consider:

what color you would like to see at the end point of the titration
the relative strengths of the acid and base you are using in the titration
how long the titration will take to complete--------
adjusting the end point of the titration to better match your indicator


When a small amount of acid is added to a buffer, the weak base form of the buffer is converted to:

its weak conjugate acid form
its strong conjugate acid form
its strong conjugate base form------
an even weaker base form

Buffers are systems that resist changes in pH by converting strong acids or bases to weak acids or bases.

TRUE-------
FALSE