If a VOLUME is mentioned and the problem involves molarity DO NOT assume that 224L should be used STP is only used when it says STP in the question and the substance is a GAS IMPORTANT ID: 465482
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Slide1
Solution Stoichiometry Slide2
If a VOLUME is mentioned, and the problem involves molarity DO NOT assume that 22.4L should be used. STP is only used when it says STP in the question and the substance is a GAS!
IMPORTANT!Slide3
Solutions of ammonia and phosphoric acid are used to produce ammonium hydrogen phosphate fertilizer. What volume of 14.8mol/L ammonia is needed to react completely with 1.00L of 12.9mol/L phospheric acid to produce fertilizer?
Example 1Slide4
A technician determines the amount concentration of sulfuric acid solution. In the experiment, 10.00mL of sulfuric acid reacts completely with 15.9mL of 0.150M potassium hydroxide. Calculate the concentrations of sulfuric acid.
Example 2Slide5
A titration is a process in which a measured amount of a solution is reacted with a known volume of another solution (one with an unknown concentration) until a desired equivalence point is reached
TitrationsSlide6
The equivalence point is the point in a titration where the ratio of the moles of each species involved exactly equals the ratio of the coefficients of the species in the balanced reaction equation.
Equivalence PointSlide7
Assume a beaker contains 0.0250L of
H2SO4. A graduated tube (burette) is used to slowly add
NaOH
solution. At the instant that
15.6mL
of the 3.2M
NaOH
has been added, that is, the equivalence point has been reached, the titration process is stopped.
Example 4Slide8
Consider the reaction between phosphoric acid and potassium hydroxide. Complete the chart provided
Example 5
Trial
1
Trial 2
Trial
3
Trial 4
Initial
Burette reading (mL)
0.00mL
21.2mL
0.15mL
19.85mL
Final
Burette reading (mL)
21.2mL
41.1mL
19.85mL
39.6mL
Change in Volume (mL)
Color Change
Bright
Yellow
Dark Yellow
Dark Yellow
Dark Yellow
Average Volume of Titrant