State if acid or base was present in the final mixed solution in Part B and...
State if acid or base was present in the final mixed solution in Part B and show a sample calculation supporting your conclusion: 6 mL of 3.0 M HCL and 4 mL of 3.0 M NaOH
Homework Answers
Neutralization reaction is
HCl + NaOH ............> NaCl + H2O
one mole NaOH is neutralized by one mole HCl.
we have
6 mL of 3.0 M HCL and 4 mL of 3.0 M NaOH.
thus
moles of HCl = volume of solution in L * molarity = 0.006 L * 3.0 mole / L = 0.018 mole HCl
and
moles of NaOH = volume of solution in L * molarity = 0.004 L * 3.0 mole / L = 0.012 mole
thus
excess HCl = (0.018 - 0.012) = 0.006 mole.
thus
acid was present in the final mixed solution.
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State if acid or base was present in the final mixed solution in
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Page 1 is just instruction for Page 2
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Determine how many liters (l) of stock HCl were used
in titration #1.
Please fill all questions under "Data Analysis"
Page 1 is just instruction for Page 2
EXPT 10: TITRATION OF STRONG ACID WITH STRONG BASE Note to Students: when you see the symbol (), this means there is something you must add into the mock data yourself. You may handwrite or type your answers directly on these pages for submission to a Blackboard link. Remember to show all...
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