In this experiment, all the acid added is neutralized by
an antacid and sodium hydroxide
In reading a buret, you should always
read the bottom of the meniscus
The purpose of Trial T is
to get an idea of the expected end-point and the amount of HCl to add in subsequent trials
When you react hydrochloric acid and sodium hydroxide you get
a salt and water
An antacid tablet was dissolved in water and 10mL of 0.16M HCl was
added. After the acid had reacted with the tablet it required 40mL of
0.02M NaOH to neutralize the HCl that remained.
How many moles of HCl were initially added to the antacid?
1.6x10-3
An antacid tablet was dissolved in water and 10mL of 0.16M HCl was
added. After the acid had reacted with the tablet it required 40mL of
0.02M NaOH to neutralize the HCl that remained.
How many moles of NaOH were required to neutralize the HCl
that remained after it had reacted with the tablet?
8.0x10-4
To determine the number of moles of acid that were initially added to the Erlenmeyer
multiply the molarity of the HCl by the volume in Liters of HCl added
How is the number of moles of acid neutralized by the antacid determined in this experiment
moles of acid added - moles of acid remaining
When the phenolphthalein changes color, then
the amount of NaOH added is just sufficient to react with all the acid present
In this experiment what do you use to dispense the acid into the Erlenmeyer flask
a repipet
The reaction:
HCl(aq) + NaOH(aq) = NaCl(aq) +
H2O(l)
is an example of a(n)
acid-base reaction
When the following chemical equation is balanced:
__Mg(OH)2(s) + __HCl(aq) = __MgCl2(aq) +
__H2O(l)
The stoichiometric co-efficients are:
1 2 1 2
The purpose of this experiment is to
determine the number of moles of acid neutralized by an antacid tablet
back titration is used in this experiment. This is because
many antacids contain more than one active ingredient
When the tablet has reacted completely with the acid
some inert binder will remain in the flask and the solution may be cloudy
An antacid tablet was dissolved in water and 10mL of 0.16M HCl was
added. After the acid had reacted with the tablet it required 40mL of
0.02M NaOH to neutralize the HCl that remained.
How many grams of HCl (Molar Mass = 36.5 g/mol) did the
antacid neutralize?
0.029
Which of the following is not a common active ingredient in commercial antacids
NaOH
What is the approximate molarity of the HCl used in this experiment
1M
An antacid tablet was dissolved in water and 10mL of 0.16M HCl was added. After the acid had reacted with the tablet it required 40mL of 0.02M NaOH to neutralize the HCl that remained
How many moles of HCl did the antacid neutralize
8.0x10-4
If during Trial P, upon addition of only a few mL of NaOH the indicator changes color you should
add more HCl, reheat, and continue with the titration